Chemical Kineti...

The reaction $${ N }_{ 2 }{ O }_{ 5 }\quad \left( In\quad { CCl }_{ 4 } \right) \rightarrow 2{ NO }_{ 2 }+{ 1 }/{ 2 }\quad { O }_{ 2 }\left( g \right) $$ is first order in $${ N }_{ 2 }{ O }_{ 5 }$$ with rate constant $$6.2\times { 10 }^{ -4 }{ S }^{ -1 }$$. What is the value of rate of reaction when $$\left[ { N }_{ 2 }{ O }_{ 5 } \right] =1.25\quad mole\quad { L }^{ -1 }$$

A certain zero order reaction has $$k = 0.025 M s^{-1}$$ for the disappearance of A. What will be the concentration of A after 15 seconds if the initial concentration is 0.50 M ? 

The rate constant for a recation is $$10.8 \times 10^{-5} mol L^{-1}S^{-1}$$. The reaction obeys:

The reaction $$ A(s) \rightarrow 2 B(g)+C(g) $$is the first order. The pressure after 20 min. and after very long time are 150 mm Hg and 225 mm Hg. The value of rate constant and pressure after 40 min. are:

$$t_{1/2} v/s \dfrac{1}{a^2}$$ is straight line graph then determine the order of a reaction:

For a first order reaction rate constant is given as $$\log K = 14 - \dfrac{1.2 \times 10^4}{T}$$ then what will be value of temperature if its half life period is $$6.93 \times 10^{-3}\ min$$?

In a first order reaction, the concentration of the reactant decreases from 0.8M to 0.4M in 15 min. The time taken for the concentration to change from 0.1 M to 0.025 M is:

K for a zero order reaction is $$2\times { 10 }^{ -2 }\quad { L }^{ -1 }{ Sec }^{ -1 }$$. If the concentration of the reactant after 25 sec is 0.5 M, the initial concentration must have been.

For a first - order reaction, the concentration of reactant:

Acid hydrolysis of ester in first order reaction and rate constant is given by $$k=\dfrac { 2.303 }{ t } log\dfrac { { V }_{ \infty  }-{ V }_{ 0 } }{ { V }_{ \infty  }-{ V }_{ t } } $$ where $${ V }_{ 0 }$$,$${ V }_{ t }$$ and $$V_{ \infty  }$$ are the volume of standard $$NaOH$$ required to neutralise acid present at a given time, if ester is $$50%$$ neutralised then: