Question

The half - life period of a first order chemical reaction is 6.93 minutes. The time required for the completion of 99% of the chemical reaction will be (log2=0.301); (A)230.3minutes(B)23.03minutes(C)46.06minutes(D)460.6minutes

Answer 1

Hence the answer is © 46.06 minutes.
Hope I helped you.

Answer 2

The time required for the completion of 99% of the chemical reaction will be 46.06 minutes

Explanation:

Expression for rate law for first order kinetics is given by:

$t=\frac{2.303}{k}\log\frac{a}{a-x}$

where,

k = rate constant  

t = age of sample

a = let initial amount of the reactant  

a - x = amount left after decay process  

a) to calculate rate constant from half life:

$t_{\frac{1}{2}}=\frac{0.693}{k}$

$k=\frac{0.693}{6.93}=0.1min^{-1}$

b) for completion of 99 % of reaction  

$t=\frac{2.303}{k}\log\frac{100}{100-99}$

$t=\frac{2.303}{k}\log\frac{100}{100-99}$

$t=\frac{2.303}{0.1}\times 2$

$t_{99}=46.06min$

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