Stoichiometry and Stoichiometric Calculations

In the Haber process $30 \mathrm{litre}$ of dihydrogen and $30 \mathrm{litres}$ of dinitrogen were taken for reaction which yielded only  $50\%$ of the expected product. What will be the composition of gaseous mixture under the aforesaid condition in the end?

In Haber's process, $30 \mathrm{litres}$ of dihydrogen and $30 \mathrm{litres}$ of dinitrogen were taken for the reaction, which yielded only $50\mathrm{\%}$ of the expected product. What will be the composition of the gaseous mixture under the aforesaid condition in the end?

Assuming full decomposition, the volume of  ${\mathrm{CO}}_2$ released at STP on heating  $9.85\hspace{0.17em}\mathrm{g}\hspace{0.17em}\mathrm{of}\hspace{0.17em}{\mathrm{BaCO}}_3$ (Atomic mass, $Ba=137$) will be:

Liquid benzene  $\left({\mathrm{C}}_6{\mathrm{H}}_6\right)$ burns in oxygen according to the equation

$2{\mathrm{C}}_6{\mathrm{H}}_6\left(\mathrm{l}\right)+15{\mathrm{O}}_2\left(\mathrm{g}\right)\to 12{\mathrm{CO}}_2\left(\mathrm{g}\right)+6{\mathrm{H}}_2\mathrm{O}\left(\mathrm{g}\right)$

How many litres of  ${\mathrm{O}}_2$ at STP are needed to complete the combustion of $39 \mathrm{g}$ of liquid benzene?  $(\mathrm{Molecular}\mathrm{weight}\mathrm{of}{\mathrm{O}}_2=32,{\mathrm{C}}_6{\mathrm{H}}_6=78)$

Liquid benzene $\left({\mathrm{C}}_6{\mathrm{H}}_6\right)$ burns in oxygen according to the equation,

$2{\mathrm{C}}_6{\mathrm{H}}_6\left(\mathrm{l}\right)+15{\mathrm{O}}_2\left(\mathrm{g}\right)\to 12{\mathrm{CO}}_2\left(\mathrm{g}\right)+6{\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right)$
How many litres of ${\mathrm{O}}_2$ at $\mathrm{STP}$ are needed to complete the combustion of $39 \mathrm{g}$ of liquid benzene? (Molecular weight of ${\text{O}}_2=32\mathrm{,} {\mathrm{C}}_6{\mathrm{H}}_6=78$)

$64.5\%$ pure sample of zinc when treated with excess of dil.$\mathrm{HCl}$ liberated some volume of hydrogen gas at STP. This hydrogen is utilised for the reduction of $23.2 \mathrm{g}$ ${\mathrm{Fe}}_3{O}_4$. Find out the amount of iron obtained and also the amount of impure zinc taken. [atomic mass of $\mathrm{Zn}=65.5 \mathrm{and} \mathrm{Fe}=56$].

Balance the following chemical reaction by identifying the products:

${\mathrm{Al}}_2{\mathrm{O}}_3 +{\mathrm{N}}_2+\mathrm{C}\to \mathrm{AlN}+ \mathrm{\_\_\_\_\_}$

Balance the following chemical reaction by identifying the product:

${\mathrm{Fe}}_3{\mathrm{O}}_4 + \mathrm{HCl}\to {\mathrm{FeCl}}_2+ {\mathrm{FeCl}}_3+ \mathrm{\_\_\_\_\_}$

Balance the following chemical reaction by identifying the product:

${\mathrm{PCl}}_5 + {\mathrm{H}}_2\mathrm{O}\to {\mathrm{H}}_3{\mathrm{PO}}_4+ \mathrm{\_\_\_\_\_}$

Balance the following chemical reaction by identifying the product:

${\mathrm{CuSO}}_4 + \mathrm{HI}\to {\mathrm{CuI}}_2+ \mathrm{\_\_\_\_\_}$

How many grams of magnesium nitrate should be heated to produce oxygen which is just sufficient to form $15.3 \mathrm{g}$ of alumina?

The gaseous product left after condensation is CO2One mole of hydrocarbon is subjected to combustion. The product obtained is condensed and the resulting gaseous product occupied a volume of $89.6 \mathrm{L}$ at STP. Oxygen required for this combustion is $145.6 \mathrm{L}$ at STP. What should be the molecular formula of x?

Calculate the amount of potassium chloride obtained by the thermal decomposition of $12.25 \mathrm{kg}$ of potassium chlorate.

Calculate the amount of mercury obtained by the decomposition of $2.16 \mathrm{kg}$ of mercuric oxide. 

Calculate the weight $\left(\mathrm{g}\right)$ of $5\times {10}^{24}$ molecules of nitrogen dioxide. 

Calculate the weight of helium gas which occupy a volume $3.36 {\mathrm{dm}}^3$ at STP.

Calculate the weight of hydrogen gas which occupy a volume $3.36 {\mathrm{dm}}^3$ at STP.