Multiple Choice
For the reaction 2HF(g) ⇌ H2(g) + F2(g) with an equilibrium constant K = 1.00x10^-2, if 1.00 mol of HF(g), 0.291 mol of H2(g), and 0.750 mol of F2(g) are mixed in a 5.00 L flask, what is the reaction quotient, Q?
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16. Chemical Equilibrium
Reaction Quotient
Multiple Choice
Which of the following is a false statement about the relationship between Q and K?
A
When Q > K, the reaction will shift toward the reactant side.
B
When Q = K, the reaction has stopped.
C
When Q < K, the reaction will shift toward the product side.
D
When Q = K, the forward reaction rate equals the reverse reaction rate.
E
All of the above are true statements.
Verified step by step guidance1
Understand the concept of the reaction quotient (Q) and the equilibrium constant (K). Q is calculated using the same expression as K, but with the current concentrations of the reactants and products. K is calculated using concentrations at equilibrium.
Recall the relationship between Q and K: If Q < K, the reaction will proceed in the forward direction to reach equilibrium. If Q > K, the reaction will proceed in the reverse direction to reach equilibrium. If Q = K, the system is at equilibrium.
Analyze the statement 'When Q > K, the reaction will shift toward the reactant side.' This is true because the reaction needs to shift in the reverse direction to reach equilibrium.
Evaluate the statement 'When Q = K, the reaction has stopped.' This is false because when Q = K, the reaction is at equilibrium, meaning the rates of the forward and reverse reactions are equal, but the reactions continue to occur.
Consider the statement 'When Q = K, the forward reaction rate equals the reverse reaction rate.' This is true because at equilibrium, the rates of the forward and reverse reactions are equal, maintaining constant concentrations of reactants and products.
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