The reduction of stannous sulphide by hydrogen takes place as follows: SnS(s) + H2(g) 2 Sn(1)...

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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.

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DATE Solution Reduction Realtion of stanour sulphid... View the full answer