Wednesday
March 12, 2014

# Search: Thermochemistry

Number of results: 110

Thermochemistry determine the final temperature if 45.67 kJ of heat energy is removed from 18.5 g of H2O (g) at 122 degrees Celsius useful information sp. heat H2O (s) = 2.03 J/g(degree C) sp heat H2O (l) = 4.18 J/g(degree C) Sp heat H2O (g) = 2.01 J/g(degree C) enthalpy H Fus...
Wednesday, February 15, 2012 at 11:12pm by Rose Bud

Thermochemistry
Thanks!
Tuesday, March 19, 2013 at 10:44pm by Sean

Thermochemistry
w is work
Friday, October 30, 2009 at 4:54pm by Kyle

ThermoChemistry
How do you find [delta]Hvap?
Wednesday, March 19, 2008 at 10:21pm by James

college chemistry-thermochemistry
thanx so much!
Saturday, November 8, 2008 at 10:38pm by maryanne

thermochemistry college
Yes! ...She has a big butt!
Tuesday, December 8, 2009 at 8:42pm by JoJo

Thermochemistry
Yes, and for some problems it is written that way.
Tuesday, December 2, 2008 at 11:55pm by DrBob222

college chemistry-thermochemistry
I just posted it at the original spot below.
Saturday, November 8, 2008 at 10:38pm by DrBob222

college chemistry-thermochemistry
ya you're right i accidently put the wrong value in!
Saturday, November 8, 2008 at 8:49pm by maryanne

College Chemistry
Go to this site and scroll down to "Energy and Enthalpy" which is approximately half way down the page. The first sentence talks about the "system" and the "surroundings." http://www.chemistryexplained.com/Te-Va/Thermochemistry.html What are the reaction products and reactants...
Tuesday, March 30, 2010 at 9:31pm by DrBob222

Thermochemistry
heat=167*c*(3.7) Normally, one wants enthalpy on a per mole basis, if so, divide by 2.
Sunday, October 17, 2010 at 9:50pm by bobpursley

Thermochemistry
C2H5OH + 3O2 ==> 2CO2 + 3H2O deltaHrxn = (2*DHfCO2)+(3*DHfH2O)-(DHfC2H5OH = ??
Monday, April 18, 2011 at 5:16pm by DrBob222

thermochemistry
Calculate the amount of heat liberated (in kJ) from 374 g of mercury when it cools from 83.7°C to 19.1°C.
Sunday, October 5, 2008 at 12:56pm by james

thermochemistry
what is the formula to find the mass of propane that must be combusted to produce 188.3kj of energy?
Saturday, August 11, 2012 at 10:30am by Anonymous

N2 + 2F2 ---> 2NF3 calculate the standard enthalpy
Thursday, February 16, 2012 at 1:36pm by Anonymous

Thermochemistry
When 1 mol of a gas burns at constant pressure, it produces 2426 J of heat and does 6 kJ of work. What is Delta H, q, and w?
Monday, October 18, 2010 at 7:44pm by Michelle

Thank You for my final temperature I got around 83.1 degrees celsius
Wednesday, February 15, 2012 at 11:12pm by Rose Bud

Thermochemistry
alchol releases 29.7kJ/g when it burns. Convert this value to the number of calories per gram
Sunday, December 4, 2011 at 8:58pm by Anonymous

Thermochemistry
The work is done against friction while the ball slows down. Consider it equal to the loss of kinetic energy
Friday, October 30, 2009 at 4:54pm by drwls

thermochemistry
q = mass water x heat vap. I would convert 491g H2O to mols by dividing by 18 g/mol.
Friday, April 13, 2012 at 12:11am by DrBob222

Thermochemistry
3CO(g)+ Fe2O3(s) --> 2Fe(s) + 3CO2(g) + 24.7 kJ. How much heat is released when 56 grams of CO react?
Tuesday, December 14, 2010 at 11:22pm by Hannah

ThermoChemistry
with ln(p1/p2)=deltaHvap/R x (1/T2-1/T2)
Wednesday, March 19, 2008 at 10:21pm by Mikal

thermochemistry college
does anyone know profesor of green river community college, auburn,wa, sue critchlow ????
Tuesday, December 8, 2009 at 8:42pm by eva

Thermochemistry
H=? q=2.426 kJ w=-6 kJ Therefore, E=-8
Monday, October 18, 2010 at 7:44pm by Jenna

thermochemistry
The heat ofvaporization of water at 373K is40.7kj/mol. Find q for the evaporation of 491g of water at this temperation
Friday, April 13, 2012 at 12:11am by Anonymous

