Chemical Kineti...

Select the correct statements out of I, II and III for zero order reaction.
I: Quantity of the product formed is directly proportional to time.
II: Larger the initial concentration of the reactant, greater the half-life period.
III: If 50% reaction takes place in 100 minutes, 75% reaction take place in 150 minutes.

For a reaction $$P \rightarrow Q$$, the half-life of the reaction was 3h, when the initial concentration of P was 0.5M. As the concentration of P was increased to 1.0M, half life changes to 6h. The order of reaction with respect to P is:

For the $$1^{st}$$ order reaction, $$A(g) \rightarrow 2B(g) + C(s),$$ $$t_{1/2}= 24 $$ min. The reaction is carried out by taking a certain mass of 'A' enclosed in a vessel in which it exerts a pressure of 400 mm Hg. The pressure of the reaction mixture after the expiry of 48 min will be:

The gaseous decomposition reaction: $$A(g)\rightarrow 2B(g) + C(g)$$, is observed to first order over the excess of liquid water at $$25^oC$$. It is found that after 10 minutes, the total pressure of the system is 188 torr and after a very long time it is 388 torr. Calculate the rate constant of the reaction in $$hr^{-1}$$. The vapour pressure of $$H_2O$$ at $$25^oC$$ is 28 torr. $$[ln 2 = 0.7,\: ln 3 = 1.1, \: ln 10 = 2.3]$$

Given $$X \rightarrow$$  product (Taking $$1^{st}$$ order reaction)

conc of $$X$$ (mol/lit.)	$$0.01$$	$$0.0025$$
Time (min.)	$$0$$	$$40$$

Half life period of this reaction is :

Two substances A $$(t_{\frac 12} =$$ 5 min) and B $$(t_{\frac 12} =$$ 15 min) are taken in such a way that initially $$[A] = 4[B]$$. The time after which both the concentrations will be equal is:

It takes 32 minutes to complete 99% of a first order reaction from start. Calculate the time required (in a minute) to complete 99.9% of the reaction from the start?

The conversion of vinyl allyl ether to pent-4-enol follows first-order kinetics. The following plot is obtained for such a reaction. Determine rate constant for the reaction.

Half-life is independent of the concentration of the reactant. After $$10$$ minutes, the volume of $$N_{2}$$ gas is $$10\ L$$ and after complete reaction, it is $$50\ L$$. Hence, the rate constant is:

In the reaction, $$2N_2O_5\rightarrow 4NO_2+O_2$$, initial pressure is $$500\ atm$$ and rate constant $$k$$ is $$3.38\times 10^{-5} sec^{-1}$$. After 10 minutes the final pressure of $$N_2O_5$$ is: