For the reaction,
`2A(g)+B(g)to2D(g)`
`DeltaU^(theta)=-10.5 kJ and DeltaS^(theta)=-44.1 JK^(-1)`
Calculate `DeltaG^(theta)` for the reaction, and predict whether the reaction can occur spontaneously or not.

Explanation

`2A_(g)+B_(g) to 2D_(g)`
`n_(g)=2-3=-1`
`triangleH=trianglev+n_(g) RT`
`triangleH=-10.5 +(-1) xx (8.314)/(10^(3)) xx 298`
`-10.5 -2.477 ="-12.977 KJ mol"^(-1)`
`triangleS=-44.1 JK^(-1)`
`triangleG^@=triangleH-TtriangleS`
`triangleG^@=-12.977-298 (-44.1)`
=-12977 +13141.8 =1648 J or +0.1648J
`triangleG^@ ` is +ve the reaction is non-spontaneous.