Chemical Kineti...

The rate for a first order reaction is $$0.6932 \times 10^{-2}$$ mol litre$$^{-1}$$ min$$^{-1}$$ and the initial concentration of the reactant is 1 M, $$t_{1/2}$$ is equal to:

For a reaction following first-order kinetics, which of the following statements is/are correct ?

The rate constant for two parallel reactions were found to be $$1.0\times 10^{-2}dm^{3}$$ $$mol^{-1}s^{-1}$$ and $$3.0\times 10^{-2}dm^{3}$$ $$mol^{-1}s^{-1}$$. If the corresponding energies of activation of the parallel reactions are 60.0 KJ $$mol^{-1}$$ and 70.0 KJ $$mol^{-1}$$ respectively, then what is the apparent overall energy of activation?

Consider an endothermic reaction $$X \rightarrow Y$$ with the activation energies  $$E_{b}$$ and $$E_{f}$$ for the backward and forward reactions respectively. In general:

At $$100^{0}C$$ , the gaseous reaction $$A \rightarrow 2B + C$$ is found to be of first order. Starting with pure $$A$$, if at the end of 10 min, the total pressure of the system is 140 mm and after a long time it is 300 nm, the partial pressure of $$A$$ at the end of 10 min is:

A substance $$A$$ decomposes in a solution following first-order kinetics. Flask I contains 1L of a 1M solution of $$A$$ and flask II contains 100 ml of a 0.6 M solution. After 8 hours the concentration of $$A$$ in flask I has become 0.50 M. What will be the time taken for the concentration of $$A$$ in flask II to become 0.3 M?

The rate of a first-order reaction is $$1.5\times 10^{-2}\ mol\ L^{-1}\ min^{-1}$$ at $$0.5$$ M concentration of the reactant. The half-life of the reaction is:

The total pressure after 200 seconds, if the initial pressure is $$0.1$$ atm is _______ .

The time required for the decomposition of $$N_{2}O_{5}$$, so that the total pressure becomes 0.15 atm is ___________.