Calculate the standard entropy, Delta S degree_rxn, of the following reaction at

Question

Calculate the standard entropy, Delta S degree_rxn, of the following reaction at 25.0 degree C using the data in this table. The standard enthalpy of the reaction, Delta H degree_rxn is = 633.1 kJ middot mol^-1. 3C_2 H_2(g) rightarrow C_6H_6(l) Delta S degree_rxn = J middot K^-1 middot mol^-1 Then, calculate the standard Gibbs free energy of the reaction, Delta G degree_rxn. Delta G degree_rxn = kJ midodt mol^-1 Finally, determine which direction the reaction is spontaneous as write at 25.0 degree C and standard pressure. forward reverse both neither

Explanation / Answer

Q1.

dSrxn = Sproducts - Sreactants

dSRxn = C6H6 - 3*C2H2 = (173.4 ) -(3*200.9) = -429.3 J/Kmol

now

dG = dH - T*dS

substitute

dS = in kJ/molK --> -0.4293

dG = -633.1 - 298*(-0.4293)

dG = -505.168 J/mol

dG = -0.505 kJ/mol

this is negative, so this favours products, so it must go in the forward direction

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