For a process at 451 k and constant pressure, Delta S_surr is -326 JK^-1. Calcul

Question

For a process at 451 k and constant pressure, Delta S_surr is -326 JK^-1. Calculate the quantity of heat (in kJ) absorbed by the system. a. 2.5 times 10^3 b. 3.1 times 10^2 c. 1.5 times 10^2 d. cannot be determined e. none of the above For the reaction of C(s) + H_2O(g) rightarrow CO(g) + H_2(g) Delta H degree = 131.3 kJ/mol and Delta S degree = 133.6 J/Kmol at 298K. At which temperature does the reaction become spontaneous? a. 273 b. 325 c. 552 d. 710 e. 983 The equilibrium constant for reaction is 48 at 25 degree C. What is the value of Delta G degree (kJ/mol) at this temperature? a. 1.8 b. -4.2 c. 1.5 times 10^2 d. 4.2 e. none of the above When a reaction is at equilibrium, which of the following statements is true? a. Delta G = Delta G b. ln K_eq = 0 c. Delta G degree = 0 d. Q = 0 e. Delta G = 0 ________is reduced in the following reaction: Cr_2O_7^2- + 6s_2O_3^2- + 14H^+ rightarrow 2 Cr^3+ + 3S_4O_6^2- + 7H_2O a. Cr_2O_7^2- b. S_2O_3^2- c. H^+ d. Cr^3+ e. S_4O_6^2- Given the following half reaction table, answer questions 10-11. F_2(g) + 2e^- rightarrow 2F^- (aq) +2.87 V Ag^+(aq) + e^- rightarrow Ag(s) +.80 V I_2(s) + 2e^- rightarrow 2I^-(aq) +.54 V Pb^2+ (aq) + 2e^- rightarrow Pb(s) -.126 V Li^+(aq) + e^- rightarrow Li(s) -3.05 V Which of the following is most likely to be a good oxidizing agent? A. F_2 b. Ag^+ c. Li d. Pb e. None of the above

Explanation / Answer

5)

Ssurr = -Qsys/T

-326 J/K = -Qsys / 451

Qsys =147026 J

Qsys =147 KJ

Answer: 1.5*10^2 KJ

6)

Ho = 131.3 KJ/mol = 131300 J/mol

So = 133.6 J/K.mol

The reaction become spontaneous when Go = 0

use:

Go = Ho - T*So

0 = 131300 - T*133.6

T = 983 K

Answer: 983

I am allowed to answer only 1 question at a time

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