Calculate the DELTA H(rxn), DELTA S(rxn), DELTA S(universe), DELTA G(rxn). For each system below indicate whether DELTA S and DELTA H are positive or negative. Then indicate if the reaction is entropy driven, enthalpy driven or neither. C3H8(g) + 2O2(g)
43,383 results
AP Chemistry
Calculate the delta H rxn for the following reaction: CH4(g)+4Cl2(g)>CCl4(g)+4HCl Use the following reactions and given delta H's: 1) C(s)+2H2(g)>CH4(g) delta H= 74.6 kJ 2) C(s)+2Cl2(g)>CCl4(g) delta H= 95.7 kJ 3) H2(g)+Cl2(g)>2HCl(g) delta H=

Chemistry
For which of the following reactions is the value of Delta H rxn equal to Delta H of formation? I. 2Ca(s) + O2(g) > 2CaO(s) II. C2H2(g) + H2(g) > C2H4(g) III. S(s) + O3(g) > SO3(g) IV. 3Mg(s) + N2(g) > Mg3N2(s). According to my answer key, the only

Chem
RXN #1: H2 (g) + O2 (g) > H2O2 (l) ; deltaH =? Calculate the enthalpy change (deltaH1) for the reaction above (RXN #1) using the information below and Hess' Law. RXN A: H2O2 (l) > H2O (l) + 1/2 O2 (g); deltaH=98.0 kJ/mol RXN B: 2 H2 (g) + O2 > 2

Chemistry
For the reaction described by the chemical equation: 3C2H2(g) > C6H6(l) .. Delta H rxn = 633.1 kJ/mol a) Calculate the value of Delta S rxn at 25.0 C... b) Calculate Delta G rxn... c) In which direction is the reaction, as written, spontaneous at 25 C

Chemistry
Given the thermodynamic data in the table below, calculate the equilibrium constant for the reaction: 2SO2(g)+O2> 2SO3 Substance (DeltaH^o) (Delat S^o) SO2 297 249 O2 0 205 SO3 395 256 Answer (it was given) 2.32x10^24 Even though the answer is given

chemistry
The standard internal energy change for a reaction can be symbolized as ΔU°rxn or ΔE°rxn. For the following reaction equations, calculate the energy change of the reaction at 25 °C and 1.00 bar. Sn(s) + 2Cl2(g) > SnCl4(l) ΔH°rxn = 511.3 kJ/mol

chemistry
Given overall reaction: P4 + 10Cl2 > 4PCl5 Delta H for the reaction = ? PCl5 > PCl3 + Cl2 Delta H = +157 kJ P4 + 6Cl2 > 4PCl3 Delta H = 1207 kJ Calculate the Delta H for the overall reaction.

chemistry
What is Delta H rxn for the following chemical reaction? H2O(l) + CCl4(l)> COCl2(g) + 2HCl(g)

Chemistry
If delta H°rxn and delta S°rxn are both positive values, what drives the spontaneous reaction and in what direction at standard conditions? The spontaneous reaction is a)enthalpy driven to the left. b)entropy driven to the right. c)entropy driven to the

CHEMISTRY
Please explain. The enthalpy changes for two different hydrogenation reactions of C2H2 are: C2H2+H2>C2H4 Delta H 1 C2H2+2H2>C2H6 Delta H 2 Which expression represents the enthalpy change for the reaction below? C2H4+H2>C2H6 Delta H = ? A. Delta

Chemistry
The standard internal energy change for a reaction can be symbolized as ΔU°rxn or ΔE°rxn. For the following reaction equations, calculate the energy change of the reaction at 25 °C and 1.00 bar. Sn(s) + 2Cl2(g) > SnCl4(l) ΔH°rxn = 511.3 kJ/mol

Chemistry
Which of the following reactions are spontaneous (favorable)? A] 2Mg(s) + O2(g) > 2MgO(s) Delta G = 1137 kJ/mol .. B] NH3(g) + HCl(g) > NH4Cl(s) Delta G = 91.1 kJ/mol ... C] AgCl(s) > Ag+(aq) + Cl(aq) Delta G = 55.6 kJ/mol .. D] 2H2(g) + O2(g) >

