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?

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

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

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.)

One litre of an acidified solution of ${\mathrm{KMnO}}_4$ containing $15.8 \mathrm{g}$ of ${\mathrm{KMnO}}_4$ is decolourised by passing a sufficient amount of ${\mathrm{SO}}_2$. If ${\mathrm{SO}}_2$ is produced by roasting of iron pyrites $\left({\mathrm{FeS}}_2\right)$, what will be the amount of pyrites (in grams) required to produce the necessary amount of ${\mathrm{SO}}_2$?

(Atomic mass of $\mathrm{K}=39, \mathrm{Mn}=55, \mathrm{S}=32, \mathrm{O}=16, \mathrm{Fe}=56, \mathrm{H}=1$)

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

The compound $N{a}_{2}C{O}_3\cdot x{H}_{2}O$ has $50\% H_{2}O$ by mass. The value of $"x"$ is

A closed $10 \mathrm{L}$ vessel contains $1 \mathrm{L}$ water gas $\left(1:1\mathrm{CO}:{\mathrm{H}}_2\right)$ and $9 \mathrm{L}$ air ($20\%{\mathrm{O}}_2$ by volume) at $\mathrm{STP}$. The contents of the vessel are ignited. The number of moles of ${\mathrm{CO}}_2,$ in the vessel is closest to :

The following process has been used to obtain iodine from oil-field brines in California.

$\mathrm{NaI}+{\mathrm{AgNO}}_3⟶\mathrm{AgI}+{\mathrm{NaNO}}_3$

$2\mathrm{AgI}+\mathrm{Fe}⟶{\mathrm{FeI}}_2+2\mathrm{Ag}$

$2{\mathrm{FeI}}_2+3{\mathrm{Cl}}_2⟶2{\mathrm{FeCl}}_3+2{\mathrm{I}}_2$

How many grams of ${\mathrm{AgNO}}_3$ are required in the first step for every $254 \mathrm{kg} {\mathrm{I}}_2$ produced in the third step? 

Equal weights of $\text{'}\mathrm{X}\text{'}$(atomic weight$=36$) and $\text{'}\mathrm{Y}\text{'}$ (atomic weight$=24$) react to form the compound, ${\mathrm{X}}_2{\mathrm{Y}}_3$.  If that is the case, then

What volume of hydrogen gas will be consumed at $273 \mathrm{K}$ and $1 \mathrm{atm}$ pressure to obtain $21.6 \mathrm{g}$ of elemental boron (atomic mass$=10.8$ ) from the reduction of boron trichloride with hydrogen?

$25 \mathrm{mL}$ solution of barium hydroxide on titration with $0.1$ molar solution of hydrochloric acid gave a titre value of $35 \mathrm{mL}$. The molarity of barium hydroxide is:

The amount (in mol) of bromoform ${\mathrm{CHBr}}_3$ produced when $1.0$ mole of acetone reacts completely with $1.0$ mole of bromine in the presence of aqueous $\mathrm{NaOH}$ is

How many grams of ${\mathrm{O}}_2$ is required for the combustion of $480$gram of $\mathrm{Mg}$? Find the mass of $\mathrm{MgO}$formed in this reaction. $\left(\mathrm{Mg}=24\mathrm{u}, \mathrm{O}=16\mathrm{u}\right)$

Which of the following weighs the most?

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