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...

See similar textbooks

Similar questions

2. Show the Boyle temperature for a van der Waals gas is T Rb Hint: (1- a)-N1+a
1 mol of an ideal gas at 25 ° C and 10 atmospheres (Cp = 3.5 R), adiabatically and reversibly 5 What will be the final volume and temperature when it expands into the atmosphere?
Problem #6: Discovering the deepest seas requires professional deep-sea divers to use special tanks with Heliox- a diving gas mix that may have a typically less of oxygen as regular air but completely replaces the nitrogen with helium for their safety and support underwater. If a diver travels 150 meters below sea level, they may experience the weight of around 10 atm. Their 10-liter tanks contain 55.3 g of 02 and 330.6 g of He as trace gases. As they descend into the sea floor, what would be the partial pressure of oxygen and helium and the total pressure in the container at a temperature of 18 •C?
As we have discussed in class, CO is highly toxic. An added danger comes from the fact that CO is very slightly less dense than air, so it rises up from the malfunctioning furnace in the basement to the bedrooms upstairs... victims are poisoned while they sleep. Calculate the density of CO and air: assume 298 K and 1 atm (assume air is 22% O2, 78% N2). (Remember not to round anything until your calculation is finished.)
1. Recall the following relationship developed in lecture: =T av - P a) What is the name of this relationship? b) Evaluate for an ideal gas. c) What is the significance of this result in terms of an ideal gas? d) Evaluate av for a van der Waals gas. e) What is the significance of this result in terms of a van der Waals gas?
In the van der Waals equation there is a large difference in the "a" values for HF and Ne despite them having almost the same Molar Mass and similar size. Why is the "a" value for these so compounds so different? FULLY EXPLAIN esc ck Edit Format Table 12pt Paragraph Р 1 A N C B I U @ 2 W S #3 X E H D $ 4 R C 8 % 5 F ¡ T V MacBook Pro I ➡ A 6 G Y & 7. B H f U 0 words *00 8 J N ⠀⠀ ( 1 9 K M MOSIS
(E) Could you gather existing thermodynamic data and find what the free energy of pure water (H2O) is around room temperature? Could you draw the phase diagram for whater from 0-100c from the data?
Needs Complete typed solution with 100 % accuracy.
Hello, I understand that cp for diatomic ideal gas is 7/2R. How do I find the same for a gas like carbon dioxide?
a. At 300 K which speed has the greatest fraction of molecules per unit speed interval? b. At 1000 K which speed has the greatest fraction of molecules per unit speed interval?
Compute the density of Methane (CH4) at 10 bar pressure and 36 deg C temperature. Hints: Use molecular weight of carbon = 12g and use molecular weight of Hydrogen = 1.01g
Q6.50 Homework • Unanswered If we made a mixture containing molecules of several different gases having strong intermolecular attractions, the total pressure of the mixture would the sum of the partial pressures. Select an answer and submit. For keyboard navigation, use the up/down arrow keys to select an answer. a Equal b Be less than Be greater than