Monday
April 21, 2014

Search: It takes 412 kJ/mol to break a carbon-hydrogen single bond

Number of results: 17,565

AP Chem
The energy change H associated with the reaction NBr3(g) + 3H2O(g) -> 3HOBr(g) + NH3(g) is +81 kJ/mol rxn. These bond energy values might be useful: O-H 459 kJ/mol; N-H 386 kJ/mol; O-Br 201 kJ/mol. The strength of the N Br bond is 1. 4 kJ/mol 2. 465 kJ/mol 3. 66 kJ/mol 4. ...
Sunday, November 7, 2010 at 4:31pm by Beth

CHEMISTRY
METHANOL=-3.92 KJ/MOL -132.788 KJ/MOL ETHANOL=-33.112 KJ/MOL -338.542 PROPANOL -783.176 KJ/MOL -443.471 KJ/MOL BUTANOL= -259 KJ/MOL - 625.812 PARAFFIN= -4603.571 KJ/MOL 5183.571 KJ/MOL
Monday, April 16, 2012 at 1:47pm by JGU

ap chemistry
Carbon monoxide reacts with oxygen to form carbon dioxide by the following reaction: 2CO2 + O2 yields 2CO2 Delta H for this reaction is -566 kJ/mol run. What is the delta H for CO? 1). +270 kJ/mol 2). -110 kJ/mol 3). +65 kJ/mol 4). -405 kJ/mol 5). -65 kJ/mol 6). -182 kJ/mol 7...
Thursday, October 18, 2012 at 11:43pm by bridget

ap chem
calculate the lattice enthalpy of potassium fluoride from the following data: enthalpy of formation of K(g): +89 kJ mol−1 first ionization energy of K(g): +418 kJ mol−1 enthalpy of formation of F(g): +79 kJ mol−1 electron affinity of F(g): +328 (H = &#...
Tuesday, July 13, 2010 at 1:57am by alexandra

Chemistry
Predict whether the following reactions will be exothermic or endothermic A) N2(g)+ 3H2(g) --> 2NH3(g) B) S(g) +O2(g) ---> SO2(g) C) 2H2O(g) ---->2H2(g) + O2(g) D) 2F(g) +F2(g) Bond H-H 432 kj/mol N-N(triple bond) 942 kj/mol O=O 494 KJ/Mol F-F 155 KJ/mol H-N 386 KJ/...
Sunday, January 22, 2012 at 10:53pm by Kristen

chemistry
Balanced equation NH3(g) + HCl(G) --> NH4Cl deltaH = (1 mol)(-314.4 kJ/mol) - (1 mol)(-45.9 kJ/mol) plus (1 mol)(-92.3 kJ/mol) =-176.2 kJ deltas = (1 mol)(94.6) - (1 mol)(192.78) plus (1 mol)(-186.90) = 0.00588 DG = DH - TDS =176.2 kJ / 0.00588 =29995
Sunday, April 6, 2008 at 6:15pm by Sarah

CHemistry Dr. Bob please?
for bond energies if tehy give u a diagram of the structure for whatever like c--h--o==h or soemthing amd a chart with c--h=-670 Kj /mol or whatever do u just add all of the KJ/mol together? but what if they only want kJ? would you just multply whatever kJ/mol *1 mol?? how do ...
Tuesday, November 11, 2008 at 5:16pm by Robin

chemistry
If 3 moles of a compound use 12 J of energy in a reaction, what is the Hreaction in kJ/mol? A. -4 kJ/mol B. -0.004 kJ/mol C. 0.004 kJ/mol D. 4 kJ/mol
Wednesday, March 14, 2012 at 2:56pm by princess

chemistry
A 79.9-L sample of a gaseous hydrocarbon, measured at 1.00 atm pressure and 25.0C, is burned in excess oxygen, liberating 4.24 10^3 kJ of heat at constant pressure. What is the identity of the hydrocarbon? (R = 0.0821 L atm/(K mol)) Substance Hf (kJ/mol) CO2(g) 393.5 ...
Wednesday, March 30, 2011 at 12:09am by chemistry

Chemistry
C6H14 + 19/2 O2 -> 6 CO2 + 7H2O delta H = -4163 kJ What mass of hexane is required to produce 1.0E5 kJ of heat by complete combustion? -4163 kJ/mol x mol C6H14 = 1E5/-4163 kJ/mol Mol = 1E5/-4163 kJ/mol Mol = -24 mol I know I can do m=n x MM now, but shouldn't the value of ...
Monday, February 11, 2013 at 6:51pm by A Canadian

CHEM:
The bond enthalpy of the Br−Cl bond is equal to H for the reaction BrCl(g) Br(g) + Cl(g). Use the following data to find the bond enthalpy of the Br−Cl bond. Br2(l)--->Br2(g) H=30.91 KJ/mol Br2(g)--->2Br2(g) H=192.9 KJ/mol Cl2(g)---->2Cl(g) H=...
Wednesday, June 6, 2012 at 3:13pm by April

