A mixture of N2 and H2 is caused to react in a closed container to form Nh3. Reaction ceases before any reactant has been totally consumed.At this stage 2 moles each of N2, H2 and Nh3 are present. Weight of N2 and H2 present originally were

Q. In a reaction $N_2+3H_2\to 2N{H}_3$, 40 ml of each $N_2$ and $H_2$ are taken to react together so that $25\%$ yield of $N{H}_3$ was obtained. The volume of $N_2$ present in the container is?

Q. $34$ gm of a mixture containing $N_2$ and $H_2$ in $1:3$ by mole is partially converted into ${NH}_3$. Calculate the vapour density of the mixture (containing remaining $N_2,H_2$ and ${NH}_3$ formed) after reaction if it has been found that the ${NH}_3$ formed required $0.5$ moles of $H_3{PO}_4$ for complete neutralization.

Q. In a reaction $N_2+3H_2\to 2N{H}_3$, 40 ml of each $N_2$ and $H_2$ are taken to react together so that $25\%$ yield of $N{H}_3$ was obtained. The volume of $N_2$ present in the container is?

Q. 28g of $N_2$ and 6g of $H_2$ were mixed. At equilibrium 17g of $N{H}_3$ was formed. The weight of $N_2$ and $H_2$ at equilibrium are _________ respectively.

Q. An equilibrium mixture of $N_2,H_2$ and $N{H}_3$ at $700$K contains $0.036$M $N_2$ and $0.15$M $H_2$. At this temperature, $K_c$ for the reaction $N_2\left(g\right)+3H_2\left(g\right)\rightleftharpoons 2N{H}_3\left(g\right)$ is $0.29$. What is the concentration of $N{H}_3$?