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Question

If the Gibbs free energy change when 1 mole of NaCl is dissolved in water at 298K is x kJ, then -1000x is
Given that,
(a) Lattice energy of NaCl = 778 kJmol1
(b) Hydration energy of NaCl=774.3 kJmol1
(c) Entropy change at 298K=43 Jmol1.

A
9117
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B
9441
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C
9114
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D
9141
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Solution

The correct option is B 9114
ΔHdissolution=ΔH(ionisation)+ΔH(hydration)=778774.3
=3.7kJmol1=3700Jmol1
ΔSdissolution=43JK1
ΔGdissolution=ΔHTΔS
=3700298×43=9114J

ΔG=9.114kJ

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