Q.A first-order reaction has a rate constant $k = 4.606 \times 10^{-3} \text{ s}^{-1}$ . The time required to reduce $2.0 \text{ g}$ of the reactant to $0.2 \text{ g}$ is:

200 \text{ s}

500 \text{ s}

1000 \text{ s}

100 \text{ s}

The correct solution involves applying the fundamental concept to derive the final value step by step...

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Q.A first-order reaction has a rate constant k=4.606×10−3 s−1k = 4.606 \times 10^{-3} \text{ s}^{-1}k=4.606×10−3 s−1. The time required to reduce 2.0 g2.0 \text{ g}2.0 g of the reactant to 0.2 g0.2 \text{ g}0.2 g is: