Chemical Equilibrium

Which one of the following statements does not describe the equilibrium state?

a. While at equilibrium, a dynamic process is still occurring.  

b. The concentration of the reactants is equal to the concentration of the products.

c. The concentration of the reactants and products reach a constant level.

d. At equilibrium, the net concentration of all species is not changing.

e. All are true.

State which is greater in amount:reactants or products, based on the given equilibrium constant, K. 

The decomposition of nitrogen monoxide can be achieved under high temperatures to create the products of nitrogen and oxygen gas. 

6 NO(aq) ⇌ 3 N₂(aq) + 3 O₂(aq) 

a) What is the equilibrium equation for the reaction above?

b) What is the equilibrium expression for the reverse reaction. 

The equilibrium constant, K, for 2 NO (g) + O₂ (g) ⇌ 2 NO₂ (g) is 6.9 x 10². 

What is the [NO] in an equilibrium mixture of gaseous NO, O₂, and NO₂ at 500 K that contains 1.5 x 10 ^–2 M O₂ and 4.3 x 10 ^–3 M NO₂?

In which of the given reactants is K_p greater than, less than and equal to K_c?

a) SO₃ (g) + NO (g) ⇌ SO₂ (g) + NO₂ (g)

b) P₄ (s) + 5 O₄ (g) ⇌ P₄O₁₀ (s)

c) 4 NH₃ (g) + 3 O₂ (g) ⇌ 2 N₂ (g) + 6 H₂O (g)

Given the hypothetical reaction 2 A (s) + ? B (g) ⇌ 3 C (g), Kp = 0.0105 and Kc = 0.45 at 250 degrees Celsius. What is the value of the coefficient of B? 

CH₄ (g) + 2 H₂S (g) ⇆ CS₂ (g) + 4 H₂ (g)

For the reaction:N₂ (g) + 2 O₂ (g) ⇌ 2 NO₂ (g), K_c = 8.3 x 10 ^-10 at 25^°C. What is the concentration of N₂ gas at equilibrium when the concentration of NO₂ is twice the concentration of O₂ gas?

At a given temperature the gas phase reaction:N₂ (g) + O₂ (g) ⇌ 2 NO (g) has an equilibrium constant of 4.00 x 10 ^-15. What will be the concentration of NO at equilibrium if 2.00 moles of nitrogen and 6.00 moles oxygen are allowed to come to equilibrium in a 2.0 L flask.

2 SO₃ (g) ⇆ 2 SO₂ (g) + O₂ (g)

2 NO (g) + O₂ (g) ⇆ 2 NO₂ (g)

what is K_c for the reaction shown below?

4 NO₂ (g) ⇆ 4 NO (g) + 2 O₂ (g)

N₂ (g) + O₂ (g) ⇆ 2 NO (g)

2 SO₃ (g) ⇆ 2 SO₂ (g) + O₂ (g)

Consider the reaction below:

CH₄ (g)  +  F₂ (g)  ⇌  CF₄ (g)  + HF (g)   H = + 38.1 KJ/mol

The following changes will shift the equilibrium to the left except one. Which one would not cause a shift to the left?

The following data was collected for the following reaction at equilibrium 

2 A (g) + 3 B (g)  ⇌ C (g)     

At 25 ^oC K is 5.2 x 10^-4 and at 50 ^oC K is 1.7 x 10^-7. Which of the following statements is true?

a) The reaction is exothermic.

b) The reaction is endothermic.

c) The enthalpy change, ΔH, is equal to zero.

d) Not enough information is given. 

Which direction will the following reaction (in a 10.0 L flask) proceed if a catalyst is added to the system? 

CaCO₃ (s)  ⇌ CaO (s) + CO₂ (g)            K_p = 3.2 x 10^-28

Consider the following gas reaction of A₂ ( shaded spheres) and B₂ ( unshaded spheres)

A₂ (g)  +  B₂ (g)  ⇌  2 AB (g) 

Which container proceeds more to completion? 

H₂ (g) + I₂ (g) ⇆ 2 HI (g)      ΔH = –9.42 kJ

CO (g) + H₂O (g) ⇆ CO₂ (g) + H₂ (g)

H₂ (g) + I₂ (g) ⇆ 2 HI (g)

I₂ (g) ⇆ 2 I (g)

After the reaction reaches equilibrium, an inert gas is introduced into the container under conditions of constant volume. Which of the following would you expect to happen?