To calculate the reaction enthalpy under standard conditions, we will need to use the standard enthalpies of formation for each substance in the reaction:

The reaction is:

$8 \text{H}_2\text{S}(\text{g}) + 4 \text{O}_2(\text{g}) \rightarrow \text{S}_8 (\text{s, rhombic}) + 8 \text{H}_2\text{O}(\text{l})$

The reaction enthalpy ($\Delta H_{\text{reaction}}$) can be calculated with the following formula:

$\Delta H_{\text{reaction}} = \sum \Delta H_f^\circ(\text{products}) - \sum \Delta H_f^\circ(\text{reactants})$

Here's the general approach:

1. Obtain the Standard Enthalpies of Formation ($\Delta H_f^\circ$) for each compound in the reaction from the table (often given in kJ/mol):

   • $\text{H}_2\text{S}(\text{g})$
   • $\text{O}_2(\text{g})$
   • $\text{S}_8(\text{s, rhombic})$
   • $\text{H}_2\text{O}(\text{l})$

   Remember that for elements in their standard state (like $\text{O}_2$ and $\text{S}_8$ in this case), the enthalpy of formation is zero.

2. Plug in the values into the formula, multiply each by the number of moles, and compute the sum for products and reactants.

3. Subtract the reactants' sum from the products' sum to find the reaction enthalpy.

If you can provide the standard enthalpies of formation for each substance, I can assist in calculating the exact value. Alternatively, if you access these values from a standard source or the ALEKS platform, you can perform the substitution and calculation.

Would you like further assistance with specific values or details on each step?

Here are five follow-up questions that might be relevant:

1. What are standard enthalpies of formation, and why are they important in calculating reaction enthalpy?
2. How do we determine the sign of the enthalpy change (exothermic or endothermic) in a reaction?
3. Why is the enthalpy of formation zero for elements in their standard state?
4. How does the stoichiometry of a reaction affect the calculation of reaction enthalpy?
5. What are common units for enthalpy, and how do we convert between them?

Tip: Always double-check units and stoichiometric coefficients when performing thermodynamic calculations to ensure accuracy.