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In the given reaction, calculate standar...

In the given reaction, calculate standard free energy change at `25^(@)C:2NO(g)+O_(2)(g)to 2NO_(2)(g)`. Is the reaction spontaneous under standard conditios?
[Given: At `25^(@)C,DeltaG_(f)^(0)[NO(g)]=88.57kJ*mol^(-1) and DeltaG_(f)^(0)[NO_(2)(g)]=51.30kJ*mol^(-1)`.

Text Solution

Verified by Experts

`DeltaG^(0)=sumDeltaG_(f)^(0)("product")-sumDeltaG_(f)^(0)("reactants")`
In the given case,
`DeltaG^(0)=2DeltaG_(f)^(0)[NO_(2)(g)]-2DeltaG_(f)^(0)[NO(g)]-DeltaG_(f)^(0)[O_(2)(g)]`
Given: `DeltaG_(f)^(0)[NO(g)]=86.57kJ*mol^(-1)`
`DeltaG_(f)^(0)[O_(2)(g)]=0 and DeltaG_(f)^(0)[NO_(2)(g)]=51.30kJ*mol^(-1)`
[`because` STandard free energy of formation of an element=0]
`therefore DeltaG^(0)=2xx51.30-2xx86.57-0=-70.54kJ`
`because` The value of `DeltaG^0` is negative, so the reaction will be spontaneous under standard conditions.
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