Chemistry
delta T = ikfm delta T is the amount f.p. is lowered. i is the number of particles; i.e., Na3PO4 will have i = 4 (3 for Na and 1 for PO4). m is molality. k is a constant and need not enter into the calculations. Arrange the following solutions in order of

Chemistry
use the data from this table of thermodynamic properties to calculate the maximum amount of work that can be obtained from the combustion of 1.00 moles of ethane, CH3CH3(g), at 25 °C and standard conditions. on the chart is said ethane(C2H6) is 84.0. In

Chemistry
How would you calculate delta H for the following reaction: 2P + 5Cl2 > 2PCl5 Given: PCl3 + Cl2 > PCl5 Delta H=87.9 kJ 2P + 3Cl2 > 2PCl3 Delta H=574 kJ I have no clue how to do this since I was absent. Can someone help?

Chemistry
Calculate the DELTA H(rxn), DELTA S(rxn), DELTA S(universe), DELTA G(rxn). For each system below indicate whether DELTA S and DELTA H are positive or negative. Then indicate if the reaction is entropy driven, enthalpy driven or neither. C3H8(g) + 2O2(g) =>

Chemistry
for the reaction of hydrogen with iodine H2(g) + I2(g) > 2HI(g) relate the rate of disappearance of hydrogen gas to the rate of formation of hydrogen iodide. and my answer is: rate formation of HI= delta [HI]/delta t and the rate of reaction of I2 =

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

Chemistry
1) A reactions has a delta H of 76 Kj and a delta S of 117 J/K. Is the reaction spontaneous at 298 K? Work: Delta G= 76kJ/mol  298K(117J/K/1000) Delta G= 41.134 Spontaneous 2) A reaction has a delta H of 11 kJ and a delta S of 49 J/K. Calculate the

chemistry
At 25 C the following heats of reaction are known: 2CIf (g)+ O2(g) > CL2O (g) + f2O Delta H rxn= 167.4 kj/mol 2CIf3(g) + 2O2 (g)> Cl2O(g) + 3F2O(g) Delta H rxn= 341.4 2F2(g) + O2(g) > 2F2O(g) Delta H rxn= 43.4kj/mol at the temperature, use Hess's Law

Chemistry
Is the following reaction spontaneous at 25*C? delta s reaction = 217 J/K*mol delta H rxn = 1202 KJ 2Mg (s) + O2 (g) > 2MgO (s) delta suniverse = delta s system  delta H system / T i got positive (+) 3.81 x 10 ^ 3 J/K and my notes says it is

chemistry 101
Calculate (delta) H rxn for 2NOCl(g) N2(g) + O2(g) + Cl(g) given the following set of reactions: 1/2N2(g) + 1/2O2(g)NO(g) delta H =90.3kJ NO(g) + 1/2Cl2(g)NOCl(g) delta H = 38.6 kJ

Chemistry
Given the Data: N2(g) + O2g) = 2NO(g) delta H = 180.7kj, 2NO(g) + O2(g) = 2NO2(g) delta H = 0113.1kj, 2N2O(g) = 1N2(g) + O2(g) delta H = 163.2kj. Using Hess’s Law calculate delta H for the reaction: N2O(g) + NO2(g) = 3NO(g)

Chemistry
CONTINUE>>>>>>>>>>> The enthalpy changes for two different hydrogenation reactions of C2H2 are: C2H2+H2>C2H4 Delta H 1 (there is a degree sign....standard enthalpy of formation??) *****WAIT A SECOND, IF I USE THE HEAT OF FORMATION VALUES TO CALCULATE

Chem
For the reaction I2(s)+Cl2(g) ==> 2ICl(g) delta H= 36kJ, delta S= 158.8J/K at 25° C. Calculate the temperature at which Keq is 4.0*10^3. delta G= (delta H) T(delta S) = 36  (298)(0.1588) = 11.32 delta G= RTlnK 11.32= 8.31Tln(4*10^3) 11.32= 6892.35

