1. | Write reversible reactions for each of the following situations (be sure to balance your equations):
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Solution:
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2. | Describe two different mixtures of starting materials that can be used to produce the equilibrium A + B ↔ C + D |
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Solution: You could start with either a mixture of A and B or with a mixture of C and D. Both starting materials will produce the same equilibrium. |
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3. | If the system represented by the following equation is found to be at equilibrium at a specific temperature, which of the following statements is true? Explain your answers.
H2O(g) + CO(g) ↔ H2 (g) + CO2 (g) |
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Solution:
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4. | Would you expect the combustion of methane, CH4 with oxygen to form carbon dioxide and water, to be a reversible reaction? Hint: Methane, or natural gas, is an important energy source. Considering this, what did you learn in the last unit that will help you predict whether or not the reverse reaction is likely to be spontaneous? |
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Solution: No - this is a very exothermic reaction, releasing a lot of heat (methane, natural gas, is used as a heating fuel). The reverse reaction would be therefore be highly endothermic, requiring a lot of energy to make it go. Thus it is not likely to be reversible. |
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