Question

Can anyone solve my this chemistry work?

Answer 1

Not spontaneous at standard conditions, and an increase in temperature will make the reaction more likely to become spontaneous, becoming spontaneous when `T>2086.702606K`

Explanation:

A reaction is spontaneous if `DeltaG^circ<0`

`DeltaG^circ=DeltaH^circ-TDeltaS^circ`

`T=298K`
`DeltaH^circ=(-59.9-110.6)-(-635)=464.5kJ` `mol^-1`
`DeltaS^circ=(197.7+70.3)-(5.7+39.7)=222.6J` `mol^-1` `K^-1` `=0.2226kJ` `mol^-1` `K^-1`

`DeltaG^circ=464.5-298(0.2226)=398.1652~~398kJ` `mol^-1`

The reaction is not spontaneous in standard conditions.

An increase in temperature will result in a greater value for `TDeltaS^circ`, and therefore make `DeltaG^circ` less and less positive until it becomes negative.

The reaction becomes spontaneous when `DeltaG^circ<0`, so `DeltaH^circ< TDeltaS^circ`

`T>464.5/0.2226`
`T>2086.702606K`

When `T>2086.702606K`, the reaction becomes spontaneous.