Chemistry!!!
Consider the rxn during the Haber Process: N2 + 3H2 > 2NH3 The equilibrium constant is 3.9 x 10^(5) at 300 K and 1.2 x 10^(1) at 500 K. Find Delta H reaction and Delta S for reaction

math
Compute delta(y) and dy for the given values of x and dx=delta(x) y=x^2 , x=8 , delta(x)=0.5 Delta(y)= ??? dy = ??? I got dy=8 by doing: dy= (f prime of x)dx dy=2xdx dy=2xdelta(x) dy=2*8*0.5 dy=8 but I have not clue how to find delta(y) please help! deltay

Chemistry(DrBob222)
So, i did this lab, a solubility and thermodynamics lab of KNO3, and in it we had to determine the delta h delta g and delta s, the question i have is what is the relationship of the signs delta h, delta s, and delta g, to the dissociation of the salt and

Chemistry
Given the Data: N2(g) + O2g) = 2NO(g) delta H = 180.7kj, 2NO(g) + O2(g) = 2NO2(g) delta H = 0113.1kj, 2N2O(g) = 1N2(g) + O2(g) delta H = 163.2kj. Using Hess’s Law calculate delta H for the reaction: N2O(g) + NO2(g) = 3NO(g)

Chemistry
Is this reaction endothermic or exothermic? AB > A+B a. Exothermic, ΔH rxn is positive. b. Endothermic, Delta ΔH rxn is negative. c. Endothermic, ΔH rxn is positive.

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.

calculus
correct me if I'm wrong please. 1. What is the value of Lim 2x+3/4x5 when x>00 (infinity?) a.3/5 b.0 c.1/2

chemistry
Calculate the enthalpy of change, Delta H of rxn, for each of the reactions. record the values in the data table part 2 I calculated the heat of rxn of the HCl +NaOHNaCl + H2O. How do i go from here to enthalpy of change

Chemistry URGENT! I really need help!
Consider the following reaction occurring at 298K BaCO3(s)> BaO(s) + CO2 (g) show that the reaction is not spontaneous under standard condition by calculating delta G rxn. I calculated delta G and got 219.7 kJ, now the question asks if BaCO3 is placed in

Dan
N2 + 3H2 > 2NH3 At 25°C (delta)Ho = 92.22 kJ and (delta)So = 198.53 J/K. Using this information, calculate the equilibrium constant for the reaction at 2.43x10^2°C. (R = 8.314 J/K) Apparently the way I'm doing it is wrong: I divide 198.53 by 1000

equibrium  help!
Consider the reaction CO(g) + H2O(g) CO2(g) + H2(g) Use the appropriate tables to calculate a) deltaG*f at 552*C b) K at 552*C I'm pretty sure I have a good idea of how to do this: I believe I can use GibbsHelmholtz equation to account for the

chem!
Calculate the heat of reaction for the incomplete combustion of 67.0g propane producing carbon monoxide gas and water vapour. how would I go about and do this question? What are you studying? Do you know how to use the thermodynamic tables (delta Ho, etc).

CHEMISTRY!!!!!!!!!!
Styrene is produced by catalytic dehydrogenation of ethyl benzene at high temperature in the presence of superheated steam. Given the following data, Ethylbenzene, C6H5CH2CH3 : delta Ht = 12.5 kJ/mol, delta Gt = 119.7 kJ/mol and S = 255 J/mol*K

Chemistry
The following reaction has the following standard thermodynamic parameters: Reaction: C(g) + D(g)> E(g) Delta H rxn=26.1kJ/mol and Delta S rxn=69.8J/(mol*K). Calculate the temperature at which the reaction becomes nonspontaneous.

Chemistry
Styrene is produced by catalytic dehydrogenation of ethyl benzene at high temperature in the presence of superheated steam. (a) Find ÄH°rxn, ÄG °rxn, and ÄS °rxn, given these data at 298 K: (b) At what temperature is the reaction spontaneous? What

Chem, LAST ONE PLEASE HELP!
consider the reaction: CO(aq) + Cl2 (aq) > COCl2 (aq). Calculate Delta G at non standard conditions. T = 298.15K. Concentration of COCl2 is reduced to 0.01832 M while the concentrations of CO and Cl2 remain 1M. Delta G rxn = 67.4 kj.

