Question

From the information on deltafH and deltafG , provided in the data section calculate the standard...

From the information on deltafH and deltafG , provided in the data section calculate the standard Gibbs energy of reaction, deltarG , and the equilibrium constant, K, at: (a) 25 °C and (b) 50 °C for the chemical reaction: CH4(g) + 3 Cl2(g) -><-CHCl3 (l) + 3 HCl (g). Assume that the reaction enthalpy is independent of temperature.

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

CH4(g) + 3Cl2(g) --------------- CHCl3(l) + 3 HCl(g)

G0rxn =[ G0f of CHCl3 + 3 xG0f of HCl] - [ G0f of CH4+3xG0f of Cl2]

G0rxn = [- 73.66 + 3x(-95.31)] - [ (-50.84)+3x0.0]

G0rxn = - 308.75KJ

Gibbs free energy change = G0 = - 308.75KJ

a) at 25C

T= 25+273= 298K

G0rxn = - RTlnK

R= 8.314x10^-3KJ

- 308.75 = - 8.314x10^-3 x298xlnK

lnK = 124.62

K = e^124.62

K= 1.32x10^54.

b) at 50C

T= 50+273= 323K

- 308.75 = - 8.314x10^-3 x323xlnK

lnK = 114.97

K= e^114.97

K= 8.53x10^49.

0 0
Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
1. The rate law for the reaction is: Cl2(g) + CHCl3 (g) = HCl (g) +...
1. The rate law for the reaction is: Cl2(g) + CHCl3 (g) = HCl (g) + CCl4 (g) Is Rate = k [Cl2]^1/2 [CHCl3] What are the units for k, assuming time inow seconds and concentration in mol/L 2. What is the unit for the rate of a chemical reaction and the rate constant for a third-order rate law?
The chemical reaction that causes iron to corrode in air is given by 4Fe+3O2→2Fe2O3 in which...
The chemical reaction that causes iron to corrode in air is given by 4Fe+3O2→2Fe2O3 in which at 298 K ΔH∘rxn = −1684 kJ ΔS∘rxn = −543.7 J/K Gibbs free energy (G) is a measure of the spontaneity of a chemical reaction. It is the chemical potential for a reaction, and is minimized at equilibrium. It is defined as G=H−TS where H is enthalpy, T is temperature, and S is entropy. Part A What is the standard Gibbs free energy for...
± Gibbs Free Energy: Temperature Dependence Gibbs free energy (G) is a measure of the spontaneity...
± Gibbs Free Energy: Temperature Dependence Gibbs free energy (G) is a measure of the spontaneity of a chemical reaction. It is the chemical potential for a reaction, and is minimized at equilibrium. It is defined as G=H−TS where H is enthalpy, T is temperature, and S is entropy. The chemical reaction that causes aluminum to corrode in air is given by 4Al+3O2→2Al2O3 in which at 298 K ΔH∘rxn = −3352 kJ ΔS∘rxn = −625.1 J/K Part A What is...
Calculate the standard entropy, ΔS°rxn, of the following reaction at 25.0 °C using the data in...
Calculate the standard entropy, ΔS°rxn, of the following reaction at 25.0 °C using the data in this table. The standard enthalpy of the reaction, ΔH°rxn, is –633.1 kJ·mol–1. 3C2H2(g)==>C6H6(l) Delta S rxn = Then calculate the standard gibbs free energy of the reaction Delta G rxn Delta G rxn=
Furamate + H2O <--> malate . At 25 degrees celsius the equilibrium constant K= (activity Malate/activity...
Furamate + H2O <--> malate . At 25 degrees celsius the equilibrium constant K= (activity Malate/activity furamatete)=4.0. The activity of malate and furamate are defined on the molatiry concentration scale (a=c in a dilute solution) a) What is the standard Gibbs free energy change for the reaction at 25 degrees celsius. b) What is the Gibbs free energy change for the reaction at equilibrium? c) What is the Gibbs free energy change when 1 mol of 0.1M furamate is converted...
Calculate the standard molar Gibbs free energy change (DeltaGrxn0) at 298 K and at 400 K...
Calculate the standard molar Gibbs free energy change (DeltaGrxn0) at 298 K and at 400 K for the following reaction (the cyclotrimerization of ethene to benzene), assuming that all heat capacities are independent of temperature:                                     3 C2H4(g)   ®   C6H6(g) + 3 H2(g).
6A) Consider the following reaction: 2CH2Cl2(g) CH4(g) + CCl4(g) If 0.432 moles of CH2Cl2(g), 0.263 moles...
6A) Consider the following reaction: 2CH2Cl2(g) CH4(g) + CCl4(g) If 0.432 moles of CH2Cl2(g), 0.263 moles of CH4, and 0.590 moles of CCl4 are at equilibrium in a 17.7 L container at 576 K, the value of the equilibrium constant, Kc, is 6B)Consider the following reaction: COCl2(g) CO(g) + Cl2(g) If 3.59×10-3 moles of COCl2, 0.265 moles of CO, and 0.211 moles of Cl2 are at equilibrium in a 12.3 L container at 772 K, the value of the equilibrium...
A. Using given data, calculate the change in Gibbs free energy for each of the following...
A. Using given data, calculate the change in Gibbs free energy for each of the following reactions. In each case indicate whether the reaction is spontaneous at 298K under standard conditions. 2H2O2(l)→2H2O(l)+O2(g) Gibbs free energy for H2O2(l) is -120.4kJ/mol Gibbs free energy for H2O(l) is -237.13kJ/mol B. A certain reaction has ΔH∘ = + 35.4 kJ and ΔS∘ = 85.0 J/K . Calculate ΔG∘ for the reaction at 298 K. Is the reaction spontaneous at 298K under standard conditions?
HgO(s) Hg(g) O2(g) Enthaply Delta H kj/mol -90.8 61.3 Entropy Delta S   j/mol. K 70.3 174.9...
HgO(s) Hg(g) O2(g) Enthaply Delta H kj/mol -90.8 61.3 Entropy Delta S   j/mol. K 70.3 174.9 205.0 Above is a table of thermodynamics date for the chemical species in the reaction: 2HgO(s) ----> 2Hg(g)+ O2(g) at 25 C A) Calculate the molar entropy of reaction at 25 C B) Calculate the standard Gibbs free enregy of the reaction at 25 C given that the enthaply of reaction at 25 C is 304.2 Kj/mol C)Calculate the equilibrium constant for the reaction...
Given the following information, calculate the standard Gibbs free energy of the reaction at 1455 K....
Given the following information, calculate the standard Gibbs free energy of the reaction at 1455 K. State if the reaction is spontaneous or nonspontaneous followed by the temperature at which the reaction switches spontaneity if applicable. CaCO3(s) --> CaO(s) + CO2(g) Given: Δ°H = 179.2 kJ , Δ°S = 160.2 J/K
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT