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- 1. For the reaction 2 Hg(l) + O2(g) → 2 HgO(s), ∆rH° = 181.6 kJ/mol-rxn. What is the enthalpy change to decompose 1.00 mol of HgO(s) to O2(g) and Hg(l)? 3633 kJ −90.8 kJ 90.8 kJ 363.3 kJCalculate the heat of reaction for: 2 C + 4 H2 + O2 ----> 2 CH3OH given: C + O2 ----> CO2 ΔH = -393.5 kJ 2 H2 + O2 ----> 2 H2O ΔH = -571.6 kJ 2 CH3OH + 3 O2 ----> 2 CO2 + 4 H2O ΔH = -1452.8 kJ a) -3383 kJ b) -477.4 kJ c) 3383 kJ d) 94.2 kJ e) -94.2 kJ0 Calculate AH for the following reaction, after it is properly balanced with smallest whole-number coefficients: rxn C,H%(g) + Ozg) → COz(g) + H,O(g) AH [C₂H6(g)] = -84.667 kJ/mol AH [CO₂(g)] = -393.5 kJ/mol AH [CO₂(aq)] = −412.9 kJ/mol AH [H₂O(g)]=-241.826 kJ/mol AH [H₂O()] = -285.840 kJ/mol f kJ [unbalanced]
- 8. Given the standard heats of formation for the following compounds, calculate the ΔH° heat of reaction, for the following reaction: Fe3O4(s) + CO(g) ---> 3 FeO(s) + CO2(g) ΔHf° for Fe3O4 = -1118 kJΔHf° for CO = -110.5 kJΔHf° for FeO = -272 kJΔHf° for CO2 = -393.5 kJ Please show workFind the heat of reaction and explain what happen to it. Calculate the ∆H of reaction for: C3H8 (g) + 5O2 (g) => 3CO2 (g) + 4H2O (l) The values of ∆H of reaction are as follows:C3H8 (g) = -103.95 kJ/molCO2 (g) = -393.5 kJ/molH2O (g) = -285.8 kJ/mol Topic: Enthalpy of ReactionDiethyl ether, C4H10O(l), a flammable compound that wasonce used as a surgical anesthetic, has the structure H3C-CH2- O- CH2-0 CH3 The complete combustion of 1 mol of C4H10O1l2 to CO21g2and H2O(l) yields ΔH° = -2723.7 kJ. (a) Write a balancedequation for the combustion of 1 mol of C4H10O(l). (b) Byusing the information in this problem and data in Table 5.3,calculate ΔHf° for diethyl ether.
- 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.…If a given reaction is A + B --> 2C with ΔH = 123.4 kJ and the needed reaction is 2A + 2B --> 4C, what is the ΔH for the needed reaction?
- Consider the combustion of liquid methanol, CH3OH1l2:CH3OH1l2 + 32O21g2¡ CO21g2 + 2 H2O1l2ΔH = -726.5 kJ(a) What is the enthalpy change for the reverse reaction?(b) Balance the forward reaction with whole-number coefficients.What is ΔH for the reaction represented by thisequation? (c) Which is more likely to be thermodynamicallyfavored, the forward reaction or the reverse reaction?(d) If the reaction were written to produce H2O1g2 insteadof H2O1l2, would you expect the magnitude of ΔH to increase,decrease, or stay the same? Explain.C6H4(OH)2(aq) + H2O2(aq) ® C6H4O2(aq) + 2H2O(l) hydroquinone quinone Calculate ∆HRxN for this reaction from the following data, CLEARLY SHOWING ALL CALCULATIONS: (i) C6H4(OH)2(aq) = C6H4O2(aq) + H2(g) ∆H = + 177.4 kJ (ii) H2(g) + O2(g) = H2O2(aq) ∆H = – 191.2 kJ (iii) H2(g) + 1/2 O2(g) = H2O(g) ∆H = – 241.8 kJ (iv) H2O(g) = H2O(l) ∆H = – 43.8 kJC6H4(OH)2(aq)+H2O2(aq) -> C6H4O2(aq) +2H2O(I) ^ Hydrooquinone Calculate HRxN for this reaction froom the following data, Show all calculation. (i) C6H4(OH)2(aq) -> C6H4O2(aq) +H2(g) H=+177.4 kJ (ii) H2(g) + O2(g) -> H2O2(aq) H=-191.2 kJ (iii) H2(g) +1/2 O2(g) -> H2O(g) H= -241.8 kJ (iv) H20(g) -> H2O(I) H=-43.8 kJ