1. | Write balanced chemical equations for each of the following. Pay close attention to the physical states! Also - you must include the charge when writing ions, otherwise your answer is incorrect. Do not balance these equations using fractions for coefficients.
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2. | For each of the above reactions, write the equilibrium expression, Keq, for the reaction. Remember not to include solids or liquids in the equilibrium constant expression. | ||||||||||||||||||
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3. | The equilibrium equation for the formation of ammonia is N2 (g) + 3 H2 (g) ↔ 2 NH3 (g) At 200°C the concentrations of nitrogen, hydrogen, and ammonia at equilibrium are measured and found to be [N2] = 2.12; [H2] = 1.75, and [NH3] = 84.3. Calculate Keq at this temperature. |
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4. | For each of the following equilibrium systems, identify whether the reactants or products are favored at equilibrium, or whether they are equally favored.
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5. | For the reaction: carbon monoxide burns in oxygen to produce carbon dioxide
Calculate [CO] |
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Check your answers | |||||||||||||||||||
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