Question

Consider the reaction:

Cl2(g)+3F2(g)→2ClF3(g)
Δ[Cl2]/Δt = -0.012 M/s .
1)Find Δ[F2]/Δt
2)Find Δ[ClF3]/Δt
3)Find the rate of the reaction.

Answer 1

1) Δ[F2]/Δt = -0.036 M/s. 2) Δ[ClF3]/Δt = -0.024 M/s. 3) The rate of the reaction is -0.012 M/s.

Step-by-step explanation:

1) To find Δ[F2]/Δt, we can use the stoichiometry of the reaction. From the balanced equation, we can see that the coefficient of F2 is 3. So, the rate of change of F2 concentration is three times the rate of change of Cl2 concentration, which is -0.012 M/s. Therefore, Δ[F2]/Δt = (3)(-0.012 M/s) = -0.036 M/s.

2) Similarly, to find Δ[ClF3]/Δt, we can use the stoichiometry of the reaction. From the balanced equation, we can see that the coefficient of ClF3 is 2. So, the rate of change of ClF3 concentration is two times the rate of change of Cl2 concentration, which is -0.012 M/s. Therefore, Δ[ClF3]/Δt = (2)(-0.012 M/s) = -0.024 M/s.

3) The rate of the reaction is determined by the coefficient of one of the reactants. In this case, since the coefficient of Cl2 is 1, the rate of the reaction is equal to the rate of change of Cl2 concentration. Therefore, the rate of the reaction is -0.012 M/s.