Chemistry
I have a test on the general concepts of thermochemistry tomorrow. how should i study for it since its not based on problem solving, just concepts?
Wednesday, October 24, 2007 at 12:40pm by Nick

ThermoChemistry
This is done the same way as the NaCl problem posted earlier; however, in this case the DHsoln is a negative number which means you make q a + number.
Friday, December 2, 2011 at 2:25pm by DrBob222

Chemistry
ok thank you, we're doing thermochemistry right now, so we actually just did that calorimeter lab yesterday, and we've been using that equation.. i dont know if my teacher wants us to use methods we already know.
Friday, September 14, 2007 at 7:31pm by Dick Rogers

Chemistry
I need to perform a chemical demonstration on thermochemistry or kinetics or colligative properties for chemistry class. However I cannot have demonstrations involving fire.
Tuesday, January 12, 2010 at 8:14am by alex

Thermochemistry
It takes 45.0 J to raise the temperature of an 9.70 g piece of unknown metal from 13.0 degrees C to 24.5 degreesC. What is the specific heat for the metal?
Sunday, October 17, 2010 at 9:20pm by Michelle

Thermochemistry Ap Chem homework
i used the formula m(delta T)Cp=delta H (10.0)(20.0-0.00)= x and so x = 200... is that correct, if so would the units be degrees celcius?
Monday, November 15, 2010 at 5:58pm by Chris

Thermochemistry
Compute the amount of heat released (absolute value) when 2.3 kg of liquid ethanol is burned in excess oxygen to make carbon dioxide and liquid water.
Saturday, December 3, 2011 at 2:43pm by LaurenB

chemistry-thermochemistry
A student mixes 85.7 g of water at 68.0°C with 50.7 g of water at 24.5°C in an insulated flask. What is the final temperature of the combined water
Sunday, October 5, 2008 at 12:55pm by james

Thermochemistry
3*28.01 g CO reacting produces 24.7 kJ heat. Therefore, 56 g CO will produce 24.7 x 56/84.03 = ??
Tuesday, December 14, 2010 at 11:22pm by DrBob222

Thermochemistry
See the Au and H2O. All of the use the same concept and the same formula. heat lost by one + heat gained by other = 0
Friday, December 2, 2011 at 2:26pm by DrBob222

Thermochemistry
How many grams of water at 0 degrees C can be frozen into ice at 0 degrees C if 55.0 kJ of heat is removed? delta Hsolid= -6.01 kJ/mol
Tuesday, December 14, 2010 at 11:23pm by Hannah

Thermochemistry
A total of 2.00 mol of a compound is allowed to react in a foam coffee cup that contains 167 g of water. The reaction caused the temperature of the water to rise from 21.0 to 24.7 degrees C. What is the enthalpy?
Sunday, October 17, 2010 at 9:50pm by Michelle

Thermochemistry Ap Chem homework
(10.0 g water) (delta 20 degrees C)(4.184J/g x C) = 836.8 J needed to heat the water. You just forgot to multiply the specific heat.
Monday, November 15, 2010 at 5:58pm by John

Thermochemistry
The enthalpy formation of ethanol, C2H5OH, is -277.0 kJ/mol @ 298.15 K. Calculate the enthalpy of combustion of one mole of ethanol, assuming that the products are CO2(g) & H2O (l).
Monday, April 18, 2011 at 5:16pm by Morgan

Thermochemistry
The standard enthalpy of formation of n-octane is -249.95 kJ/mol. Compute the amount of heat liberated when 5.24 g of n-octane is burned completely with excess oxygen to form carbon dioxide and liquid water.
Sunday, December 4, 2011 at 8:58pm by LaurenB

thermochemistry
heat=mass*specific heat*deltaTemp look up the specific heat of Hg.
Sunday, October 5, 2008 at 12:56pm by bobpursley

Thermochemistry
Transfer of energy from one ball to another during collision is an interesting process. It is done by transferring stress waves, but there must be some motion of the balls during contact to allow work to be done on the other ball.
Friday, October 30, 2009 at 4:54pm by drwls

college chemistry-thermochemistry
I got: delta H= 482.79J 482.79/150gNH4NO3 x 80gNH4NO3/mol NH4NO3 =2574.88J/mol =2.575 kJ/mol Is this right?
Saturday, November 8, 2008 at 8:49pm by maryanne

