The reduction of stannous sulphide by hydrogen takes place as follows: SnS(s) + H2(g) 2 Sn(1) + H2S(g) The equilibrium constant (K) values was determined after studying the reaction over the temperature range 533 to 679°C. The following data was recorded: T/°C K (x 104) 533 10.6 582 16.1 631 27.6 679 46.2 Use the data to determine the enthalpy change (kJ mol-1) for the reaction.

The reduction of stannous sulphide by hydrogen takes place as follows: SnS(s) + H2(g) 2 Sn(1) + H2S(g) The equilibrium constant (K) values was determined after studying the reaction over the temperature range 533 to 679°C. The following data was recorded: T/°C K (x 104) 533 10.6 582 16.1 631 27.6 679 46.2 Use the data to determine the enthalpy change (kJ mol-1) for the reaction.

Chemistry by OpenStax (2015-05-04)

1st Edition

ISBN:9781938168390

Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Chapter16: Thermodynamics

Section: Chapter Questions

Problem 52E: Benzene can be prepared from acetylene. 3C2H2(g)C6H6(g). Determine the equilibrium constant at 25 C...

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