Chemical Kineti...

What is overall activation energy of reaction, if steps (1) to (4) are much faster than (5)?

Arrhenius equation gives the change in rate constant (and hence rate of reaction) with temperature. If the activation energy of the reaction is found to be equal to $$RT$$, then

Two reactions: (I) $$A\rightarrow products$$ and (II) $$B\rightarrow products$$, follow first-order kinetics. The rate of reacion-I is doubled when temperature is raised from $$300$$ to $$310K$$. The half-life for this reaction at $$310K$$ is $$30min$$. At the same temperature, $$B$$ decomposes twice as fast as $$A$$. If the energy of activation for the reaction II is half that of reaction I, the rate constant of reaction II at $$300K$$ is

For a zero-order reaction: $$2{ NH }_{ 3 }(g)\rightarrow { N }_{ 2 }(g)+3{ H }_{ 2 }(g)$$, the rate of reaction is $$0.1atm/s$$. Initially only $${ NH }_{ 3 }(g)$$ was present at $$3atm$$ and the reaction is performed at constant volume and temperature. The total pressure of gases after $$10s$$ from the start of reaction will be

Desorption of a gas from metal surface follows first-order kinetics. The rate constant of desorption can be given by Arrhenius equation. If the desorption of hydrogen on manganese is found to increase $$10$$ times on increasing the temperature from $$600$$ to $$1000 K$$, the activation energy of desorption is :

Rate of an uncatalyzed first-order reaction at $$T$$ $$K$$ is half of the rate of a catalyzed reaction at $$0.5T$$ $$T$$. If the catalyst lowers the threshold energy by $$20\ kcal$$, what is the activation energy of the uncatalyzed reaction?
$$\left( T=300K,\ln { 2 } =0.7 \right) $$

Which of the following curves represents a zero order reaction?

Which of the following curves represents a first order reaction?

The reaction $$A+B\to C+D;\ \Delta H=25\ kJ/ mole$$ should have an activation energy :

The plot of concentration of a reactant vs time for a chemical reaction is shown below :
The order of this reaction with respect to the reactant is: