   Chapter 10, Problem 32PS

Chapter
Section
Textbook Problem

Silane, SiH4, reacts with O2 to give silicon dioxide and water:SiH4(g) + 2 O2(g) → SiO2(s) + 2 H2O(ℓ)A 5.20-L sample of SiH4 gas at 356 mm Hg pressure and 25 °C is allowed to react with O2 gas. What volume of O2 gas, in liters, is required for complete reaction if the oxygen has a pressure of 425 mm Hg at 25 °C?

Interpretation Introduction

Interpretation:

The volume of O2 gas required for completing the given reaction if the oxygen has a pressure of 425mmHgat25°C has to be determined.

Concept Introduction:

According to ideal gas equation:

PV=nRT

Numberofmoles=massmolarmass

Explanation

The volume of oxygen gas required to complete the given reaction of silane with oxygen

SiH4+2O2SiO2+2H2O

Given that silane react with oxygen in following conditions.

Pressure=356mmHg=0.4684atmVolume=5.2LTemperature=25°C=298K

According to ideal gas equation:

PV=nRT

n=PVRT=0.4684atm×5.2L0.08205L.atm/K.mol×298K=0.099molSiH4

Now we have to calculate the number of moles of oxygen required to complete the given reaction.

From the balanced equation, for one mole of silane, two moles of oxygen is required to complete the reaction

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