Question

In the nuclear industry, chlorine trifluoride is used to prepare uranium hexafluoride, a volatile compound of uranium used in the separation of uranium isotopes. Chlorine trifluoride is prepared by the reaction Cl₂(g) + 3F₂(g) ⟶ 2ClF₃(g). Write the equation that relates the rate expressions for this reaction in terms of the disappearance of Cl₂ and F₂ and the formation of ClF₃.

a) rate = -1/2d[Cl₂]/dt = -3/2d[F₂]/dt = d[ClF₃]/dt
b) rate = -d[Cl₂]/dt = -3d[F₂]/dt = 2d[ClF₃]/dt
c) rate = -1/2d[Cl₂]/dt = -1/2d[F₂]/dt = d[ClF₃]/dt
d) rate = -d[Cl₂]/dt = -1/3d[F₂]/dt = 2/3d[ClF₃]/dt

Answer 1

The rate of the reaction Cl₂ + 3F₂ → 2ClF₃ is expressed as rate = -½ d[Cl₂]/dt = -³2 d[F₂]/dt = d[ClF₃]/dt, which relates the stoichiometric coefficients from the balanced equation to the rates of disappearance of the reactants and the formation of the product. Option a

Step-by-step explanation:

In the reaction Cl₂(g) + 3F₂(g) → 2ClF₃(g), the rate of reaction can be expressed in terms of the disappearance of chlorine (Cl₂) and fluorine (F₂) gases, and the formation of chlorine trifluoride (ClF₃). The stoichiometry of the reactants and products can be used to relate the rates at which they are consumed or produced.

When defining the rate of reaction, the change in concentration of reactants is taken as negative (since they are being consumed) and the change in concentration of products is positive (as they are being formed).

Given the balanced chemical equation, we can write a rate expression that is based on the stoichiometry of the reaction:

rate = -½ d[Cl₂]/dt = -³2 d[F₂]/dt = d[ClF₃]/dt

This relates the rate of disappearance of Cl₂ and F₂ to the rate of appearance of ClF₃, taking into account their stoichiometric coefficients. Thus, the correct answer is:

a) rate = -½ d[Cl₂]/dt = -³2 d[F₂]/dt = d[ClF₃]/dt. Option a