Calculate the standard entropy change (J/mol-K).?

Question

For the reaction whose reactants and products are:



reactants: H2S (g) O2 (g)


products: H2O (g) SO2 (g)



1. calculate the standard entropy change (J/mol-K).

2. Calculate ΔSuniv in J/mol-K for the above process at 298.15 K.



The answer depends on how you balance the equation. For this question balance the equation using the smallest ratio of WHOLE numbers.

Answer 1

OK - so we need to write the balanced equation first.

Try: 2H2S + 3O2 ----> 2H2O + 2SO2

So now you need to look up the entropies of formation of the four substances, multiply them by the correct number of moles, and then subtract reactants from products.

Answer 2

the balanced equation is 2C + 2H2O -> CH3COOH and for calculating the enthalpy substitute you will possibly be able to desire to the two the entropy substitute or the enthalpy of formation of things and enthalpy of dissociation of reactants. whilst you're given entropy substitute this is S then you certainly can use the formula S=H/T T= TEMPERATURE IN KELVIN H= ENTHALPY substitute S=ENTROPY substitute whilst you're given enthalpy of formation of things and enthalpy of dissociation of reactants then you certainly will use the formula H(entire)= H(products) - H(reactants) and whilst you're given the GIBBS unfastened power substitute (G) then you certainly will use G = H - TS G= power substitute ( this is 0 for components) gadgets of the suggested parameters:- H= Joules in line with mole (J/mol) S=Joules in line with kelvin in line with mole (J/ok mol) T= kelvin (ok) G=Joules in line with mole (J/mol)