Consider a first order reaction at "450K
`X(g)rarr Y(g)+Z(g)`
What is the rate constant of the reaction using given data? [Assume initially only X is present ]
`[[Time(s),0, 5 ],[(" Total Pressure "),15,20]]`

The given data are for the reaction, 2NO(g)+Cl(g)rarr2NOCl(g)" at "298K The rate law of the reactions is

In a first-order reaction A rarr B , if K is the rate constant and initial concentration of the reactant is 0.5 M , then half-life is

A first order reaction has specific rate of 10^(-2)s^(-1) . How much time will it take for 20 g of the reactant to reduce to 5 g?

For a first order reaction A(g)rarr2B(g)+C(g) at constant volume and 300 K, the total pressure at the beginning (t=0) and at time t ae P_(0) and P_(t) respectively. Initially, only A is present with concentration [A]_(0) and t_(1//3) is the time required for the partial pressure of A to reach 1/3rd of its initial value. The correct options (s) is (are) : (Assume that all these behave as ideal gases)

Consider the reaction 2A(g) rarr 3B(g) + C(g) . Starting with pure A initially, the total pressure doubled in 3 hrs. The order of the reaction might possibly be :