Chemical Equations and Stoichiometry

Aluminium reacts with sulfuric acid to form aluminium sulfate and hydrogen. What is the volume of hydrogen gas in liters $\left(\mathrm{L}\right)$ produced at $300 \mathrm{K}$ and $1.0$ atm pressure, when $5.4 \mathrm{g}$ of aluminium and $50.0 \mathrm{mL}$ of $5.0 \mathrm{M}$ sulfuric acid are combined for the reaction? (Use molar mass of aluminium as $27.0 \mathrm{g}{ \mathrm{mol}}^{-1}, \mathrm{R}=0.082 \mathrm{atm} \mathrm{L}{ \mathrm{mol}}^{-1}{ \mathrm{K}}^{-1}$)

$1$ litre of aliphatic compound ${\mathrm{C}}_{\mathrm{x}}{\mathrm{H}}_{\mathrm{y}}{\mathrm{O}}_{\mathrm{z}}$ is completely burnt in an excess of ${\mathrm{O}}_2$ and cooled to room temperature. The reacted volume of oxygen will be

$1$ litre of gaseous aliphatic compound ${\mathrm{C}}_{\mathrm{x}}{\mathrm{H}}_{\mathrm{y}}{\mathrm{O}}_{\mathrm{z}}$ is completely burnt in excess of ${\mathrm{O}}_2$ and cooled to room temperature. The contraction in volume is

$1$ mole of gaseous aliphatic compound ${\mathrm{C}}_{\mathrm{x}}{\mathrm{H}}_{3\mathrm{n}}{\mathrm{O}}_{\mathrm{m}}$ is completely burnt in excess of ${\mathrm{O}}_2.$ The no. of moles of ${\mathrm{H}}_2\mathrm{O}$ is formed

$1 \mathrm{mol}$ of gaseous compound ${\mathrm{C}}_{\mathrm{n}}{\mathrm{H}}_{3\mathrm{n}}{\mathrm{O}}_{\mathrm{m}}$ is completely burnt in excess of ${\mathrm{O}}_2.$ The number of moles of ${\mathrm{CO}}_2$ formed is

$1$ mole of aliphatic compound ${\mathrm{C}}_{\mathrm{n}}{\mathrm{H}}_{3\mathrm{n}}{\mathrm{O}}_{\mathrm{m}}$ is completed burnt in an excess of ${\mathrm{O}}_2.$ The number of moles of oxygen reacted are

$1 \mathrm{ml}$ of gaseous aliphatic compound ${\mathrm{C}}_{\mathrm{n}}{\mathrm{H}}_{3\mathrm{n}}{\mathrm{O}}_{\mathrm{m}}$ is completely burnt in an excess of ${\mathrm{O}}_2$ and cooled to room temperature. The contraction in volume is

An element $\mathrm{A}$ reacts with compound ${\mathrm{BO}}_3$ to produce ${\mathrm{A}}_3{\mathrm{O}}_4$ and ${\mathrm{B}}_2{\mathrm{O}}_3.$ The no. of moles of ${\mathrm{A}}_3{\mathrm{O}}_4$ produced if one mole each of $\mathrm{A}$ and ${\mathrm{BO}}_3$ is reacted?

When a gaseous olefinic hydrocarbon is burnt completely in excess of ${\mathrm{O}}_2$, a contraction in volume equal to double to the volume of hydrocarbon is noticed then hydrocarbon will be

One mole of ${\mathrm{KClO}}_3$ is heated in presence of ${\mathrm{MnO}}_2.$ The produced oxygen is used in burning of $\mathrm{Al}.$ Then oxide of $\mathrm{Al}$ that will be formed

$4.6 \mathrm{g} \mathrm{Na}$ is dissolved in $1$ litre of water. Then how much ${\mathrm{H}}_2$ gas will be evolved at S.T.P.?

