$A$ substance $A$ decomposes by a first order reaction starting initially with $[A]_0 = 2.00 \, M$ and after $200 \, \min$,$[A]_t = 0.15 \, M$. For this reaction,what is the value of the rate constant $k$?
- A$1.29 \times 10^{-2} \, \min^{-1}$
- B$2.29 \times 10^{-2} \, \min^{-1}$
- C$3.29 \times 10^{-2} \, \min^{-1}$
- D$4.40 \times 10^{-2} \, \min^{-1}$
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View Solution$A$ first-order reaction decomposes such that the time taken for $1/8$ and $1/10$ of the initial concentration to decompose are $t_{1/8}$ and $t_{1/10}$ respectively. Find the value of $\frac{t_{1/8}}{t_{1/10}} \times 10$. (Given: $\log_{10} 2 = 0.3$)
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