I need help with my hw problem. I figured out the delta H for the both temperature, but I cant not figure out how to solve for delta U. # Calculation of ΔᵣH and ΔᵣU for a Chemical Reaction## IntroductionThis exercise involves calculating the change in enthalpy (ΔᵣH) and the change in internal energy (ΔᵣU) for the reaction:\[ C_{(s,\text{graphite})} + H_2O_{(g)} \rightarrow CO_{(g)} + H_2_{(g)} \]The calculations are performed at two different temperatures: 298 K and 439 K. The data provided assumes that all heat capacities remain constant over the temperature range of interest.## Table of Standard Enthalpies and Heat CapacitiesThe table below lists the standard enthalpies of formation ($Δ_fH^\circ$) and molar heat capacities ($C^\circ_{p,m}$) of various substances at 298 K:| Compound | $Δ_fH^\circ$ (kJ·mol⁻¹) | $C^\circ_{p,m}$ (J·K⁻¹·mol⁻¹) ||--------------------|----------------------------|----------------------------------|| $H_2O (l)$ | -285.83 | 75.291 || $H_2O (g)$ | -241.82 | 33.58 || $CO (g)$ | -110.53 | 29.14 || $H_2 (g)$ | 0 | 28.824 || $H (g)$ | 217.97 | 20.784 || $C_{(s, \text{graphite})}$ | 0 | 8.527 || $C (g)$ | 716.68 | 20.838 || $C_2 (g)$ | 831.90 | 43.21 |## Calculations### For 298 K- $Δ_rH^\circ$ = 131.29 kJ·mol⁻¹ (correct)- $Δ_rU^\circ$ = 0.0158 kJ·mol⁻¹ (incorrect)### For 439 K- $Δ_rH^\circ$ = 133 kJ·mol

Given, At 298 K, ∆fH0 = 131.29 KJ / mole At 439 K, ∆fH0 = 133 KJ / mole

From the data in the table below, calculate A,H and A,U (in kJ•mol ) for the reaction C(s,graphite) + H,0(g) → CO(g) H2(g) at the following conditions. Assume all heat capacities to be constant over the temperature range of interest Standard enthalpies of formation of inorganic and organic compounds at 298 K AH°(kJ-mol¯1) c°m(J•K¯1•mol¯1) pim H20() -285.83 75.291 H20(g) -241.82 33.58 CO(g) -110.53 29.14 H2(g) 28.824 H(g) 217.97 20.784 C(s,graphite) 8.527 C(g) 716.68 20.838 C2(9) 831.90 43.21 (a) 298 K 131.29 kJ•mol¬1 0.0158 X kJ•mol-1 (b) 439 K 133 kJ•mol-1 133 X kJ-mol-1

From the data in the table below, calculate A,H and A,U (in kJ•mol ) for the reaction C(s,graphite) + H,0(g) → CO(g) H2(g) at the following conditions. Assume all heat capacities to be constant over the temperature range of interest Standard enthalpies of formation of inorganic and organic compounds at 298 K AH°(kJ-mol¯1) c°m(J•K¯1•mol¯1) pim H20() -285.83 75.291 H20(g) -241.82 33.58 CO(g) -110.53 29.14 H2(g) 28.824 H(g) 217.97 20.784 C(s,graphite) 8.527 C(g) 716.68 20.838 C2(9) 831.90 43.21 (a) 298 K 131.29 kJ•mol¬1 0.0158 X kJ•mol-1 (b) 439 K 133 kJ•mol-1 133 X kJ-mol-1

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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Question

I need help with my hw problem. I figured out the delta H for the both temperature, but I cant not figure out how to solve for delta U.

# Calculation of ΔᵣH and ΔᵣU for a Chemical Reaction

## Introduction

This exercise involves calculating the change in enthalpy (ΔᵣH) and the change in internal energy (ΔᵣU) for the reaction:

\[ C_{(s,\text{graphite})} + H_2O_{(g)} \rightarrow CO_{(g)} + H_2_{(g)} \]

The calculations are performed at two different temperatures: 298 K and 439 K. The data provided assumes that all heat capacities remain constant over the temperature range of interest.

## Table of Standard Enthalpies and Heat Capacities

The table below lists the standard enthalpies of formation ($Δ_fH^\circ$) and molar heat capacities ($C^\circ_{p,m}$) of various substances at 298 K:

| Compound | $Δ_fH^\circ$ (kJ·mol⁻¹) | $C^\circ_{p,m}$ (J·K⁻¹·mol⁻¹) |
|--------------------|----------------------------|----------------------------------|
| $H_2O (l)$ | -285.83 | 75.291 |
| $H_2O (g)$ | -241.82 | 33.58 |
| $CO (g)$ | -110.53 | 29.14 |
| $H_2 (g)$ | 0 | 28.824 |
| $H (g)$ | 217.97 | 20.784 |
| $C_{(s, \text{graphite})}$ | 0 | 8.527 |
| $C (g)$ | 716.68 | 20.838 |
| $C_2 (g)$ | 831.90 | 43.21 |

## Calculations

### For 298 K

- $Δ_rH^\circ$ = 131.29 kJ·mol⁻¹ (correct)
- $Δ_rU^\circ$ = 0.0158 kJ·mol⁻¹ (incorrect)

### For 439 K

- $Δ_rH^\circ$ = 133 kJ·mol

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