Which of the following graphs are correct for first order reaction?
Choose the correct answer from the options given below:
Answer & explanation
Correct answer: option 3
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[Ro] - \(\frac{2.303}{k}\)log[R]
logR = -\(\frac{k}{2.303}\)t + log[Ro]
lnR = -kt + ln[Ro]
y = mx + c
On comparing, we get y = lnR, slope m = -k, intercept c = ln[Ro]
Plot will be 