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Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
ISBN: 9781305079243

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Section
BuyFindarrow_forward

Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
ISBN: 9781305079243
Textbook Problem

The total volume of hydrogen gas needed to fill the Hindenburg was 2.0 × 108 L at 1.0 atm and 25°C. Given that Δ H f for H2O(l) is −286 kJ/mol, how much heat was evolved when the Hindenburg exploded, assuming all of the hydrogen reacted to form water?

Interpretation Introduction

Interpretation: From the given data, amount of heat evolved or molar heat of fusion should be determined.

Concept introduction:

  • By combining the three gaseous laws namely Boyle’s law, Charles’s law and Avogadro’s law a combined gaseous equation is obtained. This combined gaseous equation is called Ideal gas law.

According to ideal gas law,

PV=nRT

Where,

P = pressure in atmospheres

V= volumes in liters

n = number of moles

R =universal gas constant ( 0.08206L×atm/K×mol )

T = temperature in kelvins

By knowing any three of these properties, the state of a gas can be simply identified,

Number of moles of the gas can be determined by,

n=PVRT

  • Molar heat of fusion can be calculated as follows.

    Heatreleased(kJ)=Numberofmole(n)×molarenthalpyoffusion

Explanation

Explanation

To determine: the number of moles of hydrogen

Number of mole (n) =8.2×106molH2

According to ideal gas equation,

PV=nRT

Number of moles of the gas can be determined by,

n=PVRT

Here,thegivendata'sare,P=1.0atmV=2.0×108LR=0.08206LatmKmolT=25°C=298KSince,K=(°C+273)K=(25°C+273)K=298 KByaddingthegivenvaluestotheaboveequation,nH2=1.0atm×2.0×108L0

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