A zero order reaction A `rarr` product , has rate constant `10^(-2)` mol `L^(-1) s ^(-1)` ,If a process is started with "10" moles of "A" in a ONE litre vessel,the number of moles of reactant after TEN minutes will be:

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) rarr B(g) + 2C (g) is a first order reaction with rate constant 3465 xx 10^(–6) s^(–1) . Starting with 0.1 mole of A in 2 litre vessel, find the concentration of A after 200 sec., when the reaction is allowed to take place at constant pressure and temperature.

The rate law for the reaction 2A to products is given by : rate =9.0 xx10^(-5) A mol L^(-1) S^(-1) . What is the decompostion rate when A=0.250 mol / litre ?

For given reaction A rarr Products, rate constant ' "K" ' for the reaction is 0.6 molL^(-1)min^(-1) ,If Initial concentration of reactant "A" is 8mol/L ,concentration of A after 10 minutes will be :-

For first order reaction involving 2A rarr products the specific reaction rate is 0.0084 s^(-1) . If 2.50 moles of A are taken in a 5.0 litre flask, then moles of A remaining after 60 seconds will be

For a first order for the reaction A rarr products : the rate of reaction at [A]=0.2 M is 1.0 xx 10^(-3) mol L^(-1)s^(-1) . The reaction will occur to 75% completion in .

A first order reaction with respect to reactant A , has a rate constant 6" min"^(-1) . If we start with [A]=0.5 "mol L"^(-1) , when would [A] reach the value 0.05" mol L"^(-1)