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Silane (SiH(4)) burns in air as: SiH(4...

Silane `(SiH_(4))` burns in air as:
`SiH_(4)(g) +2O_(2)(g) rarr SiO_(2)(s) +2H_(2)O(l)`
the standard Gibbs energies of formation of `SiH_(4)(g), SiO_(2)(s)`, and `H_(2)O(l)` are `+52.3, -805.0`, and `-228.6kJ mol^(-1)`, respectively. Calculate Gibbs enegry change for the reaction and predict whether the reaction in spontaneous or not.

Text Solution

Verified by Experts

`SiH_(4)(g) + 2O_(2)(g) to SiO_(2)(g) + 2H_(2)O(l)`
`Delta_(r)G^(@) = Delta_(r)G^(@)(SiO_(2)) + 2 Delta_(r)G^(@)(H_(2)O) - [Delta_(r)G^(@)(SiH_(4)) + 2Delta_(r)G^(@)(O_(2))]`
` = - 805.0 + 2(-228.6) - [+ 52.3 + 2(0)]`
` = - 805.0 - 457.2 - 52.3`
`= - 1314.5 kJ`
Since `Delta_(r)G^(@)` is negative, the reaction will be spontaneous.
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