Decide which of the following statements are True and which are False about equi

ID: 915837 • Letter: D

Question

Decide which of the following statements are True and which are False about equilibrium systems:

A large value of K means the equilibrium position lies far to the right.

For the following reaction: H2(g) + F2(g) 2HF(g) the values of K and Kp are not the same.

The value of K at constant temperature does not depend on the amounts of reactants and products that are mixed together initially.

For the following reaction: CaCO3(s) CaO(s) + CO2(g) the [CaCO3] appears in the denominator of the equilibrium expression.

For a reaction with K >> 1, the rate of the forward reaction is less than the rate of the reverse reaction at equilibrium.

1) A large value of K means the equilibrium position lies far to the right: True

As K = [Product] / [Reactant]

So higher value of K, means higher concentration of product, means the equilibrium position lies far to the right

2) For the following reaction: H2(g) + F2(g) 2HF(g) the values of K and Kp are not the same False

Kp = Kc as delta n = 0

3) The value of K at constant temperature does not depend on the amounts of reactants and products that are mixed together initially : True

4) For the following reaction: CaCO3(s) CaO(s) + CO2(g) the [CaCO3] appears in the denominator of the equilibrium expression :False

K = [CO2]

The CaCO3 and CaO will not be in the rate law expression as both are solid

5) For a reaction with K >> 1, the rate of the forward reaction is less than the rate of the reverse reaction at equilibrium. False

Rate of forward reaction > rate of reverse reaction

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