For the reaction,`A rarr B+C+D` starting with initial pressure 400 atm.If the total pressure after 2 hours is 800 atm,the value of rate constant is: (consider the reaction to be of `1^( st )` order )

For the first order reaction A(g) rarr 2B(g) + C(g) , the initial presuure is P_(A) = 90 m Hg , the pressure after 10 minutes is found to be 180 mm Hg . The rate constant of the reaction is

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 :

For a homogeneous gaseous reaction A rarr B + C + D , the initial pressure was P_0 white pressure after time 't' was P. if (P gt P_0) The expression for the constant K is

Consider a reaction 3A(g)rarr4B(g)+C(g) , starting with pure A having pressure (3)/(5) atm, the pressure after 10 min. reaches to 1 atm. Calculate the value of rate of disappearance of A at initial instant.

The order of the gaseous reaction A(g)rarr2B(g)+C(g) is found to be one at the intial pressure P_(0)=90 torr. The total pressure after ten minutes is found to be 180 torr. Find the value of the rate constant?