The reaction between carbon tetrachloride, ccl4, and water, h2o, to form carbon dioxide, co2, and hydrogen chloride, hcl, has a ? g? value of ? 232 kj/mole, and so is thermodynamically favored. but when you mix carbon tetrachloride with water, no change is observed. what is a possible explanation for this? a)it is a slow reaction kinetically. b)the activation energy of the reaction is too small. c)the reaction is not spontaneous. d)the reaction is not favored thermodynamically

a)It is a slow reaction kinetically.

Explanation:

The reaction of CCl₄ with H₂O is:

CCl₄ + H₂O → CO₂ + HCl the ΔG is -232kJ/mol

As ΔG<0 the reaction is spontaneous, that means the reaction is themodynicamically favored. Thus, c and d are false.

The activation energy is defined as the minimum amount of energy that is required for a reaction occurs, if the activation energy of the reaction is small, will be easy that the reaction occurs, thus, b is false.

In a chemical reaction, there are involve the thermodynamic and kinetic items. The reaction is thermodynamically favored but there is no data about kinetics of the reaction. Thus it is possible that is a slow reaction doing a true.

I hope it helps!

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