Final answer:
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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