Chemistry
"Given that the bond enthalpy of the carbon-oxygen bonds in carbon monoxide and carbon dioxide are 1073 kJ/mol and 743 kJ/mol respectively, and that of the bond in the oxygen molecule is 496 kJ/mol, calculate the enthalpy change for the combustion of 1 mole of carbon monoxide...
Thursday, April 8, 2010 at 10:54pm by Stuck

Chemistry
See if this sounds reasonable to you. moles CaCl2 = 11.11/110.98 = 0.1 mole Ca = 0.1 mol Cl = 0.2 mol Ca = 543 kJ/mol x 0.1 mol = -54.3 kJ. Cl = 167 kJ/mol x 0.2 mol = -33.4 kJ. Total released = sum of the two.
Thursday, March 4, 2010 at 11:00pm by DrBob222

CHEMISTRY
Calculate the H rxn for the following reaction. H f [H2S(g)] = -21 kJ/mol; H f [SO2(g)] = -297 kJ/mol; H f [H2O(l)] = -285.8 kJ/mol; 2H2S(g) + SO2(g) 3S(s) + 2H2O(l) a. 232.6 kJ b. 910 kJ c. -232.6 kJ d. -910 kJ
Sunday, August 22, 2010 at 12:15am by Lucinda

CHEMISTRY> HELP QUICK! pls
Calculate the reaction free energy of: H2(g) + I2(g) 2HI(g) when the concentrations are 0.026 mol L-1 (H2), 0.33 mol L-1 (I2), and 1.84 mol L-1 (HI), and the temperature is 700K. For this reaction Kc= 54 at 700 K. +11.6 kJ mol-1 0 kJ mol-1 -11.6 kJ mol-1 +2273 kJ mol-
Sunday, September 5, 2010 at 7:45am by Lucinda

Chemistry-Thermochemistry (grade 12)
Awesome I am defiantly starting to understand this stuff better. .065L x (.600 mol/L) = 0.0390 mol q=MC(delta T) = 149g x 4.184 J/g(C) x 3.5 celsius = 2181.9 J =2.2 kJ Then I did 2.2 kJ / 0.0390 mol = 56 kJ/mol for my final answer I got 56 kJ/mol
Thursday, February 16, 2012 at 1:06am by Rose Bud

AP Chem
What energy change is associated with the reaction to obtain one mole of H2 from one mole of water vapor? The balanced equation is 2 H2O(g) -> 2 H2(g) + O2(g)and the relevant bond energies are H-H : 436 kJ/mol; H-O : 467 kJ/mol; O-O : 146 kJ/mol; O=O : 498 kJ/mol. 1. +249 ...
Monday, November 15, 2010 at 11:27am by Kai

AP Chem
What energy change is associated with the reaction to obtain one mole of H2 from one mole of water vapor? The balanced equation is 2 H2O(g) -> 2 H2(g) + O2(g)and the relevant bond energies are H-H : 436 kJ/mol; H-O : 467 kJ/mol; O-O : 146 kJ/mol; O=O : 498 kJ/mol. 1. +249 ...
Monday, November 15, 2010 at 5:21pm by Kai

Chemistry
2CH3CH2CH2OH(l)+9O2(g)→6CO2(g)+8H2O(g) I have to find the delta G delta G of CH3CH2CH2OH(l)=−360.5 KJ/Mol delta G of O2(g)=0 KJ/Mol delta G of CO2(g)=−394.4 KJ/Mol delta G of H20(g)=−228.6 KJ/Mol I keep getting -3426.2 KJ/Mol but its not correct.
Friday, June 21, 2013 at 1:44pm by dave

CHemistry Dr. Bob please?
Yes, you calculate kJ/mol when you do this. If you want kJ per half mole, then multiply by 1/2 and that gives you kJ for whatever problem you are solving. However, it will ALWAYS be kJ/something; i.e., kJ/mol, kJ/g, kJ/500 mg or what have you. If you want to type in your ...
Tuesday, November 11, 2008 at 5:16pm by DrBob222

Chemistry
36913.6 J/g * 114g/mol= -4208150.4J/mol and to convert that to kJ= -4208150400 kJ/mol. the correct answer is -5116 kJ/mol
Friday, October 9, 2009 at 12:29pm by Sindy

Chemistry
What is the lattice energy of NaI? Use the given information below. Heat of formation for NaI = -288.0 kJ/mol Heat of sublimation for Na = 107.3 kJ/mol Ionization energy for Na = 496.0 kJ/mol Bond dissociation energy for I2 = 149 kJ/mol Electron affinity of I = -295.0 kJ/mol ...
Friday, November 22, 2013 at 1:05pm by Andy

chemistry
What is the lattice energy of NaBr? heat of formation of NaBr = -362 kJ/mol heat of sublimation for Na = 107.30 kJ/mol ionization energy for Na = 496 kJ/mol bond dissociation energy for Br2 = 190 kJ/mol electron affinity of Br = -325 kJ/mol heat of vaporization for Br2 = 30.90...
Saturday, December 4, 2010 at 8:57pm by chemistry

