Compounds A and B react according to the equation 2 A(g)+B(g) 2 C(g)+D(g) . The initial rate of formation was determined at different initial concentrations of A and B . The following results were obtained. The rate law for this reaction may be [All concentrations are in mol / L ]

Step-by-step solution

2 A+B 2 C+D Let order with respect to A and B are x and y respectively. Rate =k[A]^x[B]^y7.2 10⁻²=k(0.3)^x(0.2)^y ...(i) 2.88 10⁻¹=k(0.3)^x(0.4)^y ...(ii) 6 10⁻³=k(0.1)^x(0.1)^y ...(iii) 2.4 10⁻²=k(0.4)^x(0.1)^y ...(iv) Dividing Eq. (i) by Eq. (ii), we get 7.2 10⁻² 2.88 10⁻¹ = (0.2)^y (0.4)^y 1 4 = ( 1 2 )^y ( 1 2 )^2= ( 1 2 )^y y=2 Dividing Eq. (iii) by Eq. (iv), we get 6 10⁻³ 2.4 10⁻² = (0.1)^x (0.4)^x ( 1 4 )^1= ( 1 4 )^x ( 1 4 )^1= ( 1 4 )^x x=1 aligned & Rate =k[A]^x[B]^y & Rate =k[A][B]^2 aligned