The rate law expresses the relationship of the rate of a reaction to the rate constant and the concentration of the reactants raised to some powers for the general reaction.
`aA+bBtocC+dD`
Rate law takes the form
`r=k[A]^(x)[B]^(y)`
where x and y are number that must be determined experimentely k is the rate constant and [A] and [B] are concentration of A & B respectively.
The initial rate of zero order reaction of the gaseous equation `A(g)to2B (g)` is `10^(-2) M min^(-1)` If the initial concentration of A is 0.1 M what would be concentration of B after 60 seconds ?

Options

A. 0.09 M
B. 0.01 M
C. 0.02 M
D. 0.03 M

Answer

C

Explanation

`r=k_1 " " [C]_t=C_0-kt`
`=0.1-10^(-1)xx1=0.09` M
`[B]_t=0.01xx2=0.02 M`