Chem Question (thermo)
Calculate ΔG at 25 C for a reaction in which Ca2+(aq) combines with CO32(aq) to form a precipitate of CaCO3(s) if the concentrations of Ca2+(aq) and CO32(aq) are 0.023 M and 0.13 M, respectively. (ΔG = 47.94 kJ) A. 62.3 kJ/mol B. 33.5 kJ/mol C. 17.8 kJ/mol D...
Thursday, March 1, 2012 at 6:21pm by M

chemistry
2Al + Fe2O3 ==> 2Fe + Al2O3 You must know the delta H of the reaction. Make sure it is kJ/rxn and not kJ/mol. It takes 27 x 2 = 54 g Al to produce the kJ for delta Hrxn. 54 g Al x (360 kJ/deltaHrxn) = g Al required. g Fe2O3 required = g Al x (1 mol Fe2O3/2 mol Al) = g Al x...
Tuesday, April 13, 2010 at 2:15pm by DrBob222

chemistry:)
The bond enthalpy of the BrCl bond is equal to DH for the reaction BrCl(g)-> Br(g) + Cl(g). Use the following data to find the bond enthalpy of the BrCl bond. Br2(l)--->Br2(g) H=30.91 KJ/mol Br2(g)--->2Br2(g) H=192.9 KJ/mol Cl2(g)---->2Cl(g) H=243.4 KJ/mol ...
Wednesday, June 6, 2012 at 3:22pm by April

chemistry:)
The bond enthalpy of the BrCl bond is equal to DH for the reaction BrCl(g)-> Br(g) + Cl(g). Use the following data to find the bond enthalpy of the BrCl bond. Br2(l)--->Br2(g) H=30.91 KJ/mol Br2(g)--->2Br2(g) H=192.9 KJ/mol Cl2(g)---->2Cl(g) H=243.4 KJ/mol ...
Saturday, June 9, 2012 at 8:28am by April

CHEM- KINETICS
Dinitrogen tetraoxide, N2O4, decomposes to nitrogen dioxide, NO2, in a first-order process. If k = 2.5 x 103 s-1 at -5 Cand k = 3.5 x 104 s-1 at 25 C, what is the activation energy for the decomposition? 0.73 kJ/mol 58 kJ/mol 140 kJ/mol 580 kJ/mol I am having massive ...
Saturday, September 25, 2010 at 10:04pm by lucylu

Chemistry
For a particular reaction at 195.1 C, ΔG = -1488.09 kJ/mol, and ΔS = 288.67 J/(molK).? Calculate ΔG for this reaction at -20.0 C. delta G = delta H - (T*delta S) -1488.09 kJ/mol = (delta H) - ((461.8K)*(+288.67 J/(mol x K))*(1 kJ/1000 J)) -1488.09 kJ/mol = (...
Tuesday, April 30, 2013 at 4:01pm by Dee

ap chemistry
Propane (C3H8) is burned in oxygen to pro- duce carbon dioxide and water. The heat of combustion of propane is -2012 kJ/mole. How much heat is given off when 3.0 mol C3H8 are reacted with 10.0 mol O2? 1. 4024 kJ 2. 2012 kJ 3. 916 kJ 4. 1555 kJ 5. 5122 kJ 6. 672 kJ 7. 6036 kJ 8...
Wednesday, October 31, 2012 at 5:52pm by cheri

Chemistry
Not quite. 6.01 kJ/mol x 3.50 mol = ?? Note that your arrangement gives kJ/mol; my arrangement the mol cancel to give kJ as the answer and that is the quantity of heat.
Sunday, May 16, 2010 at 6:13pm by DrBob222

chemistry
calculate the lattice energy of sodium oxide (Na2O) from the following data: Ionization energy of Na(g): 495 kJ/mol Electron affinity of O2 for 2e: 603 kJ/mol Energy to vaporize Na(s): 109 kJ/mol O2(g) bond energy: 499 kJ/mol Energy change for the reaction 2Na(s)+ 1/2 O2(g)--&...
Friday, September 14, 2012 at 7:46pm by Meeeee

chemistry
it has been a while since ive done these so i just need a refresher. im looking for the heat of hydration of lithium chloride and sodium chloride. compound Lattice Energy deltaH soln LiCl -834 kj/mol -37.0 kj/mol NaCl -769 kj/mol +3.88 kj/mol what is delta H hydration?
Tuesday, September 18, 2012 at 9:46pm by michelle

chem
it has been a while since ive done these so i just need a refresher. im looking for the heat of hydration of lithium chloride and sodium chloride. compound Lattice Energy deltaH soln LiCl -834 kj/mol -37.0 kj/mol NaCl -769 kj/mol +3.88 kj/mol what is delta H hydration?
Tuesday, September 18, 2012 at 10:59pm by michelle

