Gay Lussac's Law, Avagadro's Law

Q. By how many times an atom of sulphur is heavier than an atom of carbon?

1. $32$ times
2. $12$ times
3. $\frac{8}{3}$ times
4. $\frac{12}{32}$ times

Q. Nitrogen and hydrogen combine in the ratio of 14 : 3 by mass to form ammonia. The mass of nitrogen required to react completely with 9 g of hydrogen is

Q. If we have a pure $N{a}_{2}S{O}_4$ sample that contains a total of 7 billion electrons, then find the number of moles of $N{a}_{2}S{O}_4$ present in the sample.

1. $1.66\times {10}^{-16}$ moles
2. $1.66\times {10}^{-14}$ moles
3. $3.66\times {10}^{-16}$ moles
4. $3.66\times {10}^{-14}$ moles

Q. Question 41
Compute the difference in masses of one mole each of aluminium atoms and one mole of its ions. (Mass of an electron is $9.1\times {10}^{-28}g)$ which one is heavier?

Q. Different samples of water were found to contain hydrogen and oxygen in the ratio of 1 : 8. This shows the law of:

1. Multiple proportions

2. Constant proportions

3. Conservation of mass

4. Reciprocal proportions

Q. Find the total number of moles of electrons in $6.023\times {10}^{23}N{O}_3^{-}$ ions ?

1. $32$
2. $31$
3. $30$
4. $28$

Q. Calculate the number of molecules of sulphur $\left(S_8\right)$ present in 16 g of solid sulphur. [2 marks]

Q. $10d{m}^3$ of $N_2$ gas and $10d{m}^3$ of gas X at the same temperature contain the same number of molecules.
The gas X is

1. $C{O}_2$
2. $H_2$
3. $CO$
4. $NO$

Q. $1.375$ g of cupric oxide was reduced by heating in a current of hydrogen and the weight of copper obtained was $1.098$ g. In another experiment, $1.179$ g of copper was dissolved in nitric acid and the resulting solution was evaporated to dryness. The residue of copper nitrate when strongly heated was converted into $1.4476$ g of cupric oxide. The result of this process show :

1. law of reciprocal proportion
2. law of multiple proportion
3. law of constant proportion
4. none of these

Q. When 3.0 g of carbon is burnt in 8.00 g oxygen, 11.00 g of carbon dioxide is produced.

1. What mass of carbon dioxide will be formed when 3.00 g of carbon is burnt in 50.00 g of oxygen?
2. Which law of chemical combinations will govern your answer?

Q. Find the total number of moles of electrons in $6.023\times {10}^{23}N{O}_3^{-}$ ions.

1. 32
2. 31
3. 28
4. 30

Q. Calculate the number of moles of magnesium present in a magnesium​ ribbon weighing 12 g. Molar atomic mass of magnesium is 24 g mol${}^{-1}$.​

Q. Four identical flask are filled with hydrogen, oxygen, carbon dioxide and chlorine at the same temperature and pressure. The flask with the greatest mass will be the one containing :

1. Hydrogen
2. Oxygen
3. Carbon dioxide
4. Chlorine

Q. Nitrogen reacts with oxygen to form nitrogen (III) oxide. What will be the volume ratio of the reactants and products of the given reaction?

1. 2 : 3 : 2
2. 2 : 3 : 4
3. 1 : 3 : 2
4. 2 : 1 : 2

Q. Ratio of $C_p$ and $C_v$ of a gas '$X$' is $1.4$. The number of atoms of the gas '$X$' present in $11.2$ litres of it at N.T.P. is:

1. $2.01\times {10}^{23}$
2. $6.02\times {10}^{23}$
3. $3.01\times {10}^{23}$
4. $1.2\times {10}^{24}$

Q. Balance the given equation and then write down the answer for the questions given below.
$C{H}_4+O_2\to C{O}_2+H_{2}O$
Based on the equation above, How many moles of $C{O}_2$ is formed when $10$ moles of Ethane is burned in air ?

Q. Identify the correct increasing order of molecular masses.

1. ${\mathrm{CO}}_2<\mathrm{CaO\; <}\mathrm{CO\; <}{\mathrm{CaCO}}_3$
2. $\mathrm{CO\; <}{\mathrm{CO}}_2<\mathrm{CaO\; <}{\mathrm{CaCO}}_3$
3. ${\mathrm{CaCO}}_3<\mathrm{CaO\; <}{\mathrm{CO}}_2<\mathrm{CO}$
4. ${\mathrm{CO}}_2<\mathrm{CaO\; <}{\mathrm{CaCO}}_3<\mathrm{CO}$