The half-life of a first-order reaction is $900 \text{ s}$. If the initial concentration of the reactant is $0.08 \text{ mol dm}^{-3}$, find the concentration that remains after $35 \text{ minutes}$?
- A$0.159 \text{ mol dm}^{-3}$
- B$0.0159 \text{ mol dm}^{-3}$
- C$0.05 \text{ mol dm}^{-3}$
- D$0.759 \text{ mol dm}^{-3}$
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For a first-order reaction,the concentration decreases from $800 \ mol/dm^3$ to $50 \ mol/dm^3$ in $2 \times 10^4 \ s$. What is the rate constant of the reaction?
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View Solution$A$ first order reaction takes $40 \ min$ for $20 \%$ decomposition. Calculate its rate constant.
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