Question

In the reaction (given below) reactant A is found to disappear at the rate of 6.2×10^−4 N⋅s^−1 2A+B⟶C+3D a) Determine the individual rate of disappearance or individual rate of formation for each of the reactants and products. b) Determine the General Rate of the Reaction based on each of the reactants and products.

Answer 1

The rate of disappearance of each molecule of A and B is 3.1×10^−4 N⋅s^−1, while the formation rate of C is the same. However, 3 moles of D is formed for every mole of A, so its formation rate is 9.3×10^−4 N⋅s^−1. The general rate of reaction is 3.1×10^−4 N⋅s^−1.

Step-by-step explanation:

In this chemical reaction, the rate of disappearance of A, which is 6.2×10−4 N⋅s−1, is for 2 moles of A. Thus the rate of disappearances for each mole of A would be half of this, i.e., 3.1×10−4 N⋅s−1. Since the stoichiometric coefficient of B in the reaction is 1, the rate of disappearance of B would also be 3.1×10−4 N⋅s−1.

On the product side, the rate of formation of C would also be 3.1×10−4 N⋅s−1 since its stoichiometric coefficient is 1, but the rate of formation of D is three times the rate of disappearance of A, which equates to 9.3×10−4 N⋅s−1.

The General Rate of Reaction would be -1/2 d[A]/dt = -d[B]/dt = d[C]/dt = 1/3d[D]/dt = 3.1×10−4 N⋅s−1.

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