Chemistry
Sorry, I didnt realize that data didnt attach...here it is..thank you for all your help! Substance ∆Gf C6H6 (l) 124.50 kJ/mol C6H6 (g) 129.66 kJ/mol CCl4 (l) -65.21 kJ/mol CCl4 (g) -60.59 kJ/mol
Wednesday, December 7, 2011 at 1:17pm by Minx

chemistry
This was a multiple choice question, with possible answers of -13.1 KJ/mol; -6.26 KJ/mol; -27.8 KJ/mol; or -26.2 KJ/mol. I was confused as to how to set equation but now I'm confused because if I'm doing this right-none of these answers work. Thanks!
Sunday, March 27, 2011 at 12:21pm by carla

Chem
The information below shows properties of aluminum (Al). DELTAHfus = 10.07 kJ/mol DELTAHvap = 225 kJ/mol Which quantity of heat is required to melt a 342.9-g sample of Al? 127.98 kJ 214.93 kJ 2,851.95 kJ 3,453.00 kJ
Tuesday, April 15, 2014 at 7:55am by Kiley

Thermochemistry
a. Enthalpy for the reaction is 434 kJ and that is for 16 g CH4 (1 mol). So 434 x 1.2/1 = ? or you can do 1.2 mol CH4 = 1.2*16 = 19.2 and 434 kJ x 19.2/16 = ? b. dHf for 1 mol = 826 kJ; therefore, dH rxn as written is 826/mol x 2 mol = 1652 kJ. 1652 kJ x (30g/4*atomic mass Fe...
Tuesday, March 19, 2013 at 10:44pm by DrBob222

chemistry
I've tried, I thought, all of the combinations and I can't come up with 8722.2. It would have helped if you had put units on your answer. DG = DH - TDS DG = -19.2 kJ/mol -(315)(0.261 kJ/mol) DG = -19.2 kJ/mol - 82.215 = -101.4 kJ/mol Check my work.
Tuesday, October 25, 2011 at 9:31pm by DrBob222

Chemistry
S + O2 ==> SO2 delta H is =-296 WHAT. joules, kJ, kJ/mole, ?? I assume -296 kJ/mol. The second question is what is a mol? Is that S or S8? So it is exothermic and gives off 296 kJ/1 mol, how much is given off by just 0.500 mol? how much by 0.520 mol?
Tuesday, March 23, 2010 at 2:15pm by DrBob222

Chemistry
I need help I can't seem to get the right answer. Please help! 1/2 H_2 (g) + 1/2 Cl_2 (g) --> HCl (g) -92.3 kJ/mol Na(s) + 1/2 O_2(g) + 1/2H_2(g) --> NaOH(s) -426.8 kJ/mol NaCl(s) --> Na(s) + 1/2Cl_2(g) 411.1 kJ/mol H_2O(l) -->H_2(g) + 1/2O_2(g) 285.8 kJ/mol HCl(g...
Friday, November 8, 2013 at 9:22pm by Alex

chemistry
Calculate the DHof for the following reaction under standard state conditions: 2 Ag2S(s) + 2 H2O(l) ---> 4 Ag(s) + 2 H2S(g) + O2(g) Given the following information: Ag2S(s) Hof = -32.6 kJ/mol H2O(l) Hof = -285.83 kJ/mol H2S(g) Hof = -20.6 kJ/mol Question options: 309.8...
Sunday, March 9, 2014 at 9:51am by Josh

Chemistry LAB 1
Is this a made up problem? You reported J/mol and the problem asks for kJ/mol. Since the reaction is exothermic your prof may want the negative sign included also. dH = -6649 J/5 mol = -1329.8 J/mol or -1.3298 kJ/mol and since you are limited to 3 significant figures I would ...
Wednesday, November 6, 2013 at 12:02pm by DrBob222

Plz someone Chem Urgent Help
The overall energy involved in the formation of CsCl from Cs(s) and Cl2 (g)is - 443 kj/mol. Given the following information: heat of sublimation for Cs is +76 kj/mol, bond dissociation energy for Cl2is +121 kj/mol, E(11) for Cs is +376 kj/mol, and E(a) for Cl2is 349 kj/...
Friday, January 16, 2009 at 9:06pm by Samenia

Chemistry help (DrBob222)
You don't have to use grams and you CAN use mols. I don't and the reason I don't use mols is it keeps me from making a mistake. The equation tells you that you get 2012 kJ/5 mols O2 or 2012 kJ/1 mol C3H8. (and this is where I make my mistake---I am want to reason that since it...
Tuesday, October 15, 2013 at 9:11pm by DrBob222

Chemistry
I cant figure out how to do a table :( Use the data given to calculate the value of delta G rxn for the reaction at 25C 2C(graphite)+H2(g)--->C2H2(g) C= S(J K^-1) => 5.74 and delta H(kJ/mol)=>0 H2= S(J K^-1)=> 130.68 and delta H (kJ/mol)=>0 C2H2= S(J K^-1)=> ...
Thursday, December 2, 2010 at 8:06pm by Liliy

