Calculate the mass and volume of oxygen at S.T.P., which will be evolved on electrolysis of 1 mole (18g) of water

36 g of water produces 32 g of O 2 18 g of water will produced = x 18 = 16 g of O 2 2 moles of water produces 1 mole of oxygen 1 mole of water will produce = 0.5 moles of O 2 1 mole of O 2 occupies 22.4 L volume 0.5 moles will occupy = 22.4 × 0.5 = 11.2 L

Find the mass of KNO₃ required to produce 126 kg of nitric acid. Find whether a larger or smaller mass of NaNO₃ is required for the same purpose.
KNO₃ + H₂SO₄ ⟶ KHSO₄ + HNO₃
NaNO₃ + H₂SO₄ ⟶ NaHSO₄ + HNO₃

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Pure calcium carbonate and dilute hydrochloric acid are reacted and 2 litres of carbon dioxide was collected at 27°C and normal pressure.
CaCO₃ + 2HCl ⟶ CaCl₂ + H₂O + CO₂
Calculate:
(a) The mass of salt required.
(b) The mass of the acid required

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1.56 g of sodium peroxide reacts with water according to the following equation:
2Na₂O₂ + 2H₂O ⟶ 4NaOH + O₂
Calculate:
(a) mass of sodium hydroxide formed,
(b) volume of oxygen liberated at S.T.P.
(c) mass of oxygen liberated.

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(a) Calculate the mass of ammonia that can be obtained from 21.4 g of NH₄Cl by the reaction:
2NH₄Cl + Ca(OH)₂ ⟶ CaCl₂ +2H₂O + 2NH₃
(b) What will be the volume of ammonia when measured at S.T.P?

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Chemistry

Calculate the mass and volume of oxygen at S.T.P., which will be evolved on electrolysis of 1 mole (18g) of water

Mole Concept

Related Questions

Find the mass of KNO₃ required to produce 126 kg of nitric acid. Find whether a larger or smaller mass of NaNO₃ is required for the same purpose.
KNO₃ + H₂SO₄ ⟶ KHSO₄ + HNO₃
NaNO₃ + H₂SO₄ ⟶ NaHSO₄ + HNO₃

Pure calcium carbonate and dilute hydrochloric acid are reacted and 2 litres of carbon dioxide was collected at 27°C and normal pressure.
CaCO₃ + 2HCl ⟶ CaCl₂ + H₂O + CO₂
Calculate:
(a) The mass of salt required.
(b) The mass of the acid required

1.56 g of sodium peroxide reacts with water according to the following equation:
2Na₂O₂ + 2H₂O ⟶ 4NaOH + O₂
Calculate:
(a) mass of sodium hydroxide formed,
(b) volume of oxygen liberated at S.T.P.
(c) mass of oxygen liberated.

(a) Calculate the mass of ammonia that can be obtained from 21.4 g of NH₄Cl by the reaction:
2NH₄Cl + Ca(OH)₂ ⟶ CaCl₂ +2H₂O + 2NH₃
(b) What will be the volume of ammonia when measured at S.T.P?

Chemistry

Calculate the mass and volume of oxygen at S.T.P., which will be evolved on electrolysis of 1 mole (18g) of water

Mole Concept

Related Questions

Find the mass of KNO3 required to produce 126 kg of nitric acid. Find whether a larger or smaller mass of NaNO3 is required for the same purpose.KNO3 + H2SO4 ⟶ KHSO4 + HNO3NaNO3 + H2SO4 ⟶ NaHSO4 + HNO3

Pure calcium carbonate and dilute hydrochloric acid are reacted and 2 litres of carbon dioxide was collected at 27°C and normal pressure.CaCO3 + 2HCl ⟶ CaCl2 + H2O + CO2Calculate:(a) The mass of salt required.(b) The mass of the acid required

1.56 g of sodium peroxide reacts with water according to the following equation:2Na2O2 + 2H2O ⟶ 4NaOH + O2Calculate:(a) mass of sodium hydroxide formed,(b) volume of oxygen liberated at S.T.P.(c) mass of oxygen liberated.

(a) Calculate the mass of ammonia that can be obtained from 21.4 g of NH4Cl by the reaction:2NH4Cl + Ca(OH)2 ⟶ CaCl2 +2H2O + 2NH3(b) What will be the volume of ammonia when measured at S.T.P?

Find the mass of KNO₃ required to produce 126 kg of nitric acid. Find whether a larger or smaller mass of NaNO₃ is required for the same purpose.
KNO₃ + H₂SO₄ ⟶ KHSO₄ + HNO₃
NaNO₃ + H₂SO₄ ⟶ NaHSO₄ + HNO₃

Pure calcium carbonate and dilute hydrochloric acid are reacted and 2 litres of carbon dioxide was collected at 27°C and normal pressure.
CaCO₃ + 2HCl ⟶ CaCl₂ + H₂O + CO₂
Calculate:
(a) The mass of salt required.
(b) The mass of the acid required

1.56 g of sodium peroxide reacts with water according to the following equation:
2Na₂O₂ + 2H₂O ⟶ 4NaOH + O₂
Calculate:
(a) mass of sodium hydroxide formed,
(b) volume of oxygen liberated at S.T.P.
(c) mass of oxygen liberated.

(a) Calculate the mass of ammonia that can be obtained from 21.4 g of NH₄Cl by the reaction:
2NH₄Cl + Ca(OH)₂ ⟶ CaCl₂ +2H₂O + 2NH₃
(b) What will be the volume of ammonia when measured at S.T.P?