Rate law for the reaction can be
Rate = [A]α [B]β
From first and second observations
0.004 mol L−1 min−1 = k[6 × 10−2 molL−1 ]α [1 × 10−2 molL−1 ]β ...(a)
0.008 molL−1 min−1 = k[6 × 10−2 molL−1 ]α [2 × 10−2 molL−1 ]β ...(b)
Dividing eqn (b) by (a)
Similarly from observations (i) and (iii)
Order of reaction n = a + b = 2
∴ Rate law for reaction is
Rate = k [A] [B]
From observation (i)
0.004mol L−1 min−1 = k[6 × 10−2 mol L−1 ] [1 × 10−2 mol L−1 ]