NH₄HS(s) <==> NH₃(g) + H₂S(g) ΔH_RXN > 0

A sealed rigid vessel contains NH₄HS(s) in equilibrium with NH₃(g) and H₂S(g)as represented by the equation above.

Which of the following changes will increase the amount of NH₄HS(s) in the vessel?

HgO(s) + 4 I− + H2O ⇄ HgI42− + 2 OH− ∆H < 0

Consider the equilibrium above.

Which of the following changes will increase the concentration of HgI₄²⁻?

What is the effect of increasing the pressure on the following reaction:

2NO + O₂ ---> 2NO₂?

Forward reaction is favored when

When the reaction is reversed,

When two reactions are added, then their equilibrium constants are:

The reaction 2 SO₂(g) + O₂(g) ↔ 2 SO₃(g) has an equilibrium constant of K₁. What is the K value for the reaction

SO₃(g) ↔ SO₂(g) + 1/2 O₂(g)?

What is the value for the reaction N₂(g) + 2O₂(g) ↔ N₂O₄(g) in terms of the K values for the following reactions:

1/2 N₂(g) + 1/2 O₂(g) ↔ NO(g) K₁

2 NO(g) + O₂(g) ↔ N₂O₄(g) K₂

If the solubility of MgCO₃ is represented by s, which expression is equal to the K_sp?

If the solubility of Ag₂CO₃ is represented by s, which expression is equal to the K_sp?

For the reaction,

CO₂(g) + 4 H₂(g) ↔ CH₄(g) + 2 H₂O(g),

K = 8.2 x 10¹⁹ at 25°C.

Initially CO₂(g) and H₂(g) are 1.0atm at 25°C in an evacuated container, which substance will have the highest pressure when the system is at equilibrium?

C(s) + H₂O(g) ↔ H₂(g) + CO(g)

ΔH° = +131 kJ/mol

Which stress will INCREASE the value of the equilibrium constant, K?

C(s) + H₂O(g) ↔ H₂(g) + CO(g)

ΔH° = 131 kJ/mol

Which change will increase the [H₂(g)] without affecting the value of K?