To use Hess's law to calculate the enthalpy change for the reaction \( A \rightarrow C \), we need to have other related reactions and their enthalpy changes. Hess's law states that the total enthalpy change for a reaction is the sum of the enthalpy changes for individual steps, regardless of the pathway taken.
For example, if we have the following two reactions with their respective enthalpy changes:
- \( A \rightarrow B \) with \( \Delta H_1 \)
- \( B \rightarrow C \) with \( \Delta H_2 \)
We can use Hess's law as follows:
\[ \Delta H_{A \rightarrow C} = \Delta H_1 + \Delta H_2 \]
Without specific values for \( \Delta H_1 \) and \( \Delta H_2 \) provided, I cannot calculate the exact value for \( A \rightarrow C \). Please provide the enthalpy changes for the relevant reactions, and I can help you compute the total enthalpy change for the reaction \( A \rightarrow C \).