Chemistry for Engineering Students

4th Edition
Lawrence S. Brown + 1 other
ISBN: 9781337398909



Chemistry for Engineering Students

4th Edition
Lawrence S. Brown + 1 other
ISBN: 9781337398909
Textbook Problem

9.98 Hydrogen combines with oxygen in fuel cells according to the thermochemical equation

   2H 2 ( g ) + O 2 ( g ) 2H 2 O ( g )

Δ H ° = -571.7 kJ

Suppose that you are working with a firm that is using hydrogen fuel cells to power satellites. The satellite requires 4 .0 × 1 0 5 kJ of energy during its useful lifetime to stabilize its orbit. Describe how you would determine the mass of hydrogen you would need in your fuel cells for this particular satellite.

Interpretation Introduction


The mass of hydrogen to be used in the fuel cell in order to power the satellite should be calculated.

Concept introduction:

  • Thermochemical equations depict the enthalpy change (ΔH)of a chemical reaction in terms of the reaction stoichiometry.
  • Chemical reactions proceed with the absorption (endothermic) or evolution (exothermic) of heat.
  • Enthalpy change is negative for an exothermic reaction and positive for an endothermic reaction.

Given: Thermochemical equation: 2H2(g)+O2(g) 2H2O(g)

Enthalpy change (ΔH) = -571.7 kJ

Energy required by the satellite = 4.0×105 kJ


Step I: Calculate the number for moles of hydrogen required for the given satellite energy

As per the stoichiometry of the thermochemical equation:

571.7 kJ of energy is released by 2 moles of H2

Moles of H2 required for to produce an energy of 4

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