Question

given the following information A+B->2D delta H=-710.9kJ delta S= 298.0J/K C->D     delta H =515kJ delta S=-192...

given the following information

A+B->2D delta H=-710.9kJ delta S= 298.0J/K

C->D     delta H =515kJ delta S=-192 J/K

calculate the delta G for the following reaction at 298K.

A+B->2C

**PLEASE SHOW WORK**

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Homework Answers

Answer #1

Lets number the reaction as 1, 2, 3 from top to bottom

required reaction should be written in terms of other reaction

This is Hess Law

required reaction can be written as:

reaction 3 = +1 * (reaction 1) -2 * (reaction 2)

So, deltaHo rxn for required reaction will be:

deltaHo rxn = +1 * deltaHo rxn(reaction 1) -2 * deltaHo rxn(reaction 2)

= +1 * (-710.9) -2 * (525.0)

= -1760.9 KJ

So, deltaSo rxn for required reaction will be:

deltaSo rxn = +1 * deltaSo rxn(reaction 1) -2 * deltaSo rxn(reaction 2)

= +1 * (298.0) -2 * (-192.0)

= 682 J/K

deltaHo = -1760.9 KJ/mol

deltaSo = 682 J/mol.K

= 0.682 KJ/mol.K

T = 298 K

we have below equation to be used:

deltaGo = deltaHo - T*deltaSo

deltaGo = -1760.9 - 298.0 * 0.682

deltaGo = -1964 KJ

Answer: -1964 KJ

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