Stoichiometry and Stoichiometric Calculations

Calculate the amount of potassium chloride obtained by the thermal decomposition of $12.25 \mathrm{kg}$ of potassium chlorate.

Calculate the amount of mercury obtained by the decomposition of $2.16 \mathrm{kg}$ of mercuric oxide. 

Calculate the weight $\left(\mathrm{g}\right)$ of $5\times {10}^{24}$ molecules of nitrogen dioxide. 

Calculate the weight of helium gas which occupy a volume $3.36 {\mathrm{dm}}^3$ at STP.

Calculate the weight of hydrogen gas which occupy a volume $3.36 {\mathrm{dm}}^3$ at STP.

Calculate the weight of nitrogen gas which occupy a volume $3.36 {\mathrm{dm}}^3$ at STP.

$2{\mathrm{C}}_2{\mathrm{H}}_6 + 7{\mathrm{O}}_2 \to 4{\mathrm{CO}}_2 + 6{\mathrm{H}}_2\mathrm{O}$

$60 {\mathrm{dm}}^3$ of ethane is mixed with $448 {\mathrm{dm}}^3$ of pure oxygen at STP. If the mixture is ignited and reacts as illustrated in the above reaction, calculate the volume of ${\mathrm{CO}}_2$ formed. 

Calculate the volume occupied by $0.8 \mathrm{g}$ of methane at STP. 

$84 \mathrm{g}$ of a gas occupies the same volume as $96.00 \mathrm{g}$ of oxygen under similar conditions of temperature and pressure. The molecular weight of the gas is $(\mathrm{O}=16)$.

Equal mass of oxygen, hydrogen and methane are taken in a container in identical conditions. What is the ratio of their moles?

A power company burns approximately $500$tons of coal per day to produce electricity. If the sulphur content of the coal is $1.20 \%$ by weight, how many tons ${\mathrm{SO}}_2$, are dumped into the atmosphere per hour?

If the yield of chloroform obtainable from acetone and bleaching powder is $58\%$. What is the weight of acetone(in gm) required for producing $239$ mg of chloroform?

$2{\mathrm{CH}}_3{\mathrm{COCH}}_3+6{\mathrm{CaOCl}}_2\to \mathrm{Ca}({\mathrm{CH}}_3\mathrm{COO}{)}_2+2{\mathrm{CHCl}}_3+3{\mathrm{CaCl}}_2+2\mathrm{Ca}(\mathrm{OH}{)}_2$

For reaction ${\mathrm{N}}_2\left(\mathrm{g}\right)+3{\mathrm{H}}_2\left(\mathrm{g}\right)\to 2{\mathrm{NH}}_3\left(\mathrm{g}\right)$ $6$ moles of ${\mathrm{H}}_2$ is taken with excess of ${\mathrm{N}}_2$ gas. Mass of ammonia gas produced is:

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 the reaction ${\mathrm{N}}_2+3{\mathrm{H}}_2\iff 2{\mathrm{NH}}_3\left(\mathrm{g}\right) \mathrm{if} 20 \mathrm{g}$ of dinitrogen reacts with $10 \mathrm{g}$ of dihydrogen, what is the mass of ${\mathrm{NH}}_3$ produced? Also what is the limiting reagent?

What weight of ${\mathrm{NaHSO}}_3$ is required to react with $100\mathrm{ml}$of solution containing$0.33\mathrm{g}$ of ${\mathrm{NaIO}}_3$ according to the following reaction

${{\mathrm{IO}}_3}^{\mathrm{\Theta }}+{{\mathrm{HSO}}_3}^{\mathrm{\Theta }} ⟶{\mathrm{I}}^{\mathrm{\Theta }} +{{\mathrm{SO}}_4}^{2-}$

How many grams of ethanol must be treated with sodium at STP to produce $560 \mathrm{mL}$ of dihydrogen gas?

How much quantity of Ammonium Nitrite is required to be heated to obtain $8.4$ gram of Nitrogen.

For complete combustion of $1.12$ litre of butane the produced volume of ${\mathrm{H}}_2\mathrm{O} \mathrm{and} {\mathrm{CO}}_2$ at stp will be

When ${\mathrm{C}}_2{\mathrm{H}}_4$ is burnt in air, carbon dioxide and water are formed. If on combustion of ${\mathrm{C}}_2{\mathrm{H}}_4$, 2 moles of ${\mathrm{CO}}_2$ is produced, calculate the number of drops of water produced, calculate the number of drops of water produced along with this quantity of ${\mathrm{CO}}_2$ if each drop contains $6.022\times {10}^{21}$ water molecules.