Physics
1. If the change in position delta(x) is related to velocity v (w/ units of m/s) in the equation delta(x)=Av, the constant A has which dimension? a. m/s^2 b. m c. s d. m^2 2. If a is acceleration (m/s^2), delta(v) is change in velocity (m/s), delta(x) is

CHEMISTRY
calculate the delta h for the reaction 2C+2H> C2H4 C+O2> Co2 delta h= 393.5 C2H4+ 3O2> 2CO2+ 2H2O delta h= 1410.9 H2+ 1/2 O2> H2O delta h= 285.8 2CO+ O2> 2CO2 delta h= 566.0 do you flip the first two equations and times the first and third one

Chem 2
for the evaporation of water during perspiration on a hot dry day 1.delta H is greater than zero and Tdelta S is equal to Delta H 2.delta H is greater than zero and Tdelta S is gretaer than Delta H 3.delta H is greater than zero and Tdelta S is less than

chem
calculate the delta Hf of c6h12o6 (s) from the following data: Delta H combustion= 2816 kj/mol delta Hf of Co2 = 393.5 kj/mol delta Hf= of H2 O= 285.9kj/mol

chemistry
Styrene is produced by catalytic dehydrogenation of ethyl benzene at high temperature in the presence of superheated steam. (a) Find ÄH°rxn, ÄG °rxn, and ÄS °rxn, given these data at 298 K: (b) At what temperature is the reaction spontaneous? What

chemistry
Styrene is produced by catalytic dehydrogenation of ethyl benzene at high temperature in the presence of superheated steam. (a) Find ÄH°rxn, ÄG °rxn, and ÄS °rxn, given these data at 298 K: (b) At what temperature is the reaction spontaneous? What

chemistry
Styrene is produced by catalytic dehydrogenation of ethyl benzene at high temperature in the presence of superheated steam. (a) Find ÄH°rxn, ÄG °rxn, and ÄS °rxn, given these data at 298 K: (b) At what temperature is the reaction spontaneous? What

Chemistry
A rxn has delta H ^0 rxn=112kj and delta S^0 rxn =354 J/K. at what temp is the change in entropy for the rxn equal to the change in entropy for the surroundings?

chemistry
Styrene is produced by catalytic dehydrogenation of ethyl benzene at high temperature in the presence of superheated steam. (a) Find ÄH°rxn, ÄG °rxn, and ÄS °rxn, given these data at 298 K: (b) At what temperature is the reaction spontaneous? What

Chemistry
Styrene is produced by catalytic dehydrogenation of ethyl benzene at high temperature in the presence of superheated steam. Given the following data, Ethylbenzene, C6H5CH2CH3 : delta Ht = 12.5 kJ/mol, delta Gt = 119.7 kJ/mol and S = 255 J/mol*K

College Chemistry
I was asked to find delta Grxn for the equation I2+Cl2>2ICl. Was given information to solve for Q (PICl= 2.55atm, PI2=0.315, PCl2=0.216), i ended up with 4.4588. Then I solved for the standard G rxn by: Delta G= (10.9*2) (19.3+0)= 41.1. I used the

Chemistry
I'm stuck...that is i believe I've come to an impossible answer: I need to calculate the equilibrium constant 4Fe(s) + 3O2(g) > 2Fe2O3(s) First off: Delta G G Fe(s) = 0, G O2(g) = 0, G Fe2O3(s) = 741 (x2) 741 (2)  0 = 1480 = delta G of reaction at

Chemistry
I'm stuck...that is i believe I've come to an impossible answer: I need to calculate the equilibrium constant 4Fe(s) + 3O2(g) > 2Fe2O3(s) First off: Delta G G Fe(s) = 0, G O2(g) = 0, G Fe2O3(s) = 741 (x2) 741 (2)  0 = 1480 = delta G of reaction at

Chem 141
Write the three thermochemical equations needed to calculate the delta H for the below reaction.? 2Mg(s) + O2(g) > 2 MgO(s) delta H rxn = ? (Include delta H values in kJ for each reaction)

Chemistry
Please help, I am having trouble solving these problems at nonstandard temperatures. Methanol burns in oxygen to form carbon dioxide and water. Using the balanced reaction, 2CH3OH(l) + 3OH2(g) > 2CO2(g) + 4H2O(g) 1) Calculate delta H(rxn) in kJ at 24

