Answer to Question #287532 in General Chemistry for jordan carter

Question

1.) Write the equilibrium expression and calculate the K_eq for H₂ (g) + CS₂ (g) ⇌ CH₄  (g) + 2 H₂S (g)   

Concentrations at equilibrium:

[CH₄] = [H₂S] = 1.3 x 10^-2 mol/L

[H₂] = 4.4 x 10^-1 mol/L

[CS₂] = 1.1 x 10^-3 mol/L

2.) When acetic acid reacts with water, these equilibrium concentrations are found. [CH₃COOH] = 0.20mol/L, [CH₃COO^-] = 0.0019mol/L, [H₃O⁺] = 0.0019mol/L. The equation for the reaction is

CH₃COOH (aq) +   H₂O (ℓ)  ⇌  CH₃COO^-  (aq) + H₃O⁺  (aq)

What is the equilibrium constant expression for this reaction and what is the value of the equilibrium constant? 

3.) Calculate the [NO₂] for

2 NO (g) + O₂ (g) ⇌  NO₂  (g)     

If [NO] = 4.00 x 10^-3 mol/L and [O₂] = 2.00 x 10^-3 mol/L at equilibrium, and the equilibrium constant is 2.34 x 10^-2 at 500°C. 

Answer 1

1. Equilibrium expression

$4H_2 (g) + CS_2 (g) ⇌ CH_4 (g) + 2 H_2S (g)$

$K_{eq}$