Which of the following graphs are correct for first order reaction?

Choose the correct answer from the options given below:

A and C only

Integrated rate equation for first order reaction is given by

k = \(\frac{2.303}{t}\)log\(\frac{[R_o]}{[R]}\) .... (i)

\(\frac{kt}{2.303}\) = log\(\frac{[R_o]}{[R]}\) 

mx + c = y

on comparing, y = log\(\frac{[R_o]}{[R]}\), Slope, m = \(\frac{k}{2.303}\)

Plot will be 

On rearranging the equation (i), we get

t = \(\frac{2.303}{k}\)log[R_o] - \(\frac{2.303}{k}\)log[R]

logR = -\(\frac{k}{2.303}\)t + log[R_o]

lnR = -kt + ln[R_o]

y = mx + c

On comparing, we get y = lnR, slope m = -k, intercept c = ln[R_o]

Plot will be