Which of the following graphs are correct for first order reaction? Choose the correct answer from the options given below: |
B and C only A and B only A and C only C and D only |
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[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 |