Browse by Stream
QnA
Home
QnA
Go To Your Study Dashboard

Get Answers to all your Questions

header-bg qa
  • Home
  • Engineering
  • Consider the following first-order reactions <img alt="X\overset{k_{1}}{\rightarrow}A+B\: \: and\: \: Y\overset{k_{2}}{\rightarrow}C+D" src="http://entrancecorner.oncodecogs.com/gif.latex

Consider the following first-order reactions

X\overset{k_{1}}{\rightarrow}A+B\: \: and\: \: Y\overset{k_{2}}{\rightarrow}C+D

If 50% of the reaction of X was completed when 96% of the reaction of Y was completed, the ratio of their rate constants \left ( k_{2}/k_{1} \right ) is

Option: 1

4.65


Option: 2

0.215


Option: 3

1.1


Option: 4

4.06


Answers (1)

best_answer

If 50% of the reaction of X was completed when 96% of the reaction of Y was completed

1. \mathrm{t_{1/2}=\frac{ln2}{k_1}}

2. \mathrm{t_{96%}=\frac{1}{k_2}ln\frac{100}{100-96}= \frac{1}{k_2}ln\frac{100}{4}}

Both completion time is same so, 

\mathrm{\frac{ln2}{k_1}= \frac{1}{k_2}ln\frac{100}{4}}

\mathrm{\frac{k_2}{k_1}= \frac{log5^2 }{log2}}

\mathrm{\frac{k_2}{k_1}= 2\times\frac{log5 }{log2}}

\mathrm{\frac{k_2}{k_1}= 2\times\frac{0.6989 }{0.3010}}

\mathrm{\frac{k_2}{k_1}= 2\times 2.32= 4.64}

Ans  approx 4.65

 

Posted by

Devendra Khairwa

View full answer

Similar Questions

Latest Question