For numbers 10-12, consider the reversible reaction: 2SO2(g) + O2(g) → 2SO3(g) Kc = 4.3 x 10^6 at T = 700 K 10. The correct equilibrium constant (Kc) expression for the reaction is A. [SO2]^2 / [SO3]^2[O2] B. [SO3]^2 / [SO2][O2] C. [SO3]^2 / [SO2]^2[O2] D. [SO2]^2[O2] / [SO3]^2 11. Calculate the equilibrium concentration of SO3 given the equilibrium concentrations of each species as follows: [SO2] = 0.085 M, [O2] = 0.065 M. A. 1.05 x 10^-5 M B. 1.61 x 10^-4 M C. 44.94 M D. 1.54 x 10^2 M 12. Calculate the gas-phase equilibrium constant (Kp) for the reaction. R = 0.0821 (L · atm)/(mol · K) A. 7.48 x 10^4 B. 4.30 x 10^6 C. 2.47 x 10^8 D. 1.42 x 10^10
For numbers 10-12, consider the reversible reaction: 2SO2(g) + O2(g) → 2SO3(g) Kc = 4.3 x 10^6 at T = 700 K 10. The correct equilibrium constant (Kc) expression for the reaction is A. [SO2]^2 / [SO3]^2[O2] B. [SO3]^2 / [SO2][O2] C. [SO3]^2 / [SO2]^2[O2] D. [SO2]^2[O2] / [SO3]^2 11. Calculate the equilibrium concentration of SO3 given the equilibrium concentrations of each species as follows: [SO2] = 0.085 M, [O2] = 0.065 M. A. 1.05 x 10^-5 M B. 1.61 x 10^-4 M C. 44.94 M D. 1.54 x 10^2 M 12. Calculate the gas-phase equilibrium constant (Kp) for the reaction. R = 0.0821 (L · atm)/(mol · K) A. 7.48 x 10^4 B. 4.30 x 10^6 C. 2.47 x 10^8 D. 1.42 x 10^10
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...
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For numbers 10-12, consider the reversible reaction: 2SO2(g) + O2(g) → 2SO3(g)
Kc = 4.3 x 10^6 at T = 700 K
10. The correct equilibrium constant (Kc) expression for the reaction is
A. [SO2]^2 / [SO3]^2[O2]
B. [SO3]^2 / [SO2][O2]
C. [SO3]^2 / [SO2]^2[O2]
D. [SO2]^2[O2] / [SO3]^2
11. Calculate the equilibrium concentration of SO3 given the equilibrium concentrations of each species as follows: [SO2] = 0.085 M, [O2] = 0.065 M.
A. 1.05 x 10^-5 M
B. 1.61 x 10^-4 M
C. 44.94 M
D. 1.54 x 10^2 M
12. Calculate the gas-phase equilibrium constant (Kp) for the reaction. R = 0.0821 (L · atm)/(mol · K)
A. 7.48 x 10^4
B. 4.30 x 10^6
C. 2.47 x 10^8
D. 1.42 x 10^10
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