Question 13A N2(9) + O2(g) 2 NO(g) K = 1.0 x 10-30 At 720 C, the reaction represented above has an equilibrium constant of 1.0 x 1030 which of the following mathematical expressions can be used to support the claim that the reaction is not thermodynamically favored under these conditions? AG" Tan= -8.314 x (720 + 273) x In(1.0x10) >0 A 1,000 AGn = -0.08206 x (720 + 273) x In(1.0 x 1030) x 1, 000 > 0 8.314 x 720 x ln(1.0x10) AG 1.000 D AG an = 0.08206 x (720 + 273) x In(1.0 x 10-30) x 1,000 < 0

Question 13A N2(9) + O2(g) 2 NO(g) K = 1.0 x 10-30 At 720 C, the reaction represented above has an equilibrium constant of 1.0 x 1030 which of the following mathematical expressions can be used to support the claim that the reaction is not thermodynamically favored under these conditions? AG" Tan= -8.314 x (720 + 273) x In(1.0x10) >0 A 1,000 AGn = -0.08206 x (720 + 273) x In(1.0 x 1030) x 1, 000 > 0 8.314 x 720 x ln(1.0x10) AG 1.000 D AG an = 0.08206 x (720 + 273) x In(1.0 x 10-30) x 1,000 < 0

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

The equilibrium constant, Kp, for the following reaction is 2.20×104 at 723 K. ? 2NH3(g) N₂(g) + 3H₂(g) If AH° for this reaction is 111 kJ, what is the value of Kp at 819 K? Kp = Submit Answer Retry Entire Group 9 more group attempts remaining
Interconvert K and K values. Calculate Ko for the following reactions at the indicated temperature. (a) 2 NOCI(g) 2 NO(g) + Cl₂(g) K = 2.69x10-³ at 560 K Kp = (b) NHAl(s)NH₂(g) + HI(g) Kc = 5.59×10-4 at 634 K Kp =
The equilibrium constant for the following reaction is 260 at -1 °C. 2 NO(g) + Br₂(g) 2 NOBr(g) K 260 at -1 °C - Calculate the equilibrium constant for the following reactions at -1 °C. (a) 2 NOBr(g) (b) NOBr(g) ? 2 NO(g) + Br₂(g) NO(g) + 1/2 Br₂(g) K = K =
Consider the following reaction: CO (g) + 2 H₂ (9) CH3OH (g) A reaction mixture in a 5.21 - L flask at a certain temperature initially contains 27.4 g CO and 2.36 g H₂. At equilibrium, the flask contains 8.65 g CH3OH. Calculate the equilibrium constant (K) for the reaction at this temperature. Kc = Submit ΠΑΠ ΑΣΦ 4 Request Answer ?
The equilibrium constant, Kp, for the following reaction is 1.04x102 at 548 K. Calculate Kc for this reaction at this temperature. NH4CI(s) NH3(g) + HCl(g)
Please don't provide handwritten solution ....
Question 3: Now try to solve this problem. The following system is allowed to reach equilibrium: N2(g) + 202(g) = 2 NO2(g) At equilibrium, [N2] = 0.45 M, [02] = 0.80 M and [NO2] = 0.75 M. Calculate the equilibrium constant.
7 4 (a) Calculate the value of Kc for the reaction: PC15 (2) PC13 (g) + Cl2 (g) AH = Positive Given that when 8.4 mol of PCls (g) is mixed with 1.8 mol of PC13 (g) and allowed to come to equilibrium in a 10 dm³ container the amount of PCls (g) at equilibrium is 7.2 mol. Kc = (b) Explain the effect of the following changes below on the value of Kc: (1) Increasing temperature (ii) Lowering the concentration of chlorine (Cl2) (iii) Addition of a catalyst
Find the attached image to answer the question.
7
Which of the following is correct concerning the following system at equilibrium at 298 K? A+B=C+ D A) AG = 0 AH° = +500 kJ/mol %3D B) AG° = 0 C) AG° < 0 D) The reaction is exothermic. K = 1x 10-10 E) This is a product-favored reaction.
The reaction below has a Kc value of 1.0 x 10 12 What is the value of Kp for this reaction at 300 K? 2 SO 2( 9) +O 2(g) 2 SO 3( g)