Question

If $50\%$ of a reaction occurs in $100$ second and $75\%$ of the reaction occurs in $200$ second, the order of this reaction is :

• A. 0
• B. 1
• C. 2
• D. 3

Answer 1

Answer: (B)

1

Answer 2

For a first order reaction $k=\frac{2.303}{t} \log \frac{a}{a-x}$ At $100\, s :k=\frac{2.303}{100} \log \frac{100}{100-50}$ $k=\frac{2.303}{100} \log 2=\frac{2.303 \times 0.3010}{100}=0.00693\, min ^{-1}$ At $200\, s :k=\frac{2.303}{200} \log \frac{100}{100-75}$ $k=\frac{2.303}{200} \log 4=\frac{2.303 \times 0.6020}{200}=0.00693\, min ^{-1}$ As rate constant is same at $100\, s$ and $200\, s$, therefore, order of reaction is 1 .