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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

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

Introductory Chemistry: A Foundation
Introductory Chemistry: A Foundation
9th Edition
ISBN:9781337399425
Author:Steven S. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Donald J. DeCoste
Chapter17: Equilibrium
Section: Chapter Questions
Problem 10CR: . Explain what it means that a reaction has reached a state of chemical equilibrium. Explain why...
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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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