1) For the following reaction, calculate the S rxn at 25 o C given the absolutio

Question

1) For the following reaction, calculate the Srxn at 25oC given the absolution entropies:

2A(g) + B(g) 2C(g)

SoA = 30.6 J/molK,  SoB = 128.9 J/molK ,  SoC = 55.8  J/molK

2) For the reaction A(g) + 2B(g) 2C(g) Go = -32.8 kJ. What is the value of Go in kJ for the complete reaction of 0.231mol of B

3) A reaction spontaneously produces product when starting with just reactant. Once equilibrium is established, there are 1000 times more reactants than products. What are the signs of G and Go for the reaction at the beginning of the reaction when starting off with just reactant? Are the signs positive or negative (+,-) or (-,+) or (-,-) or (+,+)

Explanation / Answer

1) to calculate delta S calculate the difference between the initial and final delta S:

Initial delta S i.e. sum of deltaS for reactants is 2(30.6) + 128.9 -> 190.1 J/molK

Final delta S i.e. sum of delta S for product is 2(55.8) ->111.6 J/molK

hence delta S for the reaction equals 111.6-190.1 -> -78.5J/molK

2) delta G is 0.231 8 -32.8

3) delta G will be (-,-)

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