Stoichiometry and Stoichiometric Calculations

$10 \mathrm{g}$ of each carbon and ${\mathrm{Cl}}_2$ are taken in a vessel made to react to form ${\mathrm{CCl}}_4$. Identify limiting reagent and find the mass of ${\mathrm{CCl}}_4$ obtained. Also find the mass of excess reactant remained at the end if any?

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

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 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:

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

The number of moles of ${\mathrm{KMnO}}_4$ that will be needed to react with one mole of Sulphite ion in acidic solution is       

When 4.2 g of ${\mathrm{NaHCO}}_3$ is added to a solution of acetic acid (${\mathrm{CH}}_3\mathrm{COOH}$) weighing 10.0 g, it is observed that 2.2 g of$\mathrm{CO}$₂ is released into the atmosphere. The residue left behind is found to weigh 12.0 g. Show that these observations are in agreement with the law of conservation of mass.

Calculate the amount of ${\mathrm{H}}_2$ which is left unreacted in the given reaction:

$2{\mathrm{H}}_2+{\mathrm{O}}_2\to 2{\mathrm{H}}_2\mathrm{O}$

If $8\mathrm{gm}$ of ${\mathrm{H}}_2$ is mixed with $16\mathrm{gm}$ of ${\mathrm{O}}_2$.

Calculate the weight of lime obtained by $200 \mathrm{kg}$ heating of $95\%$ pure lime stone.

$20\mathrm{g}$ of sugar is dissolved in water to make $100\mathrm{g}$ of solution.Determine the mass percentage of sugar.

A solution contains $20 \mathrm{g}$ of sugar in $80 \mathrm{g}$ of water. calculate the concentration of solution in terms of mass percent.

The mass of $CaC{O}_3$ required to react with $25 \mathrm{m}\mathrm{L}$ of $0.75\mathrm{M}HCl$ is

$1.2 g$ of $Mg$ (at. mass $24$) will produce $MgO$ equal to

One mole of organic compound is subjected to combustion by dumas method. On combustion it gives 6 moles of $C{O}_2$ , 1 mole of $N_2$ and 4 moles of $H_{2}O$ . Determine the formula.

When $32.25gm$ ethyl chloride dehydro halogenated, if gives $50\%$ . Alkene, what is the mass of product. (atomic mass of chlorine $= 35.5$ )

If $30 ml$ of $H_2$ and $20 ml$ of $O_2$ reacts to form water, what is left at the end of the reaction

What will be the volume of $C{O}_2$ at S.T.P., obtained by heating $9.85 g$ of $BaC{O}_3$ (Atomic number of $Ba = 137$ )

In the reaction $4\mathrm{A}+2\mathrm{B}+3\mathrm{C}\to {\mathrm{A}}_4\mathrm{ }{\mathrm{B}}_2\mathrm{ }{\mathrm{C}}_3,$ what will be the number moles of product formed, starting from one mole of $\mathrm{A},\hspace{0.17em}0.6$ moles of $\mathrm{B}$ and $\mathrm{0}.72$ moles of $\mathrm{C}\hspace{0.17em}?$