Chemistry(Please check answers)
1) For a reaction delta Go is more negative than delta Ho. What does this mean? a. delta So is zero. b. delta So is negative c. delta So is positive d. delta So is negative if delta Ho is positive. e. delta So is negative if delta Ho is negative. I think

Chemistry
The following reaction has the following standard thermodynamic parameters: Reaction: C(g) + D(g)> E(g) Delta H rxn=26.1kJ/mol and Delta S rxn=69.8J/(mol*K). Calculate the temperature at which the reaction becomes nonspontaneous.

Chemistry
The following reaction has the following standard thermodynamic parameters: Reaction: C(g) + D(g)> E(g) Delta H rxn=26.1kJ/mol and Delta S rxn=69.8J/(mol*K). Calculate the temperature at which the reaction becomes nonspontaneous.

Chemistry
I had to perform an experiment using a coffeecup calorimeter to determine the enthalpies of two separate reactions. For part 1 we worked with magnesium metal, and magnesium oxide. Data was collected and now I need to find the q, heat transferred for both

Chemistry
Why these answers are so? 1 For this reaction 2H2 + O2 = 2H2O a dela H=delta Hf bdelta Hc= delta Hf c delta H= delta Hc d delta S= delta H and the answer is b , but how and why? 2 For this reaction 2S + 3O2 = 2SO3 + 792 kJ which of the following

chem class
Our teacher told us we had to do problems on our final on Delta G and S...? all he said is we'd have to plug in numbers from a list and solve. but im very confused. but the numbers he gave in the example are different from my book, is there soemthing we

thermodynamics
A reaction has deltaHrxn=127 kJ and delta S rxn=314 J/K. At what temperature is the change in entropy for the reaction equal to the change in entropy for the surroundings? so I made delta HT delta S=0 plugged in values for S and H and solved for T. I got

science please!
Estimate the value of the cell potential for the following rxn: Mn02(s) + 4H30+(pH=3.8) + 2Ag(s) > Mn2+(aq, .1M) + 6H20(l) I got Ecell=.48V delta G circle= 92640 J/mol and delta g = 107484 is this correct?

Chem
Does my work here look right? 3. One mole of an ideal gas expands adiabatically into a vacuum. Calculate q, deltae, w, and deltaH for the process. q= 0 [adiabatic] w= Pext(V2V1) w= 0 deltae = w + q deltae = 0 + 0 = 0 deltah= deltae + P(delta V)

Chemistry
Consider the rxn during the Haber Process: N2 + 3H2 > 2NH3 The equilibrium constant is 3.9 x 10^(5) at 300 K and 1.2 x 10^(1) at 500 K. Find Delta H reaction and Delta S for reaction

Chemistry
Please explain. The enthalpy changes for two different hydrogenation reactions of C2H2 are: C2H2+H2>C2H4 Delta H 1 C2H2+2H2>C2H6 Delta H 2 Which expression represents the enthalpy change for the reaction below? C2H4+H2>C2H6 Delta H = ? A. Delta

Chemistry
Hydrogen peroxide is used as a bleachin agent, a disinfectant and medicinally as a topical antibacterial agent. Hydrogen peroxide decomposes according to the reacton 2H^2O^2(l)>2H^2O(l)+o^2(g) A. Given the standard free energy of formation values shown

chemistry
consider the reaction: CO (aq) + Cl2 (aq) > COCL2 (aq). Calculate Delta G at non standard conditions for the reaction at 298.15k, if the concentration of COCl2 is reduced to 0.01832M, while the concentrations of CO and cl2 remain at 1M. Delta G rxn =

chemistry
calculate the delta G rxn O2(g)+2 H2o(l)+2 Cu(s)> 4 OH(aq)+2 Cu^2+(aq)

chemsitry
calculate Delta H of RXN 2 N2 (g) + 3 H2( g) >2 NH3 (g)

Chemistry
2M +6HCl–>2MCl+3H2 Delta H= 638.0 Kj HClg—>HCl aq= Delta H 74.8 Kj H2+Cl2–>2HCl Delta H 1845.0 Kj MCl3s–> MCl3 aq Delta H 249.0 Kj Use the information above to determine the enthalpy of the following reaction. 2M +3Cl2–>2MCl3 Delta H =???