Chemistry
Re-read the problem. Looks like 412 mL to me. And both are in the same 412 mL. Actually, you don't need to know the volume for it cancels. Note M = moles/L. So M NH3 = 0.0742/0.412 L = ?? M NH4Cl = 0.124/0.412 L = ?? BUT since you are dividing base/acid that is pH = pKa + log...
Tuesday, May 12, 2009 at 8:56pm by DrBob222

chemistry
sorry. The reaction is: 2 NO(g) + Cl2 ---><--- 2NOCl deltaH is the heat of reaction deltaS is the change in entropy T is temperature in kelvin deltaG is a direct measure of spontaneity DeltaH (kJ/mol) 2NO= 90.29/mol DeltaH (kJ/mol) Cl2= 0 DeltaH (kJ/mol) 2NOCl= 51.71/mol...
Monday, August 1, 2011 at 10:22pm by J

Chemistry
How many grams of butane must be burned to provide the heat needed to melt a 85.0-g piece of ice (at its melting point) and bring the resulting water to a boil (with no vapourization)? Assume a constant pressure of 1 bar and use the following data: Hfo(H2O(g))=-241.83 kJ/mol, ...
Monday, January 23, 2012 at 11:40pm by David

chemistry
Consider hypothetical elements X and Y. Suppose the enthalpy of formation of the compound XY is −336 kJ/mol, the bond energy for X2 is 421 kJ/mol, and the bond energy for Y2 is 152 kJ/mol. Estimate the XY bond energy in units of kJ/mol.
Monday, December 13, 2010 at 4:33pm by a

chemistry
Consider the hypothetical elements X and Y. Suppose the enthalpy of formation for the compound XY is {336 kJ/mol, the bond energy for X2 is 414 kJ/mol, and the bond energy for Y2 is 159 kJ/mol. Estimate the XY bond energy in units of kJ/mol.
Monday, December 13, 2010 at 1:22pm by chemistry

chemistry
Consider the hypothetical elements X and Y. Suppose the enthalpy of formation for the compound XY is -336 kJ/mol, the bond energy for X2 is 414 kJ/mol, and the bond energy for Y2 is 159 kJ/mol. Estimate the XY bond energy in units of kJ/mol.
Monday, December 13, 2010 at 4:33pm by Jude

chemistry
Nitroglycerin is a powerful explosive, giving four different gases when detonated.2 C3H5(NO3)3 (l) → 3 N2 (g) + 1/2 O2 (g) + 6 CO2 (g) + 5 H2O (g)Given that the enthalpy of formation of nitroglycerin, ΔHf, is −364 kJ/mol, calculate the energy (heat at ...
Saturday, March 3, 2012 at 5:24am by ogi

chemistry
Nitroglycerin is a powerful explosive, giving four different gases when detonated.2 C3H5(NO3)3 (l) → 3 N2 (g) + 1/2 O2 (g) + 6 CO2 (g) + 5 H2O (g)Given that the enthalpy of formation of nitroglycerin, ΔHf, is −364 kJ/mol, calculate the energy (heat at ...
Saturday, March 3, 2012 at 6:25am by ogi

Chemistry Problem
Consider an ionic compound, MX, composed of generic metal M and generic halogen X. The enthalpy of formation of MX is Hf = 457 kJ/mol. The enthalpy of sublimation of M is Hsub = 121 kJ/mol. The ionization energy of M is IE = 433 kJ/mol. The electron affinity of X is EA = ...
Saturday, February 2, 2013 at 1:25am by Anonymous

chemistry
Hvap 40.65 kJ/mol Hf -285.83 kJ/mol Hfusion 6.03 kJ/mol specific heat 4.186 J/gC molar mass 18.02 g How much energy is consumed by thawing 4.3 g ice?
Thursday, June 28, 2012 at 11:18am by martin

chemistry
Hvap 40.65 kJ/mol Hf -285.83 kJ/mol Hfusion 6.03 kJ/mol specific heat 4.186 J/gC molar mass 18.02 g How much energy is consumed by thawing 4.3 g ice?
Thursday, June 28, 2012 at 11:18am by martin

chemistry
You need the heat of combustion per mol of propane. Then kJ/mol x mol = 188.23 kJ. Solve for mol and convert that to grams. g = mols x molar mass.
Saturday, August 11, 2012 at 10:41am by DrBob222

chemistry
Calculate the heat of formation of SiO4(s), given that the heats of formation of SiO2(s), -910.90 KJ/mol; H2O(l), -285.8 KJ/mol; HF (g), -271.1 KJ/mol.
Friday, November 7, 2008 at 6:15pm by matt

Chemistry
Assume for fluorine a relative electronegativity of xp=4.0, determine xcarbon. [Given: BEC-C=347 kJ/mol; BEF-F=155 kJ/mol; BEC-F=429 kJ/mol.
Saturday, October 12, 2013 at 9:21pm by ss01

