- For the reaction: H2 + Cl2 → 2 HCl carried out in 1.0 liter of solution:
- When the reaction is started with 0.10 mole of H2 and 0.20 mole of Cl2, 0.10 mole of HCl is obtained when equilibrium has been established. Calculate the equilibrium constant for the reaction.
- How much H2 would have to be added to this equilibrium mixture in order to obtain a total of 0.20 mole of HCl at equilibrium?
- When the equilibrium mixture of part a is heated to a new temperature the amount of HCl present decreases by 0.05 mole. Calculate the equilibrium constant at this new temperature.
- Consider the reaction:
CO(g) + 2 H2(g) → CH3OH(g)
- When 0.20 mole CO are mixed with 0.40 mole H2 in an empty 1.0 L flask, 0.10 mole of CH3OH are obtained when equilibrium is established. Calculate the equilibrium constant.
- If 0.10 mole of CH3OH are added to the equilibrium mixture of part a, how much CH3OH would be present when the equilibrium is reestablished?
- How much CH3OH would be obtained at equilibrium if the reaction were started with 0.40 mole CO and 0.40 H2?
- How much H2 must be mixed with 0.20 mole of CO in an empty 1.0 L flask in order to obtain 0.20 mole of CH3OH at equilibrium?
- At a higher temperature, 0.05 mole of CH3OH is obtained when the reaction is started with 0.20 mole CO and 0.40 mole of H2 in a 1.0 L flask. Is the reaction exothermic or endothermic? Explain.
- If the pressure is reduced by increasing the volume of the flask to 2.0 L, what will happen to the amount of CH3OH present at equilibrium?