Questions: Use the following information to answer the next question Sour gas is a mixture of predominantly methane gas and hydrogen sulfide gas. The Claus process can be used to remove hydrogen sulfide gas from sour gas as represented by the following equation. 8 H2 S(g)+4 O2(g) -> S8(s)+8 H2O(g) ΔH°=-1769.6 kJ 5. The enthalpy change for 1.00 mol of H2 S(g) during the Claus process, expressed in scientific notation, is ± a . b c × 10^d kJ / mol. The values of a, b, c and d are (Record your four-digit answer in the numerical-response section below.) Your answer:

Use the following information to answer the next question

Sour gas is a mixture of predominantly methane gas and hydrogen sulfide gas. The Claus process can be used to remove hydrogen sulfide gas from sour gas as represented by the following equation.
8 H2 S(g)+4 O2(g) -> S8(s)+8 H2O(g) ΔH°=-1769.6 kJ
5. The enthalpy change for 1.00 mol of H2 S(g) during the Claus process, expressed in scientific notation, is ± a . b c × 10^d kJ / mol. The values of a, b, c and d are
(Record your four-digit answer in the numerical-response section below.)
Your answer:

Transcript text: Use the following information to answer the next question Sour gas is a mixture of predominantly methane gas and hydrogen sulfide gas. The Claus process can be used to remove hydrogen sulfide gas from sour gas as represented by the following equation. \[ 8 \mathrm{H}_{2} \mathrm{~S}(\mathrm{~g})+4 \mathrm{O}_{2}(\mathrm{~g}) \rightarrow \mathrm{S}_{8}(\mathrm{~s})+8 \mathrm{H}_{2} \mathrm{O}(\mathrm{g}) \quad \Delta H^{\circ}=-1769.6 \mathrm{~kJ} \] 5. The enthalpy change for 1.00 mol of $\mathrm{H}_{2} \mathrm{~S}(\mathrm{~g})$ during the Claus process, expressed in scientific notation, is $\pm \mathbf{a} . \mathbf{b c} \times 10^{\mathrm{d}} \mathrm{kJ} / \mathrm{mol}$. The values of $\boldsymbol{a}, \boldsymbol{b}, \boldsymbol{c}$ and $\boldsymbol{d}$ are $\qquad$ $\qquad$ and $\qquad$ (Record your four-digit answer in the numerical-response section below.) Your answer: $\square$ $\square$ $\square$

Solution

Solution Steps

Step 1: Understanding the Given Reaction and Enthalpy Change

The given reaction is: \[ 8 \mathrm{H}_{2} \mathrm{~S}(\mathrm{~g}) + 4 \mathrm{O}_{2}(\mathrm{~g}) \rightarrow \mathrm{S}_{8}(\mathrm{~s}) + 8 \mathrm{H}_{2} \mathrm{O}(\mathrm{g}) \quad \Delta H^{\circ} = -1769.6 \mathrm{~kJ} \]

This indicates that the enthalpy change for the reaction involving 8 moles of $\mathrm{H}_{2} \mathrm{~S}$ is $-1769.6 \mathrm{~kJ}$.

Step 2: Calculating the Enthalpy Change per Mole of $\mathrm{H}_{2} \mathrm{~S}$

To find the enthalpy change for 1 mole of $\mathrm{H}_{2} \mathrm{~S}$, we divide the total enthalpy change by the number of moles of $\mathrm{H}_{2} \mathrm{~S}$ involved in the reaction:

\[ \Delta H_{\text{per mole}} = \frac{-1769.6 \mathrm{~kJ}}{8 \text{ moles}} \]

Step 3: Performing the Division

\[ \Delta H_{\text{per mole}} = -221.2 \mathrm{~kJ/mol} \]

Step 4: Expressing the Result in Scientific Notation

The enthalpy change per mole of $\mathrm{H}_{2} \mathrm{~S}$ in scientific notation is:

\[ -221.2 \mathrm{~kJ/mol} = -2.212 \times 10^{2} \mathrm{~kJ/mol} \]