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Question

Silane, SiH4 like methane, burns in air. The product silica (silicon dioxide) is solid quite unlike carbondioxide.
SiH4(g)+2O2(g)SiO2(s)+2H2O(g) standard Gibbs energy of formation of SiO2(s), H2O and SiH4 are 805, – 228.6 and + 52.3 (all is KJ mol1) respectively. Calculate the value of ΔrG.

A
1314.5KJmol1
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B
1413KJmol1
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C
1134.5KJmol1
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D
3411.5KJmol1
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Solution

The correct option is A 1314.5KJmol1
Applying equation,
ΔrG=VpΔfG(products)VpΔfG(reactants)

=[ΔfG(SiO2)+2ΔfG(H2O)][ΔfG(SiH4)+2ΔfG(O2)]
Gibbs energy of formation of elements being zero, we have
ΔrG=[(805KJmol1)+(228.6KJmol1)][1(+52.3KJmol1)+0]
=1314.5KJmol1
Negative value of ΔrG supports spontaneity of the above reaction.

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