Chemistry
Calculate the energy (in kJ/mol) required to remove the electron in the ground state for each of the following one-electron species using the Bohr model. (a) He+ kJ/mol (b) Li2+ kJ/mol
Tuesday, January 24, 2012 at 12:03am by Sarah

Chemistry
Calculate the energy (in kJ/mol) required to remove the electron in the ground state for each of the following one-electron species using the Bohr model. (a) He+ kJ/mol (b) Li2+ kJ/mol
Tuesday, January 24, 2012 at 6:18pm by Sarah

Chemistry
Please note that I made an error in the above. The heat of fusion is 6.02 kJ/mol. To change to J/g we must do this. 6.02 kJ/mol x (1 mol/18.015 g) x (1000 J/kJ) = 334 J/g. Sorry about that.
Friday, November 28, 2008 at 4:37pm by DrBob222

Chemistry (balance)
1320 0 kJ/mol x ?mol = 791.60 kJ. Solve for ?mol, then g = mol x molar mass.
Monday, August 20, 2012 at 1:06pm by DrBob222

chemistry
use the following data, as appropriate, to estimate the molarity of a saturated aqueous solution of Sr(IO3)2. Molarity of a saturated aqueous solution of Sr(IO3)2 Sr(IO3)2(s) delt h kJ/mol=-1019.2 delta G kJ/mol=-855.1 delta S= 234 J mol-1K-1 Sr^2+(aq) delta h= -545.8 kJ/mol ...
Sunday, December 2, 2012 at 12:34am by Allyx3

chemistry
use the following data, as appropriate, to estimate the molarity of a saturated aqueous solution of Sr(IO3)2. Molarity of a saturated aqueous solution of Sr(IO3)2 Sr(IO3)2(s) delt h kJ/mol=-1019.2 delta G kJ/mol=-855.1 delta S= 234 J mol-1K-1 Sr^2+(aq) delta h= -545.8 kJ/mol ...
Sunday, December 2, 2012 at 11:09am by Allyx3

EXAM TMRW
for the first one I got 332 kJ/mol E = hc/lamda E = (6.626E-34)(2.998E8)/(360E-9) E = 5.522 J To convert it to kJ/mol, multiply by 6.022E23 and divide by 1000 to get 332 kJ/mol
Monday, December 1, 2008 at 5:11pm by Shaniquaa

Chemistry
Glycine,C2H502N, is important for biological energy.Find the heat of combustion deltaHrxn. Delta H [C2H5O2N]=-537.3 kj/mol DeltaH [ CO2(g)=-393.5 kj/mol DeltaH[H2O(l)]-285.8 kj/mol
Tuesday, November 15, 2011 at 10:49pm by Nicole

Chemistry
Calculate the entropy change in the surroundings when 1.00 mol N2O4(g) is formed from 2.00 mol NO2(g) under standard conditions at 298 K. I get +192 J/K. The book says -192 J/K. Here is my work, where am I going wrong? Standard Enthalpy of NO2(g) = 33.18 kJ/mol * 2 mol = 66.36...
Saturday, February 21, 2009 at 1:58pm by chemstudent

chem
I really don't know. If the -118 is kJ/mol, then, yes, you divide the -118 by 2 and multiply by 0.02810. But if the -118 kJ is the heat given off by the reaction (not kJ/mol but kJ/reaction), then -118 x 0.02810 is the way to do it. I don't know if your reaction is kJ/mol or ...
Saturday, December 1, 2007 at 2:29pm by DrBob222

Chem
Calculate ΔG at 25C for the precipitation of lead(II) chloride from mixing 100. mL of 0.025 M lead(II) nitrate solution with 100. mL of 0.15 M sodium chloride solution. The ΔG for the reaction at 25C = −27.36 kJ/mol. (Hint: write out reaction equation also...
Sunday, February 23, 2014 at 4:48pm by Anonymous

AP Chemistry
Consider the reaction 2 Al2O3(s) ! 4 Al(s) + 3 O2(g) . H = +3339.6 kJ/mol What is the change in heat when 0.455 L of a 3.60 M Al solution reacts with excess O2 ? 1. -424 kJ 2. -2735 kJ 3. -1695 kJ 4. -1368 kJ 5. -26,521 kJ 6. -21,962 kJ 7. -685 kJ 8. -5477 kJ
Sunday, September 29, 2013 at 5:05pm by Anonymous

CHEMISTRY> HELP QUICK! pls
Use the given data at 298 K to calculate G for the reaction 2NO(g) + 2H2(g) N2(g) + 2H2O(g) Substance NO(g) H2(g) N2(g) H2O(g) Hf (kJ/mol) 90 0 0 -242 S(J/Kmol) 211 131 192 189 a. -270 kJ b. -630 kJ c. -3.46 x 104 kJ d. -667 kJ
Saturday, September 4, 2010 at 11:05pm by Lucinda

chemistry
A sample of naphthalene (C10H8) that has a mass of 0.7200 g is burned in a bomb calorimeter. The mass of the calorimeter is 1.580 kg, and its specific heat is 2.55 J/(g C). As a result of the reaction, the temperature of the calorimeter increases from 22.00C to 29.3C. If 1 ...
Thursday, August 22, 2013 at 5:59pm by sean