$1.16 \mathrm{g}$ of Metal $\mathrm{M}$ react with excess of ${\mathrm{O}}_2$ and convert all metal $\mathrm{M}$ into ${\mathrm{M}}_3{\mathrm{O}}_2\left(\mathrm{s}\right).$ The maximum amount of ${\mathrm{M}}_3{\mathrm{O}}_2\left(\mathrm{s}\right)$ produced is (atomic mass of $\mathrm{M}=58 \mathrm{g} {\mathrm{mol}}^{–1}$)

A mixture of ${\mathrm{CaCl}}_2$ and $\mathrm{NaCl}$ weighing $3.70 \mathrm{gm}$ is treated with ${\mathrm{Na}}_2{\mathrm{CO}}_3$ solution to precipitate all the ${\mathrm{Ca}}^{2+}$ ions as ${\mathrm{CaCO}}_3.$ The ${\mathrm{CaCO}}_3$ so obtained is heated strongly to get $0.84 \mathrm{gm}$ of $\mathrm{CaO}.$ The percentage of $\mathrm{NaCl}$ in the mixture is _____.

$\mathrm{n}$-butane is produced by monobromination of ethane followed by Wurtz reaction. Calculate volume of ethane in litres at STP to produce $29 \mathrm{g}$ of $\mathrm{n}$-butane if bromination takes place with $80\%$ yield and the Wurtz reaction with $56\%$ yield. The reactions involved are

(i) ${\mathrm{C}}_2{\mathrm{H}}_6+{\mathrm{Br}}_2 \underset{125°\mathrm{C}}{\overset{\mathrm{hv}}{\to }} {\mathrm{C}}_2{\mathrm{H}}_5\mathrm{Br}+\mathrm{HBr}$
(ii) $2{\mathrm{C}}_2{\mathrm{H}}_5\mathrm{Br}+2\mathrm{Na} \stackrel{\mathrm{Ether}}{⟶} {\mathrm{C}}_4{\mathrm{H}}_{10}+2\mathrm{NaBr}$ (Wurtz reaction)

$29.2\% \left(\frac{\mathrm{w}}{\mathrm{w}}\right) \mathrm{HCl}$ stock solution has a density of $1.15 \mathrm{g}{ \mathrm{mL}}^{-1}.$ The molecular mass of $\mathrm{HCl}$ is $36.5 \mathrm{g} {\mathrm{mole}}^{–1}.$ The volume in $\mathrm{mL}$ of stock solution is required to prepare a $460 \mathrm{mL}$ solution of $0.4 \mathrm{M} \mathrm{HCl}$ is _____.

$20.3 \mathrm{g}$ sample of pure ${\mathrm{MgCl}}_2.{\mathrm{xH}}_2\mathrm{O}$ on heating form $10.8 \mathrm{g}$ water and anhydrous ${\mathrm{MgCl}}_2.$ The value of $x$ is (Molecular mass of ${\mathrm{MgCl}}_2=95$)

$40 \mathrm{g}$ of metal oxide $\left(\mathrm{MO}\right)$ contain $4 \mathrm{g}$ of oxygen.
The equivalent weight of metal is

The volume of ${\mathrm{O}}_2$ obtained at STP, when $12.25 \mathrm{g}$ of ${\mathrm{KClO}}_3$ is decomposed, is (Molar mass of ${\mathrm{KClO}}_3=122.5 \mathrm{g} {\mathrm{mol}}^{–1}$)
${\mathrm{KClO}}_3\stackrel{\mathrm{\Delta }}{⟶}\mathrm{KCl}+\frac{3}{2}{\mathrm{O}}_2$

$1.5$ moles of ${\mathrm{ClO}}_2$ react with $72 \mathrm{g}$ of ${\mathrm{O}}_3$ according to reaction : $2{\mathrm{ClO}}_2+2{\mathrm{O}}_3⟶{\mathrm{Cl}}_2{\mathrm{O}}_6+2{\mathrm{O}}_2.$ $0.6$ moles of ${\mathrm{Cl}}_2{\mathrm{O}}_6$ is formed. What is the percent yield of reaction?

$0.5 \mathrm{g}$ of fuming ${\mathrm{H}}_2{\mathrm{SO}}_4$ oleum is diluted with $100 \mathrm{mL}$ of water. This solution is completely neutralised by $26.7 \mathrm{ml}$ of $0.4 \mathrm{N} \mathrm{NaOH}.$ The correct statement is/are