Question

For zero order reactions, the linear plot was obtained for $\left[A\right]$ vs t. The slope of the line is equal to:

• A. $k_0$
• B. $-k_0$
• C. $\frac{0.693}{K_o}$
• D. $-\frac{K_o}{2.303}$

Answer 1

Answer: (B)

$-k_0$

For a Zero Order Reaction,

$-\frac{d\left[A\right]}{dt}=k$

Integrating on both sides and finding the value of 'c'(Constant of proportionality), we get

('c' can be found out by substituting [A] = $\left[A_0\right]$ at t = 0)

$\left[A\right]=-k_{0}t+\left[A_0\right]$

Where, $-k_0$ is rate constant, $\left[A_0\right]$ is Initial Concentration.

So, the Slope of the line is $-k_0$