For a reaction `Aoverset(k_(r)=0.6M min^(-1))to2B`
starting with 1 M of 'A' only, concentration of B (in M) after 100 sec. and 200 sec. is respectively?

Consider a reaction A(g)overset(k=0.1 M min^(-1))to2B(g) . If initial concentration of A is 0.5 M then select correct graph.

Consider a reaction A(g)overset(k=0.1 M min^(-1))to2B(g) . If initial concentration of A is 0.5 M then select correct graph.

Consider a reaction A(g)overset(k=0.1 M min^(-1))to2B(g) . If initial concentration of A is 0.5 M then select correct graph. a) b) c) d)

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 ?

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 ?