One volume of nitrogen combines with one volume of oxygen to form two volumes of nitric oxide. Calculate the amount of each reactant required to produce 250 ml of nitric oxide.

Q. In the reaction:
$CO+\frac{1}{2}{O}_2\left(g\right)\to C{O}_2;N_2+O_2\to 2NO$
$10\text{mL}$ of mixture containing carbon monoxide and nitrogen required $7\text{mL}$ oxygen to form $C{O}_2$ and $NO$, on combustion. The volume of $N_2$ in the mixture will be:

Q. In the formation of nitric acid, $N_2$ and $O_2$ are made to combine. Which of the following condition will favour the formation of $NO$?
$N_2+O_2\rightleftharpoons 2NO+Heat$

Q. The equilibrium established in a reaction vessel of $2.5$L capacity. The amounts of $N_2$ and $O_2$ taken at the start were respectively $2$ moles and $4$ moles. Half a mole of nitrogen has been used up at equilibrium. The molar concentration of nitric oxide is:

Q. The half life decomposition of $N_2{O}_5$ in a first order reaction represented by
$N_2{O}_5\to N_2{O}_4+\frac{1}{2}{O}_2$
After 20 min the volume of $O_2$ produced is 10 ml and at the end of the reaction 40 ml. The value of rate constant is: $\left[Given2.303\log \left(\frac{4}{3}\right)=0.28\right]$

Q. According to Graham's Law, the rate of diffusion of $CO,O_2,N_{2}andC{O}_2$ follows the order: