For the given first order reaction

$$\mathrm{A} \rightarrow \mathrm{B}$$

the half life of the reaction is $$0.3010 \mathrm{~min}$$. The ratio of the initial concentration of reactant to the concentration of reactant at time $$2.0 \mathrm{~min}$$ will be equal to ___________. (Nearest integer)

$$\matrix{ {[A]} & \to & {[B]} \cr {{\mathop{\rm Reactant}\nolimits} } & {} & {{\mathop{\rm Product}\nolimits} } \cr } $$

If formation of compound $$[\mathrm{B}]$$ follows the first order of kinetics and after 70 minutes the concentration of $$[\mathrm{A}]$$ was found to be half of its initial concentration. Then the rate constant of the reaction is $$x \times 10^{-6} \mathrm{~s}^{-1}$$. The value of $$x$$ is ______________. (Nearest Integer)

$$2 \mathrm{NO}+2 \mathrm{H}_{2} \rightarrow \mathrm{N}_{2}+2 \mathrm{H}_{2} \mathrm{O}$$

The above reaction has been studied at $$800^{\circ} \mathrm{C}$$. The related data are given in the table below

Reaction serial number | Initial Pressure of $${H_2}/kPa$$ | Initial Pressure of $$NO/kPa$$ | Initial rate $$\left( {{{ - dp} \over {dt}}} \right)/(kPa/s)$$ |
---|---|---|---|

1 | 65.6 | 40.0 | 0.135 |

2 | 65.6 | 20.1 | 0.033 |

3 | 38.6 | 65.6 | 0.214 |

4 | 19.2 | 65.6 | 0.106 |

The order of the reaction with respect to NO is ___________.

For a reaction $$\mathrm{A} \rightarrow 2 \mathrm{~B}+\mathrm{C}$$ the half lives are $$100 \mathrm{~s}$$ and $$50 \mathrm{~s}$$ when the concentration of reactant $$\mathrm{A}$$ is $$0.5$$ and $$1.0 \mathrm{~mol} \mathrm{~L}^{-1}$$ respectively. The order of the reaction is ______________ . (Nearest Integer)