Chemistry
I know I posted this question before, but can you clarify it?? MY QUESTION IS AFTER YOU SWITCHED THE DELTA H1 THE CHANGE IN THE ENTHALPY IS NEGATIVE.... BUT THAT DOES NOT MAKE SENSE BECAUSE THE CHANGE IN ENTHALPY OF THE ORIGINAL DELTA H1 IS

CHEMISTRY
I know I posted this question before, but can you clarify it?? MY QUESTION IS AFTER YOU SWITCHED THE DELTA H1 THE CHANGE IN THE ENTHALPY IS NEGATIVE.... BUT THAT DOES NOT MAKE SENSE BECAUSE THE CHANGE IN ENTHALPY OF THE ORIGINAL DELTA H1 IS

Valid statements
Determine which statement follows validly from the statements included. 1) If Delta is an alpha, then Delta is a beta. If Delta is a theta, then Delta is a beta. Either Delta is an alpha or Delta is a theta. Therefore, Delta is ... 2)Either Delta is an

chem
Calculate delta G rxn for a redox reaction with n = 2 that has an equilibrium constant of K = 4.4×10−2.

Chemistry, PPPLLEASE Help!
Hello, I'm confused on what these problems are telling me. Is questions a) and b) the same? I don't know, please help me I don't know what to do... The inteconversion of DHAP and G3P is a part of both the glycotic pathway and the Calvin cycle for

Chemistry(Please help)
1) Nitrosyl chloride (NOCl) decomposes at high temperature. The equation is 2 NOCl (g) > 2 NO (g) + Cl2 (g) at 227oC Using delta Ho = 81.2 kJ and delta So = 128 J/K, calculate the value of the equilibrium constant for this reaction. I do not know how to

Chemistry
Given the thermodynamic data in the table below, calculate the equilibrium constant for the reaction: 2SO2(g)+O2> 2SO3 Substance (DeltaH^o) (Delat S^o) SO2 297 249 O2 0 205 SO3 395 256 Answer (it was given) 2.32x10^24 Even though the answer is given

physics
How can the alternative definition of power: P = \frac{w}{\Delta t} = F \frac{d}{\Delta t} ... can be derived by substituting the definitions of work and speed into the standard definition of power, P =\frac{W}{\Delta t}. (Equations written without latex

Chemistry
The following standard free energies are given for 25 degrees celcius. 1) N2(g) + 3H2(g)> 2NH3(g) delta g = 33.0 kJ 2) 4NH3(g) + 5O2(g)> 4NO(g) + 6H20() delta g = 1010.5 kJ 3) N2(g) + o2(g)> 2NO(g) delta g = 173.1kJ 4) N2(g) + 2O2(g) > 2NO2(g) delta

chemistry
Is delta Tf = delta Tb? The original practice problem is Detla Tf= 8.631 for an aqueous solution, what is delta Tb. I know that Delta Tf=Kf*m

Chemistry
A critical reaction in the production of energy to do work or drive chemical reactions in biological systems is the hydrolysis of adenosine triphosphate, ATP, to adenosine diphosphate, ADP, as described by ATP(aq)+H20(l)>ADP(aq)+HPO4^2(aq) for which

Chemistry
How do I find the equilibrium constant for 4NH3(g) + 5O2(g) > 4NO(g) + 6H2O(g) at 825 degrees celcius, assuming that delta H and delta S knot do not depend on temperature, and Delta H is 908 KJ and Delta S is 1206 KJ?

