The reaction `3A to 2B+C` is carried in a closed vessel. The rate of disappearance of `A[(-d[A])/(dt)]` is 0.01 `molL^(-1)s^(-1)`. Calculate `(d[B])/(dt)` and `(d[C])/(dt)`.

Explanation

To solve the problem, we need to use the stoichiometry of the reaction and the given rate of disappearance of reactant A. The reaction is:

\[ 3A \rightarrow 2B + C \]

### Step-by-Step Solution:

1. **Identify the Rate of Reaction**:
The rate of disappearance of A is given as:
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