One renewable energy fuel source is hydrogen. Hydrogen fuel cells use the chemical energy of hydrogen to cleanly and efficiently produce electricity. However, hydrogen is usually “tied-up” in other molecules such as hydrocarbons and must be harvested. The two main ways this is done is by (1) “splitting” water to make hydrogen gas or (2) reforming natural gas (methane). However, process 2 means we are using fossil fuels (non-renewable energy sources) to create renewable energy.(1) H2O(l) → H2(g) + ½ O2(g) ΔHrxn = +285.8 kJ/mol(2) CH4(g) + 2H2O(g) → CO2(g) + H2(g) ΔHrxn = _______ kJ/molUsing the standard enthalpies of formation in the table below and equation 7.15 (Tro pg. 292), calculate ΔHrxn for reaction 2. (I have a included an image of this equation)SubstanceΔHf°(kJ/mol)CH4(g)-74.6H2O(g)-241.8H2O(l)-285.8CO2(g)-393.5CO2(aq)-413.8b. compare the reaction enthalpies for splitting water and for reforming natural gas. The image displays the formula for the standard enthalpy change of a reaction (\(\Delta H_{\text{rxn}}\)):\[\Delta H_{\text{rxn}} = \sum n_p \Delta H_f^{\circ} (\text{products}) - \sum n_r \Delta H_f^{\circ} (\text{reactants})\]In this equation:- \(n_p\) and \(n_r\) represent the stoichiometric coefficients of the products and reactants, respectively.- \(\Delta H_f^{\circ}\) refers to the standard enthalpies of formation.The text emphasizes that when using this equation, it is important to remember that elements in their standard states have \(\Delta H_f^{\circ} = 0\). Examples 7.11 and 7.12 (not shown here) demonstrate this process.

Hydrogen Fuel Cells provide an inherently clean source of energy, with no adverse impact on…

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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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One renewable energy fuel source is hydrogen. Hydrogen fuel cells use the chemical energy of hydrogen to cleanly and efficiently produce electricity. However, hydrogen is usually “tied-up” in other molecules such as hydrocarbons and must be harvested. The two main ways this is done is by (1) “splitting” water to make hydrogen gas or (2) reforming natural gas (methane). However, process 2 means we are using fossil fuels (non-renewable energy sources) to create renewable energy.

(1) H₂O(l) → H₂(g) + ½ O₂(g) ΔH_rxn = +285.8 kJ/mol

(2) CH₄(g) + 2H₂O(g) → CO₂(g) + H₂(g) ΔH_rxn = _______ kJ/mol

Using the standard enthalpies of formation in the table below and equation 7.15 (Tro pg. 292), calculate ΔH_rxn for reaction 2. (I have a included an image of this equation)