AP Chem
Consider the reaction 2 Al2O3(s) -> 4 Al(s) + 3 O2(g) . H = +3339.6 kJ/mol What is the change in heat when 0.455 L of a 3.60 M Al solution reacts with excess O2 ? 1. -685 kJ 2. -21,962 kJ 3. -1368 kJ 4. -2738 kJ 5. -5477 kJ 6. -26,521 kJ 7. -424 kJ 8. -1695 kJ
Sunday, November 7, 2010 at 2:52pm by Beth

Chemistry
Using the bond entalpies ∆H: C---C: 348kJ C=C: 612 kJ CC (triple bond) : 960 kJ C---H: 412 kJ H---H: 436 kJ Calculate the calculate the value of ∆H of reaction for H2C=CH2(g) + H2(g) → CH3CH3(g)
Tuesday, February 17, 2009 at 10:30am by Anonymous

ap chemistry
The energy change H associated with the reaction NBr3(g) + 3H2O(g) ! 3HOBr(g) + NH3(g)is +81 kJ/mol rxn. These bond energy values might be useful:O-H 459 kJ/mol; N-H 386 kJ/mol;O-Br 201kJ/mol. The strength of the N Br bond is
Wednesday, October 31, 2012 at 5:49pm by cheri

Chemistry
Determine whether the following reaction is endothermic or exothermic: Mg(g) + 2 F (g)--> Mg 2+(g) + 2 F- Mg: I1= 738 kJ/mol I2= 1451 kJ/mol F: EA= -328 kJ/mol
Monday, April 18, 2011 at 4:36pm by Kamila

Chemistry (please check)
#1 is a little confusing with the use of the word largest. I think it is common practice to list LiF as the largest lattice energy but technically it is the smallest number. Lattice energies are as follows: LiF = -1036 kJ/mol NaF = -923 kJ/mol LiCl = -853 kJ/mol NaCl = -787 kJ...
Friday, April 15, 2011 at 11:18pm by DrBob222

Chemistry
"I am working on a problem like this one. I dont understand how you got to 51.4 from 30500 + (-20,907) = 51.4 kJ. Can you explain?" The 30500 should be negative: -30500+(-20907) This gives you -51407 J/mol. Convert to kJ: -51.407 kJ/mol or -51.4 kJ/mol.
Wednesday, March 14, 2012 at 11:55pm by KJ

Chemistry
Use the data given to calculate the value of delta G rxn for the reaction at 25C 2C(graphite)+H2(g)--->C2H2(g) C H2 C2H2 S(J K^-1 mol^-1)| 5.74 |130.68| 201.0 ------------------- delta H(kJ/mol) | 0 | 0 |-226.8 a.-291.4 kj b.-244.3 Kj c.-226.8 kj d.-207.6 Kj e.-64.6 Kj
Thursday, December 2, 2010 at 8:06pm by Liliy

Chemistry
Given the standard heats of reaction Reaction ∆H0 M(s) + 2 X2(g) → MX4(g) −123.7 kJ/mol X2(g) → 2 X(g) +297.3 kJ/mol M(g) → M(s) −25.1 kJ/mol calculate the average bond energy for a single M X bond. Answer in units of kJ/mol
Sunday, October 7, 2012 at 9:54pm by Austin

chemistry
Given the standard heats of reaction Reaction ∆H0 M(s) + 2 X2(g) → MX4(g) −123.7 kJ/mol X2(g) → 2 X(g) +297.3 kJ/mol M(g) → M(s) −25.1 kJ/mol calculate the average bond energy for a single M X bond. Answer in units of kJ/mol
Sunday, October 7, 2012 at 9:55pm by dave

chemistry please help
Calculate the lattice energy of potassium oxide from the following data: Enthalpy of sublimation of potassium: +89.24 kJ/mol Bond energy of oxygen: +498 kJ/mol First ionization energy of potassium: +419 kJ/mol 1st electron affinity of oxygen: -141 kJ/mol 2nd electron affinity ...
Sunday, April 17, 2011 at 11:57am by Joanie

CHEM please!!! help
Calculate the lattice energy of potassium oxide from the following data: Enthalpy of sublimation of potassium: +89.24 kJ/mol Bond energy of oxygen: +498 kJ/mol First ionization energy of potassium: +419 kJ/mol 1st electron affinity of oxygen: -141 kJ/mol 2nd electron affinity...
Tuesday, April 19, 2011 at 10:11am by Joanie

chemistry
Calculate the heat of formation of water from its constituent elements from the following information: 3 H2 (g) + O3 (g) 3H2O ∆H = ? 2 H2 (g) + O2 (g) 2H2O ∆H = - 483.6 3 O2 (g) 2O3 (g) ∆H = 284.5 a. -480 kJ/mol b. 480 kJ/mol c. -867 kJ/mol d. 867 kJ...
Saturday, April 18, 2009 at 5:13pm by lil'mama

