9. **Calculate the Enthalpy of the Reaction***Reaction Equation:*\[ 2A + 5B + 5C \rightarrow 4D + 4E \]*Data Table:*\[\begin{array}{|c|c|c|}\hline\text{Substance} & \Delta H_f^\circ (\text{kJ/mol}) & S^\circ (\text{J/mol/K}) \\\hlineA & -33.22 & 177.31 \\B & -88.23 & 137.60 \\C & 59.52 & 96.15 \\D & 34.96 & 3.70 \\E & 91.71 & 108.69 \\\hline\end{array}\]*Instructions:*To calculate the reaction's enthalpy, use the formula for the change in enthalpy (\(\Delta H\)) of a reaction:\[\Delta H = \sum (\Delta H_f^\circ \text{ of products}) - \sum (\Delta H_f^\circ \text{ of reactants})\]Apply the stoichiometric coefficients from the balanced chemical equation when summing the enthalpies for the products and reactants.

Hess's law states that the amount of heat evolved or absorbed in a process is independent of the…

Answered: Calculate the enthalpy of the following…

Calculate the enthalpy of the following reaction using the data in the table. 2A +2B + 5C 4D + 4E sOU/mol/K) AHF°(kJ/mol) A -33.22 177.31 B -88.23 137.60 C 59.52 96.15 D 34.96 3.70 E 91.71 108.69

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Concept explainers

Crystal Structures

Solids are present all around us. They have different properties and applications. Diamond and graphite are two well-known solids. Diamond is the hardest material in the world and is used in making jewelry. Graphite on the other hand is soft. The lead of your pencil is graphite. Why are they so different in appearance and properties despite the fact they are chemically the same? Both are allotropes of carbon. The answer lies in the structure, the way constituent particles are arranged in the solids.

Question

**Calculate the Enthalpy of the Reaction**

*Reaction Equation:*
\[ 2A + 5B + 5C \rightarrow 4D + 4E \]

*Data Table:*

\[
\begin{array}{|c|c|c|}
\hline
\text{Substance} & \Delta H_f^\circ (\text{kJ/mol}) & S^\circ (\text{J/mol/K}) \\
\hline
A & -33.22 & 177.31 \\
B & -88.23 & 137.60 \\
C & 59.52 & 96.15 \\
D & 34.96 & 3.70 \\
E & 91.71 & 108.69 \\
\hline
\end{array}
\]

*Instructions:*

To calculate the reaction's enthalpy, use the formula for the change in enthalpy (\(\Delta H\)) of a reaction:

\[
\Delta H = \sum (\Delta H_f^\circ \text{ of products}) - \sum (\Delta H_f^\circ \text{ of reactants})
\]

Apply the stoichiometric coefficients from the balanced chemical equation when summing the enthalpies for the products and reactants.

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