Coal, which is primarily carbon, can be converted to natural gas, primarily CH₄, by the exothermic reaction: C(s) + 2 H₂(g) ⇌ CH₄(g) Which disturbance will favor CH₄ at equilibrium?

a. adding more C to the reaction mixture b. adding more H₂ to the reaction mixture d. lowering the volume of the reaction mixture f. adding neon gas to the reaction mixture

Coal, which is primarily carbon, can be converted to natural gas, primarily CH₄, by the exothermic reaction: C(s) + 2 H₂(g) ⇌ CH₄(g) Which disturbance will favor CH₄ at equilibrium? c. raising the temperature of the reaction mixture

Coal, which is primarily carbon, can be converted to natural gas, primarily CH₄, by the exothermic reaction: C(s) + 2 H₂(g) ⇌ CH₄(g) Which disturbance will favor CH₄ at equilibrium? e. adding a catalyst to the reaction mixture

Coal can be used to generate hydrogen gas (a potential fuel) by the endothermic reaction: C(s) + H₂O(g) ⇌ CO(g) + H₂(g) If this reaction mixture is at equilibrium, predict whether each disturbance will result in the formation of additional hydrogen gas, the formation of less hydrogen gas, or have no effect on the quantity of hydrogen gas. e. adding a catalyst to the reaction mixture

Carbon monoxide replaces oxygen in oxygenated hemoglobin according to the reaction: HbO₂(aq) + CO(aq) ⇌ HbCO(aq) + O₂(aq) a. Use the reactions and associated equilibrium constants at body temperature given here to find the equilibrium constant for the reaction just shown. Hb(aq) + O₂(aq) ⇌ HbO₂(aq) K_c = 1.8 Hb(aq) + CO(aq) ⇌ HbCO(aq) K_c = 306

At 650 K, the reaction MgCO₃(s) ⇌ MgO(s) + CO₂(g) has K_p = 0.026. A 10.0-L container at 650 K has 1.0 g of MgO(s) and CO₂ at P = 0.0260 atm. The container is then compressed to a volume of 0.100 L. Find the mass of MgCO₃ that is formed.

Consider the exothermic reaction: C₂H₄(g) + Cl₂(g) ⇌ C₂H₄Cl₂(g) If you were trying to maximize the amount of C₂H₄Cl₂ produced, which tactic might you try? Assume that the reaction mixture reaches equilibrium. a. increasing the reaction volume b. removing C₂H₄Cl₂ from the reaction mixture as it forms c. lowering the reaction temperature d. adding Cl₂

Consider the endothermic reaction: C₂H₄(g) + I₂(g) ⇌ C₂H₄I₂(g) If you were trying to maximize the amount of C₂H₄I₂ produced, which tactic might you try? Assume that the reaction mixture reaches equilibrium. a. decreasing the reaction volume b. removing I₂ from the reaction mixture c. raising the reaction temperature d. adding C₂H₄ to the reaction mixture

Consider the reaction: H₂(g) + I₂(g) ⇌ 2 HI(g) A reaction mixture at equilibrium at 175 K contains P_H2 = 0.958 atm, P_I2 = 0.877 atm, and P_HI = 0.020 atm. A second reaction mixture, also at 175 K, contains P_H2 = P_I2 = 0.621 atm and P_HI = 0.101 atm. Is the second reaction at equilibrium? If not, what will be the partial pressure of HI when the reaction reaches equilibrium at 175 K?

A reaction vessel at 27 °C contains a mixture of SO₂ (P = 3.00 atm) and O₂ (P = 1.00 atm). When a catalyst is added, this reaction takes place: 2 SO₂( g) + O₂( g) ⇌ 2 SO₃( g). At equilibrium, the total pressure is 3.75 atm. Find the value of K_c.

At 70 K, CCl4 decomposes to carbon and chlorine. The Kp for the decomposition is 0.76. Find the starting pressure of CCl4 at this temperature that will produce a total pressure of 1.0 atm at equilibrium.

The equilibrium constant for the reaction SO₂(g) + NO₂(g) ⇌ SO₃(g) + NO(g) is K_c = 3.0. Find the amount of NO₂ that must be added to 2.4 mol of SO₂ in order to form 1.2 mol of SO₃ at equilibrium.

Carbon monoxide and chlorine gas react to form phosgene: CO(g) + Cl₂(g) ⇌ COCl₂(g) K_p = 3.10 at 700 K If a reaction mixture initially contains 215 torr of CO and 245 torr of Cl₂, what is the mole fraction of COCl₂ when equilibrium is reached?