Chemistry - Chemical Kinetics Question with Solution | TestHub

The decomposition of ${\mathrm{N}}_2{\mathrm{O}}_5$ according to the equation:

$$2{\mathrm{N}}_2{\mathrm{O}}_5(g)⟶4\mathrm{N}{\mathrm{O}}_2(g)+{\mathrm{O}}_2(g)$$

is a first-order reaction. After 30 minutes from the start of the decomposition in a closed vessel, the total pressure developed is found to be 289.1 mm of Hg. On complete decomposition, the total pressure is 590 mm of Hg. Calculate the rate constant of the reaction in $h{r}^{-1}$. (Given: ${\log }_{10}2=0.30$, ${\log }_{10}17=1.23$, $\ln x=2.303{\log }_{10}x$)