QUESTION 25 An important step in the synthesis of nitric acid is the conversion of ammonia to nitric oxide. AH'f [NH3(g)] = -45.9 kJ/mol; AH'f [NO(g)] = 90.3 kJ/mol; AH*f [H20(g)] = -241.8 kJ/mol 4NH3(9) + 502(g) –- 4NO(g) + 6H20(g) What is the AH'rxn for this reaction? -906.0 kJ 197.4 kJ 906.0 kJ -197.4 kJ

QUESTION 25 An important step in the synthesis of nitric acid is the conversion of ammonia to nitric oxide. AH'f [NH3(g)] = -45.9 kJ/mol; AH'f [NO(g)] = 90.3 kJ/mol; AH*f [H20(g)] = -241.8 kJ/mol 4NH3(9) + 502(g) –- 4NO(g) + 6H20(g) What is the AH'rxn for this reaction? -906.0 kJ 197.4 kJ 906.0 kJ -197.4 kJ

Chemistry & Chemical Reactivity

10th Edition

ISBN:9781337399074

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter5: Principles Of Chemical Reactivity: Energy And Chemical Reactions

Section: Chapter Questions

Problem 115SCQ: Methane, CH4, can be converted to methanol, which, like ethanol, can be used as a fuel. The energy...

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Methane, CH4, can be converted to methanol, which, like ethanol, can be used as a fuel. The energy level diagram shown here presents relationships between energies of the fuels and their oxidation products. Use the information in the diagram to answer the following questions. (The energy terms are per mol-rxn.) (a) Which fuel, methanol or methane, yields the most energy per mole when burned? (b) Which fuel yields the most energy per gram when burned? (c) What is the enthalpy change for the conversion of methane to methanol by reaction with O2(g)? (d) Each arrow on the diagram represents a chemical reaction. Write the equation for the reaction that converts methane to methanol.
Give only typing answer with explanation and conclusion to all parts CH4 + 2O2 ------- CO2 + 2H2O + 890.1 kj What is theoretical yield of CO2 in moles using 1.5 moles of O2? What is theoretical yield of H2O in grams using 1.5 moles of CH4? How much heat is released by burning 120 g of O2?
2KCl(s) + 3O2(g) 2KClO3(s)Which of these 5 are true for the reaction above? Check all that apply. Hrxn is 89.0kJ. Hrxn is -827.3kJ. The reaction is endothermic, +H. The reaction is exothermic, –H. Heat is a reactant.
When 0.2490 moles of methane, CH4(g) is burned in excess oxygen at thermodynamic standard state, 221.74 kJ of heat is released. What is ΔHfor the combustion for 1 mole of methane, CH4(g)? CH4(g) + 2 O2(g) -> CO2(g) + 2 H2O(l) ΔHrxn= ______________________ 2) What is the enthalpy change for making exactly 2 moles of methane (instead of combusting the methane) by the following reaction: CO2(g) + 2 H2O(l) -> CH4(g) + 2 O2(g)
The burning of 48.7 g of ZnS in the presence of oxygen gives 220.0 kJ of heat. What is ΔH for the reaction as written below? 2 ZnS + 3 O2 ----> 2 ZnO + 2 SO2 a) -110 kJ b) -293 kJ c) -441 kJ d) -882 kJ e) +441 kJ
HCl + NaOH --> H2O + NaCl how many grams of water were produced if the reaction above took place in 200. mL of solution and the temp changed from 25.5 °C to 27.5 °C? assume the reaction occurs in a coffee cup calorimeter the density of the solution is 1.0 g/mL and the heat capacity is 4.2 J/g°C. the enthalpy of reaction ▲H is -58 kJ/mol water
A 1.3-g sample of rice is placed in a calorimeter. When the sample is burned, 22.00 kJ is given off. What is the energy value, in kcal/g, for the rice?
When 1.00 gg of toluene, C7H8 C7H8 , is burned in a bomb calorimeter, the temperature rises by 13.0 ∘C∘C. If the heat capacity for the calorimeter is 3.21 kJ/∘CkJ/∘C, calculate the combustion energy (ΔE)(Δ�) for toluene in kilojoules per mole. Please type answer note write by hend.
33.9 Given the following two reactions and their enthalpy changes, 2 ClO2 (g) --> Cl2 (g) + 2 O2 (g) Delta H = – 204 kJ 2 TiCl4 (l) + 2 O2 (g) --> 2 TiO2 (s) + 4 Cl2 Delta H = – 139.8 kJ What is the value of the enthalpy change for the reaction that is the sum of these two reactions? 2 ClO2 (g) + 2 TiCl4 (l) --> 2 TiO2 (s) + 5 Cl2 Delta H = ? Select one: a. – 64 kJ b. – 344 kJ c. 64.2 kJ d. 64 kJ e. 344 kJ f. – 204 kJ g. none of these
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need it fast!! Calculate the standard enthalpy change ∆Ho for the reaction below in kJ given the following standard enthalpy of formation values (kJ): NH4NO3(s) = -365.3, N2O(g) = 81.6, H2O(g)= -241.8 NH4NO3(s) -> N2O(g) + 2 H2O(g)
Balance the following reactions, calculate [delta]Hrxn, calculate the energy released (or required) for the combustion of 10.00 grams of fuel (H2, CH4 (methane), or C4H10 (butane)) in each reaction, and compare the energetics for the reactions (which is the best fuel). H2 (g) + O2 (g) --> H2O (g) CH4 (g) + O2 (g) --> CO2 (g) + H2O (g) C4H10 (g) + O2 (g) --> CO2 (g) + H2O (g)