When a reversible reaction reaches equilibrium, which of the following statements is not true?The forwards and backwards reactions have the same rate of reactionThe concentrations of all reactants and products remain constantThe forwards and backwards reactions are still happeningThe concentrations of all reactants and products are equal
Question
When a reversible reaction reaches equilibrium, which of the following statements is not true?The forwards and backwards reactions have the same rate of reactionThe concentrations of all reactants and products remain constantThe forwards and backwards reactions are still happeningThe concentrations of all reactants and products are equal
Solution
The statement that is not true when a reversible reaction reaches equilibrium is: "The concentrations of all reactants and products are equal."
Here's why:
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"The forwards and backwards reactions have the same rate of reaction" - This is true. At equilibrium, the rate of the forward reaction equals the rate of the reverse reaction.
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"The concentrations of all reactants and products remain constant" - This is also true. At equilibrium, the concentrations of reactants and products do not change over time, although the reactions are still occurring.
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"The forwards and backwards reactions are still happening" - This is true as well. Even at equilibrium, the forward and reverse reactions continue to occur. However, because they occur at the same rate, there is no net change in the concentrations of the reactants and products.
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"The concentrations of all reactants and products are equal" - This is not necessarily true. At equilibrium, the concentrations of the reactants and products are constant, but they are not necessarily equal. The equilibrium constant, K, which is the ratio of the concentrations of the products to the reactants, determines the concentrations at equilibrium. If K > 1, the products are favored and their concentration is greater than that
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