CHEMISTRY
0.1985L x 0.400 = 0.07940 mol HCl 0.1501L x 0.500 = 0.07505 mol NaOH Therefore, 0.07505 mol react. 0.07505 mol x 56 kJ/mol = ? kJ
Tuesday, May 1, 2012 at 1:22am by DrBob222

Chemistry
I wonder if that is kJ/month or kJ/mol. I assume kJ/mol. No, the equation isn't q = CmT. It's mass x delta Hvap.
Tuesday, May 18, 2010 at 11:04pm by DrBob222

Chemistry Urgent
Do you want enthalpy/grams or enthalpy/mol. Most prefer it to be kJ/mol. q = g H2O x specific heat H2O x (Tfinal-Tinitial) That gives you q/2.30g X = ? J/g If you want J/mol it is J/g x 82.0 = ? J/mol. You can change that to kJ/mol if you wish.
Tuesday, March 11, 2014 at 10:35pm by DrBob222

chemistry
(products)- (reactants)=delta H (-403.4 kJ/mol)-(-425.3 kJ/mol)=21.9 kJ
Sunday, September 4, 2011 at 9:34pm by Hightower

Chemistry
Delta H for the reaction is the heat released when 1 mol Al reacts with 3 mol HCl. You have 30 kJ from 4.00 g Al. You want to convert that to 1 mol Al. So 30 kJ x molar mass/4.00 = ? kJ per mol.
Sunday, January 22, 2012 at 2:41pm by DrBob222

chem 1406
you shouldve got a bigger answer and ur solving for the kj not kj/mol. remember you have to multiply the 2000 moles by the 4130 kj/mol to get rid of the mole.
Tuesday, April 27, 2010 at 12:19am by Kevin

Chemistry
Octane (C8H18) undergoes combustion according to the following thermochemical equation: 2 C8H18(l) + 25 O2(g) ---> 16 CO2(g) + 18 H2O(l) DHo = -11,200 kJ Given : DHfo [CO2(g)] = -393.5 kJ/mol and DHfo[H2O(l)] = -285.8 kJ/mol. Calculate the enthalpy of formation of one mole...
Wednesday, November 25, 2009 at 1:50am by Robert

chemistry
Given handbook std enthalpies of formation at 298K for C5H10 (liq)=-105.9 kJ/mol and C5H10 (g)=-77.2 kJ/mol, estimate the normal boiling point of cyclopentane. I calculated delta H (vap or rxn) to be +28.7 kJ/mol. I am not sure how to proceed from here. Thank you very much for...
Thursday, September 22, 2011 at 4:25pm by Holly

Chem
Bond enthalpy is the energy required to break a mole of a certain type of bond. O=O = 495 kj/mol S-F = 327 kj/mol S=O = 523 kj/mol Use average bond enthalpies to estimate the enthalpy delta H (rxn) of the following reaction: 2SF4 + O2 ---- 2OSF4 Express your answer numerically...
Wednesday, November 12, 2008 at 11:27pm by Dr BOB plz ANSWER

chemistry
C8H18(g) + 25/2(O2)(g) -> 8CO2(g) + 9H2O(g) STANDARD ENTHALPY VALUES (H): 02(g) = 0 kj/mol CO2 (g) = -393.5 kj/mol H20(g) = -241.8 kj/mol H total = -5094 kJ H of C8H18(g) is your unknown, so call that x. use: H of reaction = H of products - H of reactants so, -5094 kJ = [8(...
Sunday, January 29, 2012 at 11:38pm by Paige

Chemistry
-2.1786E-18 J to AN electron x 6.02E23 will give you J/mol H atoms and that x 2 gives J/mol H2 and that x (1 kJ/1000) converts to kJ/mol
Thursday, November 29, 2012 at 1:55am by DrBob222

chemistry
Just to be sure we're on the same page my post could be misinterpreted. You are SUPPOSED to convert kJ/mol to J/mol. Using kJ/mol won't work.
Tuesday, March 25, 2014 at 11:21pm by DrBob222

Chemistry
262 kJ/mol? per mol of what? And 272 kJ/mol = energy difference of what? And how many otato chips = 1 serving?
Wednesday, February 13, 2008 at 9:38pm by DrBob222

Chemistry
Calculate delta H for this reaction: N2 + 3H2 --> 2NH3 I am given the bond dissociation energy for N-N (163 kJ/mol), H-H (436 kJ/mol), and N-H (391 kJ/mol) I can't seem to find a similar problem anywhere, they are all given 2 or 3 similar equations.
Saturday, December 1, 2012 at 5:53pm by Emily

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