Stoichiometry and Stoichiometric Calculations

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,

$2{\mathrm{C}}_6{\mathrm{H}}_6\left(\mathrm{l}\right)+15{\mathrm{O}}_2\left(\mathrm{g}\right)\to 12{\mathrm{CO}}_2\left(\mathrm{g}\right)+6{\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right)$
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 ${\text{O}}_2=32\mathrm{,} {\mathrm{C}}_6{\mathrm{H}}_6=78$)

A chemist has prepared a solution in which the volume of water is $30\%$ of the total volume. It is observed that on adding $5\mathrm{L}$ of water in the solution, the volume of wate increases to $40\%$. What was the quantitiy of water (in litres) in original solution?

In an experiment equal weights of iron and sulphur$\left(1 \mathrm{g}\right)$ are heated together and react to form $\mathrm{FeS}$. What fraction of the original weight of excess reactant is left unreacted? $\left(\mathrm{Fe}=55.85 \mathrm{g}/\mathrm{mol} ; \mathrm{S}=32.10 \mathrm{g}/\mathrm{mol}\right)$

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

A welding fuel gas contains carbon and hydrogen only. Burning a small sample of it in oxygen gives $3.38 \mathrm{g}$ carbon dioxide. $0.690 \mathrm{g}$ of water and no other products. A volume of $10.0 \mathrm{L}$ (measured at STP) of this welding gas is found to weight $11.6 \mathrm{g}$. Calculate the molar mass of the gas.

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

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. $\left(\mathrm{Mg}=24\mathrm{u}, \mathrm{O}=16\mathrm{u}\right)$

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.

What mass of heavy water is required to yield $448 \mathrm{kL}$ of heavy hydrogen at $\mathrm{STP}$?

What volume of hydrogen in liter will be liberated at STP by the reaction of Zn on 50 ml of dilute ${\mathrm{H}}_2\mathrm{S}{\mathrm{O}}_4$ of specific gravity 1.3 having purity of 40%?
Report your answer by rounding it up to the nearest whole number.

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

What mass of calcium chloride in grams would be enough to produce $14.35 \mathrm{g}$ of $\mathrm{AgCl}$ ? (Atomic mass $\mathrm{Ca}=40,\mathrm{ }\mathrm{Ag}=108$ )

The mass of oxygen that would be required to produce enough $CO$ which completely reduces $1.6 \mathrm{k}\mathrm{g} F{e}_2{O}_3$ (at. mass of $Fe=56$ ), 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.

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