Part B What is the enthalpy for reaction 1 reversed? reaction 1 reversed: N2O4→N2 + 202 Express your answer numerically in kilojoules per mole. • View Available Hint(s) ? AH =- 9.15 kJ/mol
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Q: What is the enthalpy for reaction 1 reversed? reaction 1 reversed: N2O4→N2 + 202
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A: Since ∆H = ∆E + ∆ngRT For the above reaction ∆ng = 2-4 = -2 R = 2 cal / mole-K T= 291 K ∆E =…
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Q: What is the enthalpy for reaction 1 reversed? reaction 1 reversed: 2NO + 02→2NO2 Express your answer…
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Q: What is the enthalpy for reaction 1 reversed? reaction 1 reversed: N2O4→N2 + 202 Express your answer…
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Q: Calculate the heat of reaction AH for the following reaction: 2 NH3(g)-N,(9) + 3 H,(g) You can find…
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Q: From this reaction 2NO(g) + 2H₂(g) à N₂(g) + 2H₂O(1), NO H2 N2 Sº (J/mol K) 75.10 191.5 192.3 AH'f…
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- Pentaborane B5H9(s) burns vigorously in O2 to give B2O3(s) and H2O(l). What is ΔH° for the combustion of 1 mol of B5H9(s)? Delta heats of formation for substances B5H9(s) +73.2 B2O3 -1273.5 H2O(l) -285.8Determine ΔS0 for the following reaction using the data from the table. Explain whether this value agrees with prediction of the ΔS0 value. C2H5OH (l) + 3 O2 (g) → 2 CO2 (g) + 3 H2O (g)For which one of the following reactions is the value of ΔH°rxn equal to ΔH°f for the product? C (s, graphite) + 2H2(g) → C2H4 (g) 2H2 (g) + O2 (g) → 2H2O (l) 2H2 (g) + O2 (g) → 2H2O (g) H2O (l) + 1/2 O2 (g) → H2O2 (l)
- Calculate ΔG°rxn, ΔH°rxn, and ΔS°rxn of the following reaction: N2(g) + O2(g) -> 2NO(g)Using the table of average bond dissociation enthalpies at 25°C, determine which of the following reactions are energetically favorable at room temperature. Assume that ▲S = 0. Q.CH2=CH2 + 2H2 + N2 --> H2NCH2CH2NH2Estimate ΔG°rxn for the following reaction at 317 K. HCN(g) + 2 H2(g) → CH3NH2(g) ΔH°= -158.0 kJ; ΔS°= -219.9 J/K
- For which one of the following reactions is the value of ΔH0rxn equal to ΔH0f for the product? H2(g) + O2(g) → 2H2O(g) None of these. H2O2(g) + ½ O2(g) → H2O2(l) 2H2(g) + O2(g) → 2H2O(l)For which one of the following reactions is the value of ΔH°rxn EQUAL to ΔH°f for the product? (a) 2C(graphite) + 2H2(g) ➜ C2H4(g) (b) N2(g) + O2(g) ➜ 2NO(g) (c) N2(g) + O3(g) ➜ N2O3(g) (d) 2H2(g) + O2(g) ➜ 2H2O(g)When a neutralization reaction was carried out using 100.0 mL of 0.7890M NH3 water and 100.0 mL of 0.7940M acetic acid, ΔT was found to be 4.76 °C. The specific heat of the reaction mixture was 4.104 J g-l K-1 and its density was 1.03 g mL-1. The calorimeter constant was 3.36 JK-1 a) Calculate ΔH neutralization for the reaction of NH3 and acetic acid. b) At the end of the experiment, it was discovered that the thermometer had not been calibrated. When it was calibrated, it was found that the thermometer read 0.50 °C low. What effect would this thermometer reading have on the reported DH neutralization calculated above? c) When the temperature-time data graph was reviewed, it was found that an error had been made in determining ΔT. Instead of 4.76 °C, ΔT was actually 4.70 °C. Based on this change only, calculate the correct ΔH neutralization for the reaction of NH3, and acetic acid. d) Calculate the percent error for the correct ΔH neutralization if aΔ DT of 4.76 °C had been used.…
- When a neutralization reaction was carried out using 100.0 mL of 0.7890M NH3 water and 100.0 mL of 0.7940M acetic acid, ΔT was found to be 4.76 °C. The specific heat of the reaction mixture was 4.104 J g-l K-1 and its density was 1.03 g mL-1. The calorimeter constant was 3.36 JK-1 a) Calculate ΔH neutralization for the reaction of NH3 and acetic acid. b) At the end of the experiment, it was discovered that the thermometer had not been calibrated. When it was calibrated, it was found that the thermometer read 0.50 °C low. What effect would this thermometer reading have on the reported DH neutralization calculated above? c) When the temperature-time data graph was reviewed, it was found that an error had been made in determining ΔT. Instead of 4.76 °C, ΔT was actually 4.70 °C. Based on this change only, calculate the correct ΔH neutralization for the reaction of NH3, and acetic acid. d) Calculate the percent error for the correct ΔH neutralization if aΔ DT of 4.76 °C had been used.…An English chemistry professor needs a cup of hot tea before grading 50 homeworkassignments but his electric water heater is broken . In his lab, however, he doeshave some ethanol (CH3CH2OH, MW=46.07gmol-1) and 1 gram of benzoic acid(C6H5COOH, MW=122.12 gmol-1). He knows that the benzoic acid has an enthalpyof combustion, H, of -3226.7 kJmol-1. In a constant volume (bomb) calorimeterinitially at 293.15 K, he finds that the combustion of 1.000 g of benzoic acidincreased the temperature to 297.67 K. In the exact same calorimeter, 1.000 g ofethanol raised the temperature from 293.15K to 298.38K.(a) What is the enthalpy of combustion for 1 mole of ethanol? I am confused about this question and I need help.Given the following enthalpy change values for the reactions below: A + B → 2C ; ΔrH = 305.5 kJ mol-1 C + 2D → E + F ; ΔrH = 135.1 kJ mol-1 H → ½ E + G ; ΔrH = -99.2 kJ mol-1 Calculate ΔrH for the following reaction (in kJ mol-1) using Hess's Law: A + B + 4D + 4G → 4H + 2F