(I) The equilibrium partial pressure of NO in the reaction N2(g) + O2(g) ⇌ 2 NO(g) at 800
K is 3.0 x 10-6 Pa. What are the partial pressures of N2 and O2 at equilibrium if K = 3.4 × 10-21 at 800 K?
(II) How should the total volume of the following equilibrium reaction mixture be changed to increase the amount of CO2(g)? C(s) + CO2(g) ⇌ 2 CO(g)
A) Total volume should decrease.
B) Total volume should remain the same.
C) There is insufficient information given.
D) Total volume should increase.
(III) Consider the reaction A (aq) + 3 B (aq) ⇌ 2 NH3 (g). If we have 1.0 L and K = 9, calculate Q if the volume is increased to 10.0 L.