Laws of Chemical Combination

The molecular weight of ${\text{O}}_2$ and ${\text{S}\text{O}}_2$  are $32$ and $64$ respectively. At $15^o\text{C}$ and $150$ mm of Hg pressure, one litre of ${\text{O}}_2$ contains ‘N’ molecules. The number of molecules in two litres of ${\text{S}\text{O}}_2$ under the same conditions of temperature and pressure will be :

The law of definite proportions states that a given chemical compound always contains the same elements in the exact same proportion by mass.

The individual elements that constitute a chemical compound are always present in a _____.

What are the significance of the law of definite proportion?

There are five laws of chemical combinations.

A balanced chemical reaction follows law of conservation of _____

Law of conservation of energy states that mass can neither be created nor destroyed.

Law of conservation of mass is useful for a number of calculations and can be used to solve for unknown masses.

What is the significance of law of conservation of mass?

When $10 \mathrm{mL}$ of propane (gas) is combusted completely, the volume of ${\mathrm{CO}}_2\left(\mathrm{g}\right)$ obtained in similar condition is:

${\mathrm{H}}_2\mathrm{S}$ contains $94.11\%$ sulphur; ${\mathrm{SO}}_2$ contains 50% oxygen and ${\mathrm{H}}_2\mathrm{O}$ contains $11.11\%$ hydrogen. Thus, 

The volume of one mole of a gas is called _____ .

Potassium chloride contains $52\%$ of $\mathrm{K}$, potassium iodide contains $23.6\%$ of $\mathrm{K}$ and iodine monochloride contains $77.8\%$ of $\mathrm{I}$.  The given information illustrates which of the followin laws?

Given $3\mathrm{g}$ of carbon reacts with $1\mathrm{g}$ of hydrogen to form ${\mathrm{CH}}_4$ and $8\mathrm{g}$ of oxygen reacts with $1\mathrm{g}$ of hydrogen to form ${\mathrm{H}}_2\mathrm{O}$. Similarly, $12\mathrm{g}$ of carbon reacts with $32\mathrm{g}$ of oxygen to form carbon dioxide. In both cases the ration of carbon and oxygen is 3 : 8. Which of the following laws illustrate the given example?

Which of the following compounds verify Law of Reciprocal Proportions?

Two oxides of metal contain $36.4 \mathrm{and} 53.4$ percent of oxygen by mass respectively. If the formula of the first oxide is ${\mathrm{M}}_2\mathrm{O}$, then that of the second oxide is 

$100 \mathrm{g}$ of ethylene polymerizes to polythene according to the equation:
$\mathrm{n} {\mathrm{CH}}_2={\mathrm{CH}}_2\to {\left({\mathrm{CH}}_2-{\mathrm{CH}}_2\right)}_{\mathrm{n}}$
The mass of polythene produced will be

Two oxides of metal contain $36.4 \mathrm{and} 53.4$ percent of oxygen by mass respectively. If the formula of the first oxide is ${\mathrm{M}}_2\mathrm{O}$, then that of the second is

$20.8 \mathrm{g}$ of $\mathrm{B}\mathrm{a}\mathrm{C}{\mathrm{l}}_2$ on reaction with $9.8 \mathrm{g}$ of ${\mathrm{H}}_2\mathrm{S}{\mathrm{O}}_4$ produces $7.3 \mathrm{g}$ of $\mathrm{H}\mathrm{C}\mathrm{l}$ and some amount of $\mathrm{B}\mathrm{a}\mathrm{S}{\mathrm{O}}_4$. The amount in grams of $\mathrm{B}\mathrm{a}\mathrm{S}{\mathrm{O}}_4$ formed is

A gaseous compound having carbon, hydrogen and oxygen was burnt in the presence of oxygen. After combustion, $1$ volume of the gaseous compound produces$2$ volumes of ${\mathrm{CO}}_2$ and$2$volumes of steam. Determine the molecular formula of the compound, if all the volumes were measured under the same conditions of pressure and temperature.