# Gay Lussac's Law, Avagadro's Law

## Trending Questions

**Q.**The volume of a drop of water is 0.05 mL and the density of water is 1.0 g/mL. How many water molecules are present in a drop of water?

- 1.7×1021
- 5.4×1023
- 2.2×1026
- 1.71×1020

**Q.**

Which of the following has the smallest number of molecules?

$22\mathrm{g}$ of ${\mathrm{CO}}_{2}$ gas

$11.2\mathrm{L}$ of ${\mathrm{CO}}_{2}$ gas

$22.4\times {10}^{3}\mathrm{mL}$ of ${\mathrm{CO}}_{2}$ gas

$0.1\mathrm{mole}$ of ${\mathrm{CO}}_{2}$ gas

**Q.**

How do you calculate the number of moles from volume?

**Q.**

One liter of ${\mathrm{CO}}_{2}$ is passed through red hot coke. The volume becomes 1.4 litres at same temperature and pressure. The composition of the products is ____.

**Q.**

Calculate the number of molecules in $4\mathrm{g}$ of oxygen.

**Q.**The density of air is 0.001293 g/cm3 at STP. Which of the following statements is/are correct?

- Vapour density is 14.48
- Molecular weight is 28.96 amu
- Vapour density is 0.001293
- Vapour density and molecular weight cannot be determined

**Q.**

Hydrogen gas is prepared in the laboratory by reacting dilute$\mathrm{HCl}$ with granulated zinc. The following reaction takes place: $\mathrm{Zn}+2\mathrm{HCl}\to {\mathrm{ZnCl}}_{2}+{\mathrm{H}}_{2}$ Calculate the volume of hydrogen gas is liberated at STP when $32.65\mathrm{g}$of Zinc reacts with$\mathrm{HCl}$ . 1 mole of a gas occupies $22.7\mathrm{L}$ volume at STP; atomic mass of $\mathrm{Zn}=65.3\mathrm{u}?$

$10.03\mathrm{L}$

$11.35\mathrm{L}$

$11.57\mathrm{L}$

$9.53\mathrm{L}$

**Q.**

Compute the number of ions present in 5.85 g of sodium chloride.

**Q.**

The number of Carbon atoms in 1g of CaCO_{3 }is:

6.02×10

^{23}6.02×10

^{21}3.0125×10

^{22}1.204×10

^{23}

**Q.**

What is the definition of a perfect gas?

**Q.**

The number of atoms present in $1.6\text{g}$ of methane is

$6.02\times {10}^{23}$

$3.01\times {10}^{24}$

$3.01\times {10}^{23}$

$6.02\times {10}^{24}$

**Q.**

$108\mathrm{g}$ silver (molar mass $108\mathrm{g}{\mathrm{mol}}^{-1}$) is deposited at cathode from ${\mathrm{AgNO}}_{3}\left(\mathrm{aq}\right)$solution by a certain quantity of electricity. The volume (in $\mathrm{L}$) of oxygen gas produced at $273\mathrm{K}$ and $1\mathrm{bar}$ pressure from water by the same quantity of electricity is:

**Q.**

Illustrate the law of definite proportions from the following data:-1)0.32g of sulphur on burning in air produced 224ml of SO2 at N.T.P

**Q.**

45.4 L of dinitrogen reacted with 22.7 L of dioxygen and 45.4 L of nitrous oxide was formed. The reaction is given below

2N2(g)+ O2(g)→2N2O (g)

Which law is being obeyed in this experiment? write the statement of the law?

**Q.**The ratio of volumes occupied by 1 mole of O2 and 1 mole CO2 under identical conditions of temperature and pressure is

- 1:2
- 1:3
- 1:1
- 2:1

**Q.**5.6 litres of a gas at NTP is found to have a mass of 11 g.

The molecular mass of the gas is:

- 44 g
- 36 g
- 11.4 g
- 16 g

**Q.**

A gas of mass 32 gms has a volume of 20 litres at S.T.P .Calculate the gram molecular weight of the gas.

**Q.**A sample of water gas has a composition by volume of 50% H2, 45% CO and 5% CO2. Calculate the volume in litres at STP at which the water gas on treatment with excess of steam will produce 5 L of H2. The equation for the reaction is: CO+H2O→CO2+H2

- 5.26 L
- 2.33 L
- 5.00 L
- 7.20 L

**Q.**

A sample of Vitamin C is known to contain $2.58\times {10}^{24}$ oxygen atoms. How many moles of oxygen atoms are present in the sample?

**Q.**Which of the following represents Avogadro’s hypothesis?

- Gases react together in volumes which bear a simple ratio to one another.
- Equal volumes of all gases under the same conditions of temperature and pressure contain an equal number of molecules.
- Atoms of different elements may combine with each other in a fixed, simple, whole number ratio to form compounds.
- Equal volumes of all gases under the same temperature and pressure conditions contain an equal number of atoms.

**Q.**

Calculate the number of particles in $0.1\mathrm{mol}$ of carbon atoms.

**Q.**The density of potassium bromide crystal is 2.75 g cm−3 and the length of a unit cell is 654 pm. What will be the crystal lattice of KBr?

Molar mass of KBr=119 g mol−1

- Face centred cubic
- Body centred cubic
- Simple cubic
- Edge centred cubdic

**Q.**

ammonia contains 82.35% of nitrogen and 17.65% of hydrogen , water contains 88.90% of oxygen and 11.10% of Hydrogen. Nitrogen trioxide contains 63.15% of oxygen and 36.85% of nitrogen. Show that this data illustrate the law of Reciprocal proportion.

**Q.**

Define a molecule. How many molecules are present in

(a) 9 gram of water

(b) 17 gram of ammonia

**Q.**

What is the SI unit used to measure the amount of substance?

**Q.**The density of a unit cell in (g/cm3) can be represented as :

Here,

a is the edge length in pm

Zeff is the effective number of particles in a unit cell

M is the molar mass NA is the avogadro number

- MNA×a3×10−30×Zeff
- Zeff×MNA×a3×10−30
- NA×a3×10−30Zeff×M
- NA×a3×10−30×ZeffM

**Q.**{ The vapour pressure of }n -hexane at }350K is }840 torr }}{ and that of cyclohexane is }600 torr. Mole fraction of }}{ hexane in the mixture that boils at }350K and }1 atm }} pressure assuming ideal behaviour is

**Q.**An element exists in bcc lattice with a cell edge of 300 pm. Calculate the molar mass if density of the unit cell is 7g//cm3.

Take NA=6×1023

- 56.7 g mol−1
- 5.67 g mol−1
- 113.4 g mol−1
- 11.34 g mol−1

**Q.**11.2 L of CH4 and 22.4 L of C2H6 at STP are mixed. Then the correct statement(s) is/are:

- Vapour density of the mixture is 12.67
- Average molecular weight will be less than 16
- Average molecular weight will be greater than 16 and less than 30
- Average molecular weight will be greater than 30

**Q.**If you are given Avogadro's number of atoms of a gas 'X'. If half of the atoms are converted into X+(g) by energy ΔH. The IE of X is

- 2ΔHNA
- 2NAΔH
- ΔH2NA
- NAΔH