The reaction 2ClO₂(g)+ F₂(g)$\rightarrow$ 2FClO₂(g) Is first order in both ClO₂ and F₂.When the initial concentrations of ClO₂ and F₂ are equal,the rate after 25% of the F₂ has reacted is what percent of the initial rate?

Question

Quizplus · Accepted Answer

Since the reaction is first order in both ClO₂ and F₂, the rate law can be written as: Rate = k[ClO₂][F₂] When the initial concentrations of both reactants are equal, we can assume their concentration to be 'x', so the initial rate is: Rate(initial) = k(x)(x) = kx^2 Now, after 25% of F₂ has reacted, the concentration of F₂ remaining is 0.75x. We can plug this into the rate law and simplify as follows: Rate = k(x)(0.75x) = 0.75kx^2 The rate after 25% of F₂ has reacted is therefore 0.75 times the initial rate. This is equivalent to a percentage decrease of 25%, so the answer is (C) 37.5%.

The Reaction 2ClO2(g)+ F2(g) →\rightarrow→ 2FClO2(g) Is First Order in Both ClO2 and F2

The Reaction
2ClO₂(g)+ F₂(g) $\rightarrow$ 2FClO₂(g)
Is First Order in Both ClO₂ and F₂