For a reversible first order reaction,

`K_(f) =10^(-2) sec^(-1) and (B_(eq))/(A_(eq))=4," If "A_(0) =0.01 ML^(-1) and B_(0) =0`, what will be concentration of B after 30 sec ?

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.

The reaction A(g) to B(g) + 2C(g) is a first-order reaction with a rate constant of 2.303 xx 10^(-3)s^(-1) . Strating with 0.1 moles of 'A' in a 2 litre vessel, find the concentration of A after 301 sec when the reaction is allowed to take place at constant pressure at 300 K.

The reaction A(g) to B(g) + 2C(g) is a first-order reaction with a rate constant of 2.303 xx 10^(-3)s^(-1) . Strating with 0.1 moles of 'A' in a 2 litre vessel, find the concentration of A after 301 sec when the reaction is allowed to take place at constant pressure at 300 K.

The specific rate constant for a first order reaction is 1 times 10^–3 sec^–1 . If the initial concentration of the reactant is 0.1 mole/lt, the rate of reaction mol l^–1 sec^–1 is:

An observed event B can occur after one of the three events A_(1), A_(2), A_(3) . If P(A_(1)) = P(A_(2)) = 0.4, P(A_(3)) = 0.2 and P(B//A_(1)) = 0.25, P(B//A_(2)) = 0.4, P(B//A_(3)) = 0.125 , what is the probability of A_(1) after observing B ?