Answer:
A) Forward rate = 1.1934 × 10^(-4) M/min
B) I disagree with the claim
Explanation:
A) We are told that [HF] reaches a constant value of 0.0174 M at equilibrium.
The reversible reaction given to us is;
BF4-(aq) +H20(l) → BF3OH-(aq) + HF(aq)
From this, we can see that the stoichiometric ratio is 1:1:1:1
Thus, concentration of [BF4-] is now;
[BF4-] = 0.150 - 0.0174
[BF4-] = 0.1326 M
From the rate law, we are told the forward rate is kf [BF4-].
We are given Kf = 9.00 × 10^(-4) /min
Thus;
Forward rate = 9.00 × 10^(-4) /min × (0.1326M)
Forward rate = 1.1934 × 10^(-4) M/min
(B) The student claims that the initial rate of the reverse reaction is equal to zero can't be true because at equilibrium, rates for the forward and reverse reactions are usually equal.
Thus, I disagree with the claim.