ThermoChemistry
Just a quick note to say that changing celsius to kelvin and back again is not necessary. Since it is a difference of temperatures only, and since 1 degree C = 1 degree K, you may subtract with C or K and come up with the same value.
Friday, December 2, 2011 at 2:21pm by DrBob222

How did you know that the temperature dropped down to 100 degrees C? I have the same exact problem, except the heat is being added, not taken away. And the initial temperature is 73.5 degrees C.
Wednesday, February 15, 2012 at 11:12pm by Neva

Thermochemistry
heat in combustion as measured by the calorimeter = 60.8 kJ/K x (delta T) = ? kJ released. ?kJ released/deltaH in kJ/mol = #moles.
Sunday, December 4, 2011 at 8:57pm by DrBob222

Thermochemistry
Heat formation CaF2 is 30.3 kJ/1.95 g CaF2. Convert 1.95 g to moles if you want the answer in kJ/mol which is the usual way you find it in table.
Saturday, June 19, 2010 at 12:43am by DrBob222

ThermoChemistry
If 18 g of Kr initially at 0.5 bar and 18 L is brought to 0.49 bar and 5L, what is the overall change in enthalpy of this process? Assume that Kr is an ideal gas.
Friday, December 2, 2011 at 2:22pm by LaurenB

Thermochemistry
2C2H5OH + 6O2 ==> 4CO2 + 6H2O Calculate delta H (DHrxn) for the reaction from DHrxn = (n*DHf products) - (n*DHf reactants) Then heat released = DHrxn x (2,300/2*molar mass C2H5OH)
Saturday, December 3, 2011 at 2:43pm by DrBob222

thermochemistry
A chemical reaction takes place in a container of cross-sectional area 100 cm2 . As a result of the reaction, a piston is pushed out through 19 cm against an external pressure of 596 torr. What is the value for w for this reaction?
Sunday, October 14, 2012 at 3:42pm by valerie

Thermochemistry
So q=mc(Tf-Ti) could be written as Delta H=mc(Tf-Ti) assuming the pressure is constant?
Tuesday, December 2, 2008 at 11:55pm by Kevin

Thermochemistry
6.01 kJ/mol x ?mol = 55 kJ/ Solve for ?mol.
Tuesday, December 14, 2010 at 11:23pm by DrBob222

ThermoChemistry
When 19 mL of water at 22 C is combined with 18 mL of water at 64 C, what is the final temperature of the water?. The specific heat of water is 4.184 J/g/K and its density is 1.0 g/mL.
Friday, December 2, 2011 at 2:21pm by LaurenB

college chemistry-thermochemistry
A 1.50g sample of NH4NO3(s) is added to 35.0g of water in a foam cup and stirred intil it dissolves. The temperature of the solution drops from 22.7 to 19.4 degrees celcius. What is the heat of dissolution of NH4NO3, expressed in kJ/mol NH4NO3?
Saturday, November 8, 2008 at 8:49pm by maryanne

Thermochemistry
A 1.00-g sample of solid calcium was burned in fluorine to give a 1.95 g sample of pure CaF2. The energy given off in this reaction was 30.3 kJ. Given this information, we can say that the heat of formation of 1 mol of CaF2 is
Saturday, June 19, 2010 at 12:43am by joan

Thermochemistry
I'm confused about the difference between the q in q=mc(Tf-Ti) and (Delta)H, or enthalpy. What exactly does enthalpy mean and how is that different than q? (I'm also confused about what Gibbs Free Energy actually means; I know that if it's negative, the reaction is spontaneous...
Tuesday, December 2, 2008 at 11:55pm by Kevin

Thermochemistry
If a chalice made of pure gold weighing 1.24 kg and initially at 15 C is filled with 100.0 mL of water at 89 C, what is the final equilibrium temperature of the system? The heat capacities of water and gold are 75.29 and 25.42 J/mol/K, respectively.
Friday, December 2, 2011 at 2:26pm by LaurenB

THERMOCHEMISTRY
The IUPAC name for acetylene is ethyne. Ethylene is not the same compound and the IUPAC name for that is ethene. Are you melting the snow and ice with acetylene or with ethylene? You need to know the heat of combustion of whatever it is you're using.
Tuesday, February 21, 2012 at 4:28pm by DrBob222

Thermochemistry
q = mass metal x specific heat metal x delta T. Solve for specific heat metal, the only unknown.
Sunday, October 17, 2010 at 9:20pm by DrBob222

You need to check the post carefully. The equation you want is not balanced. I think you have made two typos. I think the left H2O should be H2O2 and I think the right H2) should be H2O
Thursday, February 16, 2012 at 1:36pm by DrBob222

