The given plots represent the variation of the concentration of a reactant R with time for two different reaction (i) and (ii) The respective orders of the reactions are

Step-by-step solution

Integrated rate law for first order reaction is k = 1 t 1 n C o C t [Where C t → concentration of reactant at time t , C o → initial concentration of reactant] 1 n C o C t = 1 n C o - 1 n C t = k t 1n ( C t ) = - k t + 1 n ( C o ) If ( C t ) = [ R ] = concentration of reactant 1 n [ R ] = - k t + 1 n ( C o ) On comparing with y = mx + C ⇒ Slope m = - k for graph between 1n (R) and t with intercept 1n ( C o ) ⇒ First graph is of first order Integrated rate law for zero order reactions is C t = C o - k t