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Hello! I'm confused about the answer to problem 5G.1 of the 7th edition of the textbook. In the solutions manual, the answer for part b states the "equilibrium reactions are affected by the presence of both products and reactants" and then for part c states that "the value of the equilibrium constant is not affected by the amounts of reactants or products added as long as the temperature is constant". Could someone explain the difference between these two answers? Thank you!
The first statement is true because equilibrium reactions take account for both the reactants and products. If there is more products or reactants, the reaction will adjust accordingly according to the Le Chatelier's Principle. The second statement refers to its equilibrium CONSTANT, not reaction. For the equilibrium constant, it is Products/Reactants. As long as the ratios (co-efficients) and temperature are the same, then the equilibrium constant will not change just because it is a ratio and adding more products/reactants won't change the ratio.
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