| Assertion: Half-life period of a reaction of first order is independent of initial concentration. |
| Reason: Half-life period for a first order reaction \[{{t}_{1/2}}=\frac{2.303}{K}\log 2.\] |
| Read the assertion and reason carefully to mark the correct option out of the options given below: |
A) If both assertion and reason are true and the reason is the correct explanation of the assertion.
B) If both assertion and reason are true but reason is not the correct explanation of the assertion.
C) If assertion is true but reason is false.
D) If the assertion and reason both are false.
E) If assertion is false but reason is true.
Correct Answer: A
Solution :
[a] For a first order reaction, \[K=\frac{2.303}{t}\log \frac{a}{a-x}\], where a is initial concentration, and x is the amount reacted in time t. For half-life \[x=a/2\], \[t={{t}_{1/2}}\] \[K=\frac{2.303}{K}\log \frac{a}{a-a/2}\] \[{{t}_{1/2}}=\frac{2.303}{K}\log \ 2=\frac{0.693}{K}\].
You need to login to perform this action.
You will be redirected in
3 sec
