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.

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?

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 ?

The rate constant for a first order reaction was found to be 0.082 min^(-1) . If initial concentration of reactant is 0.15M , how long would it take: (a) to reduce the concentration of A to 0.03 M ? (b) to reduce the concentration of A by 0.03 M ?

For a zero order reaction : A rarr 2B, initial rate of a reaction is 10^(-1)"M min"^(-1) . If concentration of 'A' is 0.1 after 120 sec then what would be concentration of B after 60 sec.

For any reaction A(g) rarr B(g) , rate constant k = 8.21 xx 10^(-2) atm/min at 300 K. If initial concentration of A is 2M then what is the half life (in hr.)?

Consider the reaction : {:(,P(g)+,2Q(g)overset(K_(C )=10^(12))hArr,R(g)+,S(g)),("Initial conc.",2M,4M,0,0):} then select correct statement(s)