Thermochemistry
delta H is defined as the change in heat content of a process at constant pressure. Then qp = delta H. In fact, you will see some problems in which a solid is added to water in a calorimeter and the change in T is noted; the question than asks for delta H of the reaction.
Tuesday, December 2, 2008 at 11:55pm by DrBob222

Thermochemistry, calorimetry
The density of ice is 0.9168 g/cm3. The density of water is 0.9998 g/cm3. Calculate the difference between ΔU (internal energy) and ΔH (enthalpy) during the fusion of 2.5 moles of ice at atmospheric pressure.
Tuesday, November 20, 2012 at 6:38pm by Peter

college chemistry-thermochemistry
I worked the problem and obtained a different answer. Isn't that 1.50 g (not 150)? I used 80.04 for the molar mass of NH4NO3 and obtained 25.762 kJ/mol which I would round to 25.8 kJ/mol.
Saturday, November 8, 2008 at 8:49pm by DrBob222

Thermochemistry
A sample of liquid mercury (mass 58 g and temperature 149.0 C) is poured into 79 g of H2O at 19 C. Calculate the final temperature of the mixture, assuming no heat is lost. The heat capacities of Hg and H2O are 27.98 and 75.33 J/mol/K, respectively.
Friday, December 2, 2011 at 2:26pm by LaurenB

chemistry-thermochemistry
call the 85 g water water1, and the other water2. sum of heat changes =0 heatfromwater1+heatfromwater1=0 One will be negative, as one of them cools. mass1*cw*deltaTemp1+mass2*cw+deltaTemp2=0 I assume you can handle it from here. Tf in each will be the same, ti for each is ...
Sunday, October 5, 2008 at 12:55pm by bobpursley

Chem. Copper and Chromium. Random Q...
So, I have a general chemistry test. My teacher said to know... "Copper and Chromium exceptions." I have no idea what that means. I am currently learning about Thermochemistry and the Quantum Theory of an Atom. Do you have any idea what this might mean?? Thank you for any ...
Saturday, November 15, 2008 at 1:13am by Sarah

Thermochemistry
A constant pressure calorimeter having a heat capacity of 60.8 kJ/K is used to measure the energy released from burning a compound in excess oxygen to form CO2(g) and H2O(l). If the enthalpy of combustion of the compound is -2914.0 kJ/mol and the temperature of the calorimeter...
Sunday, December 4, 2011 at 8:57pm by LaurenB

thermochemistry college
No, but she is listed in the school directory website as a member of the chemistry faculty. http://www.greenriver.edu/Staff/Default.aspx
Tuesday, December 8, 2009 at 8:42pm by drwls

college chemistry-thermochemistry
How much heat is absorbed. mass H2O x specific heat water x delta T. 35.0g x 4.18 J/g*C x (22.7-19.4) = ?? That is delta H/1.50 g NH4NO3. Change that to delta H/mol NH4NO3 and change to kJ/mol. Post your work if you get stuck.
Saturday, November 8, 2008 at 8:49pm by DrBob222

Thermochemistry
What is w? How can only one ball be "the system" ? The collision is elastic since the balls have equal mass and exchange velocities. The only time kinetic energy is lost is when the originally moving ball slows down. The lost energy as the ball slows from 4.5 to 3.5 m/s is ...
Friday, October 30, 2009 at 4:54pm by drwls

Thermochemistry
Compute the change in temperature when 1.1 g of sodium chloride is dissolved in 200.0 mL of water initially at 28 C. The heat capacity of water is 4.184 J/mL/K. Neglect the heat capacity of the NaCl. Species ΔfH (kJ/mol) NaCl(aq)-407.3 NaCl(s) -411.2
Friday, December 2, 2011 at 4:02pm by LaurenB

Thermochemistry
When 1.477 mole of an inorganic salt were dissolved in 1.00 L of water in a constant pressure solution calorimeter, the temperature of the calorimeter changed from 25.00oC to 24.40 oC. The total heat capacity of the calorimeter including all its contents was 2.18 kJ oC-1 What ...
Friday, June 12, 2009 at 12:25am by Douglas

Thermochemistry
Suppose 23.6 g of ClF3(g) and 40 g of Li(s) are mixed and allowed to react at atmospheric pressure and 25 C until one of the reactants is used up, producing LiCl(s) and LiF(s). Using the NIST value for the enthalpy of formation of ClF3 (webbook.nist.gov), calculate the ...
Saturday, December 3, 2011 at 2:44pm by LaurenB

