- #1

- 6

- 0

## Main Question or Discussion Point

The question asks to solve for delta S surroundings at 298K when 2.49 moles of H2S (g) react.

reaction:

2H2S (g) + 3O2 (g)= 2H2O (g) + 2SO2 (g)

My problem is that I don't know how to calculate delta S surroundings. So to solve the problem I'm making the assumption that -Delta S surroundings = Delta S system and using products minus reactants to find Delta S system.

Attempt:

I begin by finding tabulated S values for all compounds in rxn. Then multiply and cancel units to find out how many moles of each will be in the reaction. Then Using products minus reactants with accurate mol coefficients calculate delta S of rxn. I get this to be -210.4 J/K. Then assuming that Delta S surroundings = -Delta S run I get that Delta S surroundings equals 210.4 J/K.

If anyone could point me in the right direction that would be great. Thanks in advance

reaction:

2H2S (g) + 3O2 (g)= 2H2O (g) + 2SO2 (g)

My problem is that I don't know how to calculate delta S surroundings. So to solve the problem I'm making the assumption that -Delta S surroundings = Delta S system and using products minus reactants to find Delta S system.

Attempt:

I begin by finding tabulated S values for all compounds in rxn. Then multiply and cancel units to find out how many moles of each will be in the reaction. Then Using products minus reactants with accurate mol coefficients calculate delta S of rxn. I get this to be -210.4 J/K. Then assuming that Delta S surroundings = -Delta S run I get that Delta S surroundings equals 210.4 J/K.

If anyone could point me in the right direction that would be great. Thanks in advance