Chemical Kineti...

$$A_{(g)}  \rightarrow  B_{(g)}$$ is a first order reaction. The initial concentration of A is 0.2mol $$l^{-1}$$ . After 10 minutes, the concentration of B is found to be 0.18mol $$l^{-1}$$ . Calculate rate constant of the reaction?

The concentration of reaction decreases from 0.2M to 0.05M in 5 minutes. The rate of reaction in $$mol. lit^{-1}.s^{-1}$$ is:

The rate constant of a first order reaction is $$0.0693$$ $$min^{-1}$$. 

From the graph, pick out the correct one :

A first order reaction was commenced with 0.2 M solution of the reactants. If the molarity of the solution falls to $$0.02M$$ after 100 minutes the rate constant of the reaction is:

The amount left after completion of average life period in a first order reaction is :

With respect to the figure which of the following statement is correct?

Statement - I : The reactions $$2NO+O_{2}\rightarrow 2NO_{2}$$ and $$2CO+O_{2}\rightarrow 2CO_{2}$$ proceed at the same rate because they are similar.
Statement - II Above two reactions will have different activation energies.

A first-order reaction is carried out with an initial concentration of $$10$$ mole per litre and $$80$$% of the reactant changes into the product. Now if the same reaction is carried out with an initial concentration of $$5$$ mol per litre, the percentage of the reactant changing to the product is:

A first order reaction A $$\rightarrow$$ products has k$$=$$6.93 $$min^{-1}$$ . If 90% of first order reaction B $$\rightarrow$$ products is completed in the time taken by 50% of the first reaction, what is the rate constant for the second reaction?