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

For the reaction whose reactants and products are:











reactants: C (graphite) H2O (l)








products: CH3COOH(l)











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





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





Enter a numeric answer only

Calculate the standard entropy change (J/mol-K).?
Lancenigo di Villorba (TV), Italy





+2,03 CAL / (K * MOL) = +8.5 J / (MOL * K)





I started from the reaction





2 C(graphite) + 2 H2O(l) ---%26gt; CH3COOH(l)





thus I wrote





DeltaS = 38.19 - 2 * (1.36 + 16.72) = 2.03 cal /(K*mol)





As I think the experiment runs in a Mahler's bomb, I assume the adiabatic nature of it, so I write :





(DeltaS)system = (DeltaS)universe





I hope this helps you.
Reply:the balanced equation is


2C + 2H2O -%26gt; CH3COOH





and for calculating the enthalpy change you need to either the entropy change or the enthalpy of formation of products and enthalpy of dissociation of reactants.





if you are given entropy change that is S then you can use the formula S=H/T


T= TEMPERATURE IN KELVIN


H= ENTHALPY CHANGE


S=ENTROPY CHANGE





if you are given enthalpy of formation of products and enthalpy of dissociation of reactants then you will use the formula


H(total)= H(products) - H(reactants)





and if you are given the GIBBS FREE ENERGY CHANGE (G) then you will use


G = H - TS


G= energy change ( it is zero for elements)





Units of the mentioned parameters:-





H= Joules per mole (J/mol)


S=Joules per kelvin per mole (J/K mol)


T= kelvin (K)


G=Joules per mole (J/mol)