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

Thermochemistry Ap Chem homework
Any help would be great, even if it is just a way to start or a formula. Calculate the heat necessary to convert 10.0 g of water (just melted) at 0 degrees Celcius to water at 20 degrees Celcius, assuming that the specific heat remains constant at 1 cal/gram degrees celcius.
Monday, November 15, 2010 at 5:58pm by Chris

ThermoChemistry
Calculate the final temperature of solution when 10 g of oxalic acid, (COOH)2(s), is dissolved in 110.0 mL of water that is initially at 26 C. The enthalpies of formation of oxalic acid in the solid and aqueous phases are -826.8 and -818.8 kJ/mol, respectively. The heat ...
Friday, December 2, 2011 at 2:25pm by LaurenB

ThermoChemistry
c_hot = (4.184J/g*K)(18mL)(1g/mL) c_cold = (4.184J/g*K)(19mL)(1g/mL) Use: 0 = c_hot(T_f - T_initial,hot)+ c_cold(T_f - T_initial,cold) Solve for T_f and remember to convert temperature back to C from Kelvin and vice versa. Best of luck, ChemVantage Loather
Friday, December 2, 2011 at 2:21pm by JT

ap chemistry
DrBob222, thank you. Is there any online worksheets related to chemistry 8th edition zumdahl up to chapter 9. The topic include.. -percent composition of compounds and formula for compound like molecular and empirical -balancing equations -limiting reactant -theoretical and ...
Sunday, November 4, 2012 at 4:07pm by zoya

thermochemistry
A 12.48g sample of an unknown metal, heated to 99'c was then plunged into 50mL of 25'c water. The temperature of the water rose to 28.1'c. The specific heat of water is 4.184J/g. 1. How many joules of energy did the water absorb? 2. How many joules of energy did the metal lose...
Sunday, November 23, 2008 at 10:33pm by nichole

Chemistry
In a thermochemistry experiment the reaction of 0.0857 g of an unknown metal and an excess of 4.0 M HCl resulted in a 0.210 mL decrease in the volume of an ice/water mixture. Calculate the enthalpy of this reaction per 1 g of metal reacted. Needed data: density of water at 273...
Saturday, December 1, 2007 at 4:25pm by Raj

Chemistry (Thermochemistry)
Is there any equation out there that links the change in enthalpy (H) to the change in cell potential/voltage (E)? Yes, but the relationship involves the Gibbs Free Energy, which is G = H - TS, snd S is the entropy change. The change in G is approximatly the change in H in ...
Thursday, August 2, 2007 at 8:39am by Vic

Chemistry
please help! Is RTP in chemistry (thermochemistry and electrochemistry) referring to room temperature of 25degreeC (or 298K) and 1atm, or 20degreeC (293K) and 1atm? In my lecture notes on gas law, they stated RTP refers to 25degreeC, but in my electrochem lecture notes they ...
Sunday, November 6, 2011 at 4:57am by Hailey

Chemistry(defintions)
I need help on finding the definitions to these: Pressure being constant, the amount of heat in a chemical equation ___________. Randomness of particle measurement is called __________. Calories required to convert 1gm of liquid to vapor without a change in temperature ...
Tuesday, April 6, 2010 at 9:41pm by Bill

thermochemistry
Compute the heat of reaction per mole of combustion of C3H8 with O2. It should be in kJ per mole of C3H8. Divide 188.3 kJ by the heat of reaction per mole. Assume the H2O ends up in liquid state at 298 K. This will give you the number of moles of C3H8 required. Convert that to...
Saturday, August 11, 2012 at 10:30am by drwls

You are defiantly right. it is suppose to be 2H2O2(l) and 4H2O(l) and the first equation is suppose to be -622.2 kJ/mol actually they are all suppose to be kJ/mol, but that was a typo on the exercise. For a final answer I got -818.2 kJ/mol i used the first equation as is. then...
Thursday, February 16, 2012 at 1:36pm by Rose Bud

calculate enthalpy of H for the reaction N2H4(l) + 2H2O(l) -> N2(g) + 4H2)(l) Given the reactions N2H4(l) + O2(g) -> N2(g) + 2H2O(l) Enthalpy of H = -6.22.2 kJ H2(g) + (1/2)O2(g) -> H2O(l) enthalpy of H = -285.8 kJ/mol H2(g) + O2(g) -> H2O2(l) enthalpy of H = -187....
Thursday, February 16, 2012 at 1:14am by Rose Bud

calculate enthalpy of H for the reaction N2H4(l) + 2H2O(l) -> N2(g) + 4H2)(l) Given the reactions N2H4(l) + O2(g) -> N2(g) + 2H2O(l) Enthalpy of H = -6.22.2 kJ H2(g) + (1/2)O2(g) -> H2O(l) enthalpy of H = -285.8 kJ/mol H2(g) + O2(g) -> H2O2(l) enthalpy of H = -187....
Thursday, February 16, 2012 at 1:36pm by Rose Bud

