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

(a) 156 g of sodium peroxide produces 160 g of sodium hydroxide 1.56 g of sodium peroxide will produce x 1.56 = 1.6 g of sodium hydroxide (b) 156 g of sodium peroxide produces 22.4 L of oxygen 1.56 g of sodium peroxide will produce x 1.56 = 0.224 L Converting L to cm 3 As 1 L = 1000 cm 3 So, 0.224 L = 224 cm 3 (c) 156 g of sodium peroxide produces 32 g of oxygen 1.56 g of sodium peroxide will produce x 1.56 = 0.32 g

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Chemistry

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.

Mole Concept

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Chemistry

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.

Mole Concept

Related Questions

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CaCO₃ + 2HCl ⟶ CaCl₂ + H₂O + CO₂
Calculate:
(a) The mass of salt required.
(b) The mass of the acid required

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

(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?

Aluminium carbide reacts with water according to the following equation.
Al₄C₃ + 12H₂O ⟶ 3CH₄ + 4Al(OH)₃
(a) What mass of aluminium hydroxide is formed from 12g of aluminium carbide?
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Chemistry

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.

Mole Concept

Related Questions

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

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

(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?

Aluminium carbide reacts with water according to the following equation.Al4C3 + 12H2O ⟶ 3CH4 + 4Al(OH)3(a) What mass of aluminium hydroxide is formed from 12g of aluminium carbide?(b) What volume of methane is obtained from 12g of aluminium carbide?

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.

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

(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?

Aluminium carbide reacts with water according to the following equation.
Al₄C₃ + 12H₂O ⟶ 3CH₄ + 4Al(OH)₃
(a) What mass of aluminium hydroxide is formed from 12g of aluminium carbide?
(b) What volume of methane is obtained from 12g of aluminium carbide?