Using the data given below, establish that the vaporization of `C Cl_(4)(l)` 298 K to produce `C Cl_(4)(g)` at 1atm pressure does not occur spontaneously.
Given : `C Cl_(4)(l,1"atm")toC Cl_(4)(g 1 "atm")` ,
`DeltaS^(@)=94.98JK^(-1)mol^(-1)`
`DeltaH_(f)^(@)(C Cl_(4),g)=-106.7kJmol^(-1)`
`&DeltaH_(f)^(@)(C Cl_(4),l)=-139.3kJmol^(-1)`

Explanation

To determine whether the vaporization of carbon tetrachloride (CCl₄) from liquid to gas at 298 K and 1 atm is spontaneous, we can use the Gibbs free energy change (ΔG) for the process. The process is given as:

\[ \text{CCl}_4(l) \rightarrow \text{CCl}_4(g) \]

### Step 1: Calculate ΔH for the reaction

We can calculate the change in enthalpy (ΔH) for the vaporization process using the enthalpy of formation values provided:

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