At 445 ºC calculate the equilibrium concentration of HI when 0.500 M HI, 0.0200 M H₂, and 0.0200 M I₂ are placed in a sealed flask and allowed to reach equilibrium. K_c for this reaction is 50 at 445 ºC.
H₂ (g) + I₂ (g) ⇆ 2 HI (g)

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)

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?

Select correct answer(s) that would yield more products in the following reaction.

CH₄(g) + 4 F₂(g) ⇌ CF₄(g) + 4 HF(g)     ΔH = 38.2 kJ/mol

a) increase pressure                          c) add 0.31 moles of F₂                   e) cool down reaction vessel
b) increase temperature                    d) add some Xenon gas                  f) decrease volume

At 26°C K_p = 2.3 x 10^–12 and at 56°C K_p = 3.7 x 10^–5 for the hypothetical reaction. Determine if the reaction is endothermic or exothermic.

AB(s) + 2 B(g) ⇌ 3 BB (g) + C (g)

When lead(IV) oxide is heated above 300°C, it decomposes according to the reaction, 2 PbO₂(𝑠) ⇌ 2PbO(𝑠) + O₂(𝑔). Consider the two sealed vessels of PbO₂ shown here. If both vessels are heated to 400°C and allowed to come to equilibrium, which of the following statements is or are true? (c) The amount of PbO₂ remaining in each vessel will be the same. [Find more in Section 15.4]