A sample of nitrosyl bromide (NOBr) decomposes according to the equation 2 NOBr(𝑔) ⇌ 2 NO(𝑔) + Br₂(𝑔) An equilibrium mixture in a 5.00-L vessel at 100°C contains 3.22 g of NOBr, 2.46 g of NO, and 6.55 g of Br₂. (b) What is the total pressure exerted by the mixture of gases?

When 2.00 mol of SO₂Cl₂ is placed in a 2.00-L flask at 303 K, 56% of the SO₂Cl₂ decomposes to SO₂ and Cl₂: SO₂Cl₂(g) ⇌ SO₂(g) + Cl₂(g) (c) According to Le Châtelier's principle, would the percent of SO₂Cl₂ that decomposes increase, decrease or stay the same if the mixture were transferred to a 15.00-L vessel?

Consider the hypothetical reaction A(𝑔) ⇌ 2 B(𝑔). A flask is charged with 0.75 atm of pure A, after which it is allowed to reach equilibrium at 0°C. At equilibrium, the partial pressure of A is 0.36 atm. (c) To maximize the yield of product B, would you make the reaction flask larger or smaller?

When 2.00 mol of SO₂Cl₂ is placed in a 2.00-L flask at 303 K, 56% of the SO₂Cl₂ decomposes to SO₂ and Cl₂: SO₂Cl₂(g) ⇌ SO₂(g) + Cl₂(g) (a) Calculate K_c for this reaction at this temperature.

As shown in Table 15.2, the equilibrium constant for the reaction N₂(g) + 3 H₂(g) ⇌ 2 NH₃(g) is K_p = 4.34 × 10^-3 at 300°C. Pure NH₃ is placed in a 1.00-L flask and allowed to reach equilibrium at this temperature. There are 1.05 g NH₃ in the equilibrium mixture. (b) What was the initial mass of ammonia placed in the vessel?