Question

Time required for a particular reaction to be half completed is 693 seconds. Calculate the time required for 90% completion of this reaction

Answer 1

Pls refer to the pic below.

Answer 2

The time required for 90% completion of this reaction is 2303 seconds

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) for completion of half life:  

Half life is the amount of time taken by a radioactive material to decay to half of its original value.

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

$k=\frac{0.693}{693}=0.001$

b) for completion of 90 % of reaction  

$t=\frac{2.303}{0.001}\log\frac{100}{100-90}$

$t=\frac{2.303}{0.001}\log\frac{100}{10}$

$t=2303sec$

The time required for 90% completion of this reaction is 2303 seconds

Learn more about first order kinetics

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