16. Chemical Equilibrium

The reaction: 2 NO(g) + Br₂(g) ⇌ 2 NOBr(g), has a K_p of 2.5 x 10² at 35°C. Calculate the equilibrium concentration of NOBr, if equilibrium concentrations of NO and Br₂ are 0.2 atm and 0.050 atm, respectively.

For the reaction below, K_c = 1.5 at a constant temperature. A 3.2 L flask contains an equilibrium mixture of 3 compounds: 3.7 g of NH₄HS, 70. g of NH₃ and unknown amount of H₂S. What is the mass (grams) of H₂S produced at equilibrium?

NH₄HS(s) ⇌ NH₃(g) + H₂S(g)

The diagram shown here represents the equilibrium state for the reaction A2(𝑔) + 2B(𝑔) ⇌ 2AB(𝑔). (a) Assuming the volume is 2 L, calculate the equilibrium constant 𝐾𝑐 for the reaction.

The following equilibria were attained at 823 K:

CoO(s) + H₂(g) → Co(s) + H₂O(g) K_c = 67

CoO(s) + CO(g) → Co(s) + CO₂(g) K_c = 490

Based on these equilibria, calculate the equilibrium constant for H₂(g) + CO₂(g) → CO(g) + H₂O(g) at 823 K.

Calculate the value of the equilibrium constant at 427 °C for the reaction

Na O1s2 + 1>2 O 1g2 ∆ Na O 1s2

given the following equilibrium constants at 427 °C.

Na2O1s2 ∆ 2 Na1l2 + 1>2 O21g2 Kc = 2 * 10-25 Na O 1s2 ∆ 2 Na1l2 + O 1g2 K = 5 * 10-29

Ethene (C₂H₄) can be halogenated by this reaction: C₂H₄(g) + X₂(g) ⇌ C₂H₄X₂(g) where X₂ can be Cl₂ (green), Br₂ (brown), or I₂ (purple). Examine the three figures representing equilibrium concentrations in this reaction at the same temperature for the three different hal- ogens. Rank the equilibrium constants for the three reactions from largest to smallest.