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]
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-xaa−x
ForFor halfhalf lifelife
tt == t1/2;t1/2; x=a2x=a2
t1/2=2.303klogt1/2=2.303klog aa−a2aa−a2
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)
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