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

The stoichiometric reaction of $516 \mathrm{g}$ of dimethyldichlorosilane with water results in a tetrameric cyclic product $\mathbf{X}$ in $75\%$ yield. The weight (in $\mathrm{g}$) of $\mathbf{X}$ obtained is ____________

[Use, molar mass $\left({\mathrm{gmol}}^{-1}\right):\mathrm{H}=1,\mathrm{C}=12,\mathrm{O}=16,\mathrm{Si}=28,\mathrm{Cl}=35.5$]

$2\mathrm{A}+3\mathrm{B}\stackrel{}{\to }4\mathrm{C}+5\mathrm{D}$

$3\mathrm{C}+4\mathrm{E}\stackrel{}{\to }5\mathrm{G} + 6\mathrm{F}$

Starting with $7 \mathrm{mol}$ of $\mathrm{A}$, $6 \mathrm{mol}$ of $\mathrm{B}$ and $8 \mathrm{mol}$of $\mathrm{E}$, find the moles of $\mathrm{G}$ formed($\mathrm{yield}=70\%$).

$1 \mathrm{g}$ alloy of $\mathrm{Cu} \text{and} \mathrm{Zn}$ reacted with excess of ${\mathrm{H}}_2{\mathrm{SO}}_4$ gives $60 \mathrm{ml}$ of ${\mathrm{H}}_2$ at $\mathrm{STP}$. What is the $\%$ of $\mathrm{Zn}$ in the alloy?

Atomic weight of $\mathrm{Cu}=63.5 \mathrm{u} \& \mathrm{Zn} = 65.4$

$56.0\mathrm{L} \mathrm{of} {\mathrm{N}}_2$ gas is mixed with excess of ${\mathrm{H}}_2$ gas and it is found that $20\mathrm{L} \mathrm{of} {\mathrm{NH}}_3$ is produced. The volume of unused ${\mathrm{N}}_2$ gas is found to be

When x grams of carbon are heated with y grams of oxygen in a closed vessel, no solid residue is left behind. Which of the following statement is correct?

$10 \mathrm{mL}$ of a gaseous hydrocarbon was exploded with sufficient oxygen. After explosion, there was a contraction of 20mL in volume. On shaking the residual gaseous mixture with $\mathrm{KOH}$, there was a further contraction of 20mL in volume. Calculate the molecular formula. All the volumes were recorded at same temperature and pressure.

If the reaction sequence given below is carried out with $15$ moles of acetylene, the amount of the product $\mathrm{D}$ formed (in $\mathrm{g}$) is

The yields of $\mathrm{A},\mathrm{B},\mathrm{C}$ and $\mathrm{D}$ are given in parentheses.

[Given: Atomic mass of $\mathrm{H}=1,\mathrm{C}=12,\mathrm{O}=16,\mathrm{Cl}=35$]

The treatment of an aqueous solution of $3.74 \mathrm{g}$ of $\mathrm{Cu}{\left({\mathrm{NO}}_3\right)}_2$ with excess $\mathrm{KI}$ results in a brown solution along with the formation of a precipitate. Passing ${\mathrm{H}}_2\mathrm{S}$ through this brown solution gives another precipitate $\mathrm{X}$. The amount of $\mathrm{X}$ (in $\mathrm{g}$) is____[Given: Atomic mass of $\mathrm{H}=1, \mathrm{N}=14, \mathrm{O}=16, \mathrm{S}=32, \mathrm{K}=39, \mathrm{Cu}=63, \mathrm{I}=127$]

Calculate the millimoles of ${{\mathrm{SeO}}_3}^{2-}$ in solution on the basis of following data:

$70 \mathrm{ml}$ of $\frac{\mathrm{M}}{60}$ solution of ${\mathrm{KBrO}}_3$ was added to ${{\mathrm{SeO}}_3}^{2-}$ solution. The bromine evolved was removed by boiling and excess of ${\mathrm{KBrO}}_3$ was back titrated with $12.5 \mathrm{ml}$ of $\frac{\mathrm{M}}{25}$ solution of ${\mathrm{NaAsO}}_2.$

The reactions are given below.

$\left(\mathrm{a}\right)$ ${\mathrm{SeO}}_3{}^{2-}+{\mathrm{BrO}}_3{}^{-}+{\mathrm{H}}^{+}\to {\mathrm{SeO}}_4{}^{2-}+{\mathrm{Br}}_2+{\mathrm{H}}_2\mathrm{O}$

$\left(\mathrm{b}\right)$ ${\mathrm{BrO}}_3^{-}+{\mathrm{AsO}}_2^{-}+{\mathrm{H}}_2\mathrm{O}\to {\mathrm{Br}}^{-}+{\mathrm{AsO}}_4^{3-}+{\mathrm{H}}^{+}$

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.)