Thermochemistry
Suppose a 0.17-kg billiard ball is rolling down a pool table with an initial speed of 4.5 m/s. As it travels, it loses some of its energy as heat. The ball slows down to 3.5 m/s and then collides straight-on with a second billiard ball of equal mass. The first billiard ball ...
Friday, October 30, 2009 at 4:54pm by Kyle

Thermochemistry
DH = delta H. DHsoln = DHsolvation - DHlatticeenergy DHsoln = -407.3 -(-411.2) = 3.9 kJ/mol The + means it is an endothermic reaction and the water will become cooler; we are extracting heat from the water. How much? 3.9 kJ/mol x (1000 J/kJ) x 1.1 g NaCl x (1 mol NaCl/molar ...
Friday, December 2, 2011 at 4:02pm by DrBob222

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

A 65.0 g sample of 0.600 M HI at 18.46 degrees celsius is added to 84.0 g of solution containing excess KOH, also at 18.46 degrees celsius. The final temperature is 21.96 degrees celsius. Calculate the enthalpy of H for the reaction. Assume the specific heat of the solution is...
Thursday, February 16, 2012 at 1:06am by Rose Bud

chem
topic: thermochemistry i'm not really sure how to go about his question. i'm not sure with formula to use. (perhaps Cspht= q/(m x deltaT)?)can you please help me step by step or give me a hint and i'll post my answer, pretty please? "250g of hot coffee at 95 degree celsius are...
Saturday, April 16, 2011 at 7:00pm by marie

Thermochemistry
Assistance needed. -------------------------- Raymonddd, AnthoniiEllis, Jenny B, Douglas, or whoever, Please type your subject in the School Subject box. Any other words are likely to delay responses from a teacher who knows that subject well. Please also note that we don't do...
Friday, June 12, 2009 at 12:25am by Writeacher

Thermochemistry
heat gained by gold + heat lost by water = 0 [mass Au x specific heat Au x (Tfinal-Tinitial)] + [mass H2O x specific heat water x (Tfinal-Tinitial) = 0 Solve for Tfinal. Note that you quote specific heat of Au and H2O in J/mol; therefore, the mass of Au and mass H2O must be in...
Friday, December 2, 2011 at 2:26pm by DrBob222

You have 65.0 g soln from HI and 84.0 g H2O with the KOH so total mass soln is 149 g. q = mass H2O x specific heat water x (delta T). USUALLY delta H for a reaction is done in kJ/mol. This problem has no easy way to get to moles but q/mol = J/mol and you can convert that to kJ...
Thursday, February 16, 2012 at 1:06am by DrBob222

chemistry
thermochemistry chem conceptual. i just want to check my understanding of this Say you got this: 1)A + b=c A=4.0 grams and -91.8kj evolve How do you find change of H ? I guess you convert A to grams and then shove it under the evolved heat ? ie. change of H= -91.8kj/2 mol= 2)...
Friday, August 7, 2009 at 1:23am by Jim_R

college chemistry-thermochemistry
i have one more question: I know this one has to do with hess's law but i'm not sure of how to get the enthalpy of vaporization? Clculate the enthalpy of vaporization of solid potassium bromide to a gas of ions, the process KBr--->K{+1}(g)+Br{-1}(g), from the following ...
Saturday, November 8, 2008 at 8:49pm by maryanne

college chemistry-thermochemistry
i have one more question: I know this one has to do with hess's law but i'm not sure of how to get the enthalpy of vaporization from this? Clculate the enthalpy of vaporization of solid potassium bromide to a gas of ions, the process KBr--->K{+1}(g)+Br{-1}(g), from the ...
Saturday, November 8, 2008 at 10:38pm by maryanne

Chemistry
In lab we did thermochemistry, where we are supposed to find the heats of solution, heat change of calorimeter and molar heat solution of the salt. I calculated that the calorimeter constant for the water we had was 883.194 Joules. We took 1/10 of a mole of NH4Cl and tried to ...
Sunday, October 31, 2010 at 3:44pm by Rani