Chemical Equations and Stoichiometry

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 ${\text{O}}_2=32\mathrm{,} {\mathrm{C}}_6{\mathrm{H}}_6=78$)

For the reaction ${\mathrm{SO}}_{2\left(\mathrm{g}\right)}+\frac{1}{2}{\mathrm{O}}_{2\left(\mathrm{g}\right)}\rightleftharpoons {\mathrm{SO}}_{3\left(\mathrm{g}\right)}$$,$the percentage yield of product at different pressures is shown in the figure. Then. which among the following is true?

Calculate the amount of hydrogen gas required in order to produce $100 \mathrm{g}$ of ammonia by the reaction of ${\mathrm{N}}_2\left(g\right)$ and ${\mathrm{H}}_2\left(\mathrm{g}\right)$ gases.

Gastric juice contains about $3.0 \mathrm{g}$ of $\mathrm{HCl}$ per liter. If a person produces about $2.6$ liters of gastric juice per day, find the number of antacid tablets required to neutralize all the $\mathrm{HCl}$ produced. Consider each antacid tablet contains $400 \mathrm{mg}$ of $\mathrm{Al}(\mathrm{OH}{)}_3.$ Given atomic masses: $\mathrm{Al}\to 27,0\to 16,\mathrm{H}\to 1,\mathrm{Cl}\to 35.5.$

The amount of arsenic pentasulphide that can be obtained when $35.5 \mathrm{g}$ arsenic acid is treated with excess ${\mathrm{H}}_2\mathrm{S}$ in the presence of conc. $\mathrm{HCl}$ (assuming $100\%$ conversion) is

A gaseous hydrocarbon gives upon combustion $0.72 \mathrm{g}$ of water and $3.08 \mathrm{g}$ ${\mathrm{CO}}_2$. What is the empirical formula of the hydrocarbon?

$5 \mathrm{L}$ of an alkane requires $25 \mathrm{L}$ of oxygen for its complete combustion. If all volumes are measured at constant temperature and pressure, the alkane is

When $22.4$ litres of ${\mathrm{H}}_2\left(\mathrm{g}\right)$ is mixed with $11.2$ litres of $\mathrm{C}{\mathrm{l}}_2\left(\mathrm{g}\right),$ each at STP, the moles of $\mathrm{H}\mathrm{C}\mathrm{l}\left(\mathrm{g}\right)$ formed is equal to

If $1.5 \mathrm{moles}$of oxygen combine with $\mathrm{Al}$ to form ${\mathrm{Al}}_2{\mathrm{O}}_3$, the mass of $\mathrm{Al}$ in $\mathrm{g}$ (Atomic mass of $\mathrm{Al}=27$) used in the reaction is

What weights of ${\mathrm{P}}_4{\mathrm{O}}_6$ and ${\mathrm{P}}_4{\mathrm{O}}_{10}$ will be produced by the combustion of $31 \mathrm{g}$ of ${\mathrm{P}}_4$ in $32 \mathrm{g}$ of oxygen leaving no ${\mathrm{P}}_4$ and ${\mathrm{O}}_2$.

In an experiment, pure carbon monoxide was passed over red-hot copper oxide. ${\mathrm{CO}}_2,$ so produced, weighed $0.88 \mathrm{g}$ and the weight of copper oxide was reduced by $0.3232 \mathrm{g}$. Calculate the atomic weight of carbon. [ Take molar mass of carbon dioxide =$44\mathrm{g}$ ]

An alloy of aluminium and copper was treated with aqueous $\mathrm{HCl}$. The aluminium dissolved according to the reaction $\mathrm{Al}+3{\mathrm{H}}^{+}\to {\mathrm{Al}}^{3+}+\frac{3}{2}{\mathrm{H}}_2$, but the copper remained as a pure metal. A $0.350 \mathrm{g}$ sample of the alloy gave $415 \mathrm{cc}$ of ${\mathrm{H}}_2$ measured at $273 \mathrm{K}$ and $1 \mathrm{atm}$ pressure. What is the weight percentage of $\mathrm{Al}$ in the alloy?

Give the final answer after rounding off to two significant figures.

When a mixture of $\mathrm{NaBr}$ and $\mathrm{NaCl}$ is repeatedly digested with sulphuric acid, all the halogens are expelled and ${\mathrm{Na}}_2{\mathrm{SO}}_4$ is formed quantitatively. With a particular mixture, it was found that the weight of ${\mathrm{Na}}_2{\mathrm{SO}}_4$ obtained was precisely the same as the weight of $\mathrm{NaBr}-\mathrm{NaCl}$ mixture taken. Calculate the ratio of the weights of $\mathrm{NaCl}$ and $\mathrm{NaBr}$ in the mixture.

(Note: Report your answer after multiplying with 100 and rounding up to the nearest integer value.)