ICSE Worksheet for chapter-5 Mole Concept & Stoichimetry class 10

Worksheet For class 10

This page is prepared by the Academic team of Physics Wallah which consists of ICSE Board Worksheet for Class 10 Chemistry. Students of Class 10 Chemistry can get a free Worksheet for Class 10 Chemistry in PDF format prepared as per the newest syllabus and examination pattern in your schools.

Standard 10 students can practice questions and answers which are given here for Chemistry in Grade 10 that will help them to improve their knowledge of all important chapters and their topics. Students can also download free pdf of Class 10 Chemistry Notes prepared by teachers and solve important problems provided here with solutions on daily basis to get more scores in school exams and tests.

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  1. Gas laws, Gay-Lussac’s law.
  2. Avogadro’s law and its application.
  3. Relative atomic/molecular weight, mole, Avogadro’s number.
  4. Vapour density and molecular weight.
  5. Percentage composition, empirical formula, molecular formula.
  6. Calculations based on chemical equation.

Section - 1 

Q1. What is atomicity? Give the examples of diatomic gases?

Q2. What do you understand by g-mole of a gas?

Q3. What is Absolute Zero?

Q4.What do you understand by the ‘Standard Molar Volume’? Calculate the volume occupied by 3.4g of ammonia at S.T.P.?

Section - 2

Q5. Calculate the atomicity of oxygen molecule from the following information: Vapour Density of Oxygen=16

  • Relative Atomic mass of Oxygen=16
  • Show all the calculations.

Q6. What is the mass of Nitrogen in 1000kg of Urea [CO(NH2)2] ?

(Answer correct to the nearest kg) [H=1 , C=12, N=14, O=16]

Q7. Find the total percentage of oxygen in Mg(NO3)2.6H2O.

Q8. Solid ammonium dichromate (relative molecular mass= 252) on heating decompose as follows:

(NH4)2Cr2O7 N2+ Cr2O3 + 4H2O

  • Calculate the volume of nitrogen at S.T.P., that will be evolved when 31.5g of ammonium dichromate is heated and
  • The mass of chromium (III) oxide formed at the same time.

(H= 1; N= 14; O= 16; C= 52)

Q9.Determine the empirical formula of a compound containing 47.9% potassium, 5.5% beryllium and 46.6% fluorine by mass.

(Atomic weight of Be= 9; F= 19; K= 39) Work to one decimal place.

Q10. Water can be splitted into hydrogen and oxygen under suitable conditions. The equation representing the change is2H2 O→2H2+O2:

  • If 2000 cm3 of hydrogen is produced, what volume of oxygen is liberated at the same time under the same condition of temperature and pressure?
  • Calculate the number of molecules in 1 kg of sodium hydroxide.

(Na=23, O=16,H=1)

  • A gas cylinder can hold 1 kg of hydrogen under the same conditions of temperature and pressure.
  • Find the weight of sulphur dioxide it can hold.
  • If the number of molecules of hydrogen is ‘y’ find the number of molecules of sulphur dioxide present in the cylinder.(S=32, O=16).

Q11. How many grams of sulphuric acid will be required to completely neutralize 16.0 gm of caustic soda? What volume of H2 be evolved at S.T.P.?

Q12. State Avogadro’s law

  • State four applications of Avogadro’s Law
  • Calculate the number of molecules in 1 kg of sodium hydroxide.

[Na=23, O= 16, H=1]

Q13. Why are gases at different temperature and pressure reduced to STP?

  • Calculate the number of molecules in
  • 11.2 litres of CO2 at STP.
  • 22.4 lirtes of oxygen at STP.
  • Formula of urea is CON2H. Calculate the percentage of nitrogen in urea.

[C=12, O=16, H=1, N=14]

Q14. Calcuate the molecular mass of a gas, 5.6 litres of which at STP weighs 8 gm. If the gas is an element with atomic mass 16, what is its atomicity?

Calculate the percentage weight of nitrogen in [K4FE(CN)6].

[K=39, Fe=65, C=12, N=14]

A gas when filled in a vessel weighs 2.5 gm. When hydrogen is filled in the same vessel it weighs 0.30 gm at the same temperature and pressure. Calculate the molecular weight of the gas.

Q15. State Gay-Lussac’s law of gaseous volumes.

When carbon dioxide is passed over red hot carbon, carbon monoxide is produced according to the equation CO2+C→2CO:

60 cm3 of oxygen was added to 24 cm3 of carbon monoxide and the mixture ignited, calculate:

  • The volume of oxygen used up, and
  • The volume of carbon dioxide formed.

Q16. Express Kelvin zero in degree centigrade.

  • A compound of sodium, sulphur and oxygen has the following percentage composition: Na=29.1%, S=40.5% and O=30.4%. Find its empirical formula.
  • Hydrogen and oxygen combine to form water according to the following equation 2H2+O2→2H2 O:

A mixture of 22.4 litres of hydrogen and 22.4 lirtes of oxygen at 100oC is ignited. Calculate the volume of stem produced.

Q17. Ammonia is oxidized according to the equation:

4NH3+SO2→4NO+6H2 O

How many litres of nitric oxide are formed when 90 litres of oxygen react with ammonia at STP?

Calculate the mass of chromium atoms in 0.5 kg of cr2S3 [Cr=52, S=32]

Q18. If the densities of hydrogen and a gas X are 0.09 litre and 1.35 per litre respectively, calculate

  • The vapour density of X,
  • The molecular weight of X

The equation for the complete combustion of butane is

2C4 H10+13O2→8CO2+10H2 O

[C=12, H=1, O=16, molar volume of a gas at STP is 22.4 litre (or 22.4 dm3)]

  • How many moles of oxygen would be needed for the complete combustion of 58 gm of butane?
  • What volume of carbon dioxide would be formed at STP?

The mass of 5.6 litres of certain fas at STP is 12 gm. What is the relative molecular mass or molar mass of the gas?

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