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3. Calculate the heat of reaction, AHn, for the combustion of one mole of C,H(1) using the reactions provided below. rxn 6 C(s, graphite) + 3 H2(g) → CgHo(1) AH = 49.0 kJ H2(g) + ½ O2(g) → H2O(I) AH = -285.8 kJ %3D C(s, graphite) + O2(g) → CO2(g) AH = -393.5 kJ

3. Calculate the heat of reaction, AHn, for the combustion of one mole of C,H(1) using the reactions provided below. rxn 6 C(s, graphite) + 3 H2(g) → CgHo(1) AH = 49.0 kJ H2(g) + ½ O2(g) → H2O(I) AH = -285.8 kJ %3D C(s, graphite) + O2(g) → CO2(g) AH = -393.5 kJ

Chemistry
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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**Exercise #98 (Group Work – hand in)** 1. **Determine the amount of energy released when 93.6 g of liquid butane, C<sub>4</sub>H<sub>10</sub>(l), is combusted.** Given: - ΔH<sub>f</sub>°(CO<sub>2</sub>(g)) = -393.5 kJ/mol - ΔH<sub>f</sub>°(H<sub>2</sub>O(l)) = -285.8 kJ/mol - ΔH<sub>f</sub>°(C<sub>4</sub>H<sub>10</sub>(l)) = -147.6 kJ/mol 2. **Write the formation reactions for the following substances:** - Solid aluminum chloride, ΔH<sub>f</sub>° = -704.9 kJ/mol - Aqueous ammonium ion, ΔH<sub>f</sub>° = -132.5 kJ/mol 3. **Calculate the heat of reaction, ΔH<sub>rxn</sub>, for the combustion of one mole of C<sub>6</sub>H<sub>6</sub>(l) using the reactions provided below.** - 6 C(s, graphite) + 3 H<sub>2</sub>(g) ⟶ C<sub>6</sub>H<sub>6</sub>(l) ΔH = 49.0 kJ - H<sub>2</sub>(g) + ½ O<sub>2</sub>(g) ⟶ H<sub>2</sub>O(l) ΔH = -285.8 kJ - C(s, graphite) + O<sub>2</sub>(g) ⟶ CO<sub>2</sub>(g) ΔH = -393.5 kJ 4. **Calculate the heat of reaction, ΔH<sub>rxn</sub>, for the reaction between nitrogen and oxygen to form nitrogen dioxide using the reactions provided below.** - 2 NH<sub>3</sub>(g) ⟶ N<sub>2</sub>(g) + 3 H<sub>2</sub
Transcribed Image Text:**Exercise #98 (Group Work – hand in)** 1. **Determine the amount of energy released when 93.6 g of liquid butane, C<sub>4</sub>H<sub>10</sub>(l), is combusted.** Given: - ΔH<sub>f</sub>°(CO<sub>2</sub>(g)) = -393.5 kJ/mol - ΔH<sub>f</sub>°(H<sub>2</sub>O(l)) = -285.8 kJ/mol - ΔH<sub>f</sub>°(C<sub>4</sub>H<sub>10</sub>(l)) = -147.6 kJ/mol 2. **Write the formation reactions for the following substances:** - Solid aluminum chloride, ΔH<sub>f</sub>° = -704.9 kJ/mol - Aqueous ammonium ion, ΔH<sub>f</sub>° = -132.5 kJ/mol 3. **Calculate the heat of reaction, ΔH<sub>rxn</sub>, for the combustion of one mole of C<sub>6</sub>H<sub>6</sub>(l) using the reactions provided below.** - 6 C(s, graphite) + 3 H<sub>2</sub>(g) ⟶ C<sub>6</sub>H<sub>6</sub>(l) ΔH = 49.0 kJ - H<sub>2</sub>(g) + ½ O<sub>2</sub>(g) ⟶ H<sub>2</sub>O(l) ΔH = -285.8 kJ - C(s, graphite) + O<sub>2</sub>(g) ⟶ CO<sub>2</sub>(g) ΔH = -393.5 kJ 4. **Calculate the heat of reaction, ΔH<sub>rxn</sub>, for the reaction between nitrogen and oxygen to form nitrogen dioxide using the reactions provided below.** - 2 NH<sub>3</sub>(g) ⟶ N<sub>2</sub>(g) + 3 H<sub>2</sub
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