Question
In: Chemistry
Decide which of the following statements are True and which are False about equilibrium systems: The...
Decide which of the following statements are True and which
are False about equilibrium systems:
The value of K at constant temperature depends on the amounts
of reactants and products that are mixed together initially.
For a reaction with K >> 1, the rate of the forward
reaction is less than the rate of the reverse reaction at
equilibrium.
A large value of K means the equilibrium position lies far to
the left.
For the following reaction: CaCO3(s) ⇌ CaO(s) + CO2(g) the
[CaCO3] should not appear in the equilibrium expression.
For the following reaction: H2(g) + F2(g) ⇌ 2HF(g) the values
of K and Kp are the same.
Solutions
Expert Solution
=> The value of K at constant temperature depends on the amounts of reactants and products that are mixed together initially is False. Because K depends upon the equilibrium concentrations, not initial concentration.
=> For a reaction with K >> 1, the rate of the forward reaction is less than the rate of the reverse reaction at equilibrium is False. Because, at equilibrium, both rates are the same; that's the definition of equilibrium.
=> A large value of K means the equilibrium position lies far to the left is False. Because K is products over reactants, so high K means more products, therefore more to the right.
=> For the following reaction: CaCO3(s) ⇌ CaO(s) + CO2(g) the [CaCO3] should not appear in the equilibrium expression is False. Because the expression for K is products over reactants, K=[CaO][CO2]/[CaCO3].
=> For the following reaction: H2(g) + F2(g) ⇌ 2HF(g) the values of K and Kp are the same is true. The relation bvetween K and Kp is K=Kp/1bar.
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