Explanation Given: Volume of O 2 , V O 2 = 1 .4 L Temperature, T = 315 K Pressure of O 2 , P O 2 = 0 .957 atm Explanation: To determine the mass of H 2 O , moles of H 2 O are required that can be obtained on applying the stoichiometry of the given reaction. For this, the number of moles of O 2 is calculated. Use ideal law of gas to calculate the number of moles of O 2 : P O 2 V O 2 = n O 2 R T ⇒ n O 2 = P O 2 V O 2 T Substitute P O 2 = 0.957 atm , V O 2 = 1.4 L , R = 0.08206 L . atm/mol/K , and T = 315 K in the above expression to get n O 2 = 0 .957 atm × 1 .4 L 0 .08206 L . atm mol . K ×315 K = 0 .052770 mol Therefore, the number of moles of O 2 is 0.052770 mol . The given reaction is 2 H 2 O ( l ) → 2 H 2 ( g ) + O 2 ( g ) As per the above reaction 1 mol oxygen O 2 is formed from = 2 mol H 2 O ∴ 0 .052770 mol oxygen O 2 is formed from = 2 mol H 2 O × 0

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Chapter 5, Problem 72E

Interpretation Introduction

To determine: Mass of water H2O required for the formation of oxygen at a temperature of 315 K and a pressure of 0.957 atm.

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Chapter 5, Problem 71E

Chapter 5, Problem 73E

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