Question

For nth order reaction,
$\left(\frac{dx}{dt}\right)=$ rate $=k[A{]}^n$
Graphs between log (rate) and log $\left[A_0\right]$ are of the type $(\left[A_0\right]$ is the initial concentration)

Lines $P,Q,R$ and $S$ are for the order

• A. P-0, Q-1, R-2, S-3
• B. P-0, Q-3, R-2, S-1
• C. P-1, Q-2, R-3, S-0
• D. P-3, Q-2, R-1, S-0

Answer 1

Answer: (D)

$\log \left(\frac{dx}{dt}\right)=\log k+n/y[A]$

$n=$ order of the reaction $=$ slope of the line

Larger the value of the slope of the line, larger the order.

Thus, $P=3,Q=2,R=1,S=0$