Chemistry II
Saw this one already answered, but did not understand at all... Calculate the delta Hf of C6H12O6 (s) from the following data: Delta H combustion= 2816 kj/mol delta Hf of Co2 = 393.5 kj/mol delta Hf= of H2 O= 285.9kj/mol

Chemistry
I am having trouble with this equation and calculating the enthalpy of formation. 2 NaHCO3 (s) > Na2CO3 (s) + H2O (g) + CO2 (g) delta H129.2kj I get as far as this step and then I don’t know what to do next. delta H= [1*delta H (Na2CO3) + 1* delta

Chemistry
Consider the following reaction occurring at 298K BaCO3(s)> BaO(s) + CO2 (g) show that the reaction is not spontaneous under standard condition by calculating delta G rxn. I calculated delta G and got 219.7 kJ, now the question asks if BaCO3 is placed in

CalculusSolved  Incorrect
calculate delta y for f(x)= x^(3/2) with x= 4 and delta x= dx=0.1 delta y= f(x+delta x) f(x) = f(4.1)  f(4) delta y= f(4.1)8 f(x + delta x)= 8 + 3/2*x^(1/2)*0.1 = 8 + 0.15x^(1/2) = 8 + 0.30 = 8.30 delta y= 8.30  8 delta y= 0.30 but this is wrong. why

Chemistry
Na reacts violently with H2O to produce NaOH and H2. The resulting solution has a higher T than it did before the Na was added. What are the expected changes? deltaH ? deltaS >0 deltaG 0 I know the last three for a fact. Is deltaG "

Chem
I don't believe I'm getting the correct answers for this problem. Could someone look over my work and verify whether it is correct or not? One mole of an ideal gas (Cv = 3/2R) at 300. K expands adiabatically against a constant external pressure of 2.00 atm

uconn
calculate delta h delta s and delta g for the transfer of methan from a nonpolar solvent to water at 298 kelvin temperature.

Chemistry
I need to calculate the value of Kp at 25 degrees celsius using the delta Go value. Delta Go = 29.10kJ I know that Delta Go = RT lnK and that R=8.314e3kJ/K mol delta Go / RT I did 29.10 / 8.314e3 X 298K and 11.74 but this was wrong. I am stuck. What

Chemistry
Calculate the S(univ) for the following phase change at 25 deg celcius. The boiling point of heptane is 98.0 Celcius and has a Delta Hvap= +21.6kj/mol. C7H16(l)> C7H16(g) Delta S= +79.0j/k I know that the equation is Delta Suniv= DSsys + DSsurr PLEASE

Chemistry
1)Which thermochemical equation and data does not agree with the other two written? a) 2NO (g)+ O2 (g) >2 NO2 (g) deltaH=169.8 b) NO (g) + 1/2 O2 (g) > NO2 (g) delta H = 56.6 c) 4 NO2 (g) > 4 NO (g) + 2 O2 (g) delta H = +226.4 d)all three equations

Chemistry(Please help)
delta Go = 431.16kJ/mol  (298k X 0.12529 kJ/K*mol) I am having trouble converting the units for delta H and delta s to match. I multiplied delta H by 1000 to get kJ but this didn't give me the correct answer.

math
I really dk how to do them,i have spend hours doing it Can somebody please solve and if possible show the steps thx,just 3 questions __ 3)Given that tan theta = ✓3 and that 90 degree ≤ delta ≤ 180 degree,find the value of: a) tan delta b)cos delta

Chemistry(Please check)
Delta G^o for a reaction can be calculated from? 1. delta G^o f data 2. Delta H^o f and delta S data 3. equilibrium constants I chose that delta G can be calculated from H and S values. Would you agree?

Chemistry
Calculate the enthalpy of the reaction 2B2H6 + 6O2=2B2O3 +6H2O given the following pertinent information: A. B2O3(s) + 2H2) )g) = 3O2 (g) + B2H6 (g), delta H= +2035kJ B. 2B (s) + 3H2 (g) =B2H6 (g), delta H= +36 kJ C. H2 (g) + 1/2)2 (g) =H2O (l), delta

Mike
N2 + 3H2 > 2NH3 At 25°C (delta)Ho = 92.22 kJ and (delta)So = 198.53 J/K. Using this information, calculate the equilibrium constant for the reaction at 2.43x10^2°C. (R = 8.314 J/K) Apparently the way I'm doing it is wrong: I divide 198.53 by 1000

Chem
CH4(g)+2O2 arrow CO2(g)+2H2O(1) delta H=890.3kJ. Calculate delta Hwhen 5 grams of methane react with an excess of oxgen?o i just divide Delta H by 5?