The correct graphical representation of first-order reaction is:

(a)  (b)
(c) (d)

   

1. (a) and (b) 2. (b) and (c)
3. (c) and (d) 4. (a) and (d)

HINT: k=2.303tlog[Ro][R]k=2.303tlog[Ro][R]

Explanation:

Step 1:

For the first-order reaction

k=2.303tlog[Ro][R]k=2.303tlog[Ro][R]
log[Ro][R]=k2.303tlog[Ro][R]=k2.303t            ......(1)......(1)

The first equation is the same as y=mx+c. Thus, straight-line graph is obtained. The slope is k2.303k2.303

The correct plot between log [R]0[R}[R]0[R} vs t can be represented by (d)

Step 2:

The time taken for any fraction of the reaction to complete is independent of the initial concentration Let, us consider it for half of the reaction to complete.

tt == 2.303klog2.303klog aa-xaax
ForFor halfhalf lifelife    
tt == t1/2;t1/2; x=a2x=a2
t1/2=2.303klogt1/2=2.303klog aaa2aaa2
t1/2=2.303klogt1/2=2.303klog 22
 t1/2=0.693kt1/2=0.693k

t1/2 is independent of initial concentration. Hence, the correct plot of t1/2, and [Ro] can be represented by (a)