Using the standard enthalpies of formation, calculate the standard enthalpy change for the overall reaction that occurs when ammonia is burned in air to form nitrogen dioxide and water. 4NH,(g) +70,,g) 4NO,(g) 6H.O(1) AH of NH₂(g) = -46 kJ/mol AH of NO(g) = 34 kJ/mol, AH of H₂O() = -286 kJ mol f f 5 O-360 kJ -1396 kJ O-1496 kJ O -1496 kJ Question 9 - 1 Not yet answered - Flag question

Using the standard enthalpies of formation, calculate the standard enthalpy change for the overall reaction that occurs when ammonia is burned in air to form nitrogen dioxide and water. 4NH,(g) +70,,g) 4NO,(g) 6H.O(1) AH of NH₂(g) = -46 kJ/mol AH of NO(g) = 34 kJ/mol, AH of H₂O() = -286 kJ mol f f 5 O-360 kJ -1396 kJ O-1496 kJ O -1496 kJ Question 9 - 1 Not yet answered - Flag question

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...

See similar textbooks

Similar questions

For questions 4-7 Calculate ?Hrxn for the given reaction using the enthalpy of formation values provided at the end of the assignment.4) CaO(s) + SO3(g) → CaSO4(s) Substance Heat of Formation (?Hf) in kJ/mol CaO(s) -635.5 SO₃(g) -395.2 CaSO₄(s) -1432.7 Al(s) 0 Fe₂O₃(s) -822.2 Al₂O₃(s) -1669.8 C₄H₁₀(l) -147.6 O₂(g) 0 CO₂(g) -393.5 H₂O(g) -241.8 H₂O(l) -285.8 H₂O₂(l) -187.6
< Question 21 of 29 O Attempt 2 When 0.376 g of sodium metal is added to an excess of hydrochloric acid, 3910 J of heat are produced. What is the enthalpy of the reaction as written? 2 Na(s) + 2 HCI(aq) 2 NaCl(aq) + H2(g) Enthalpy of reaction: 478.35 kJ Incorrect
Given the standard enthalpy changes for the following two reactions: ΔΗ° (1) N₂(g) + 2O2 (g) → 2NO2 (g) (2) 2N₂O(g) → 2N2(g) + O2(g) ΔΗ° = 66.4 kJ Standard enthalpy change : = - 164.2 kJ What is the standard enthalpy change for the following reaction? (3) 2N₂O(g) + 3O2 (g) → 4NO2 (g) AH° =? kJ
Consider the following reaction. CH3OH(g) CO(g) + 2 H2(g) H = +90.7 kJ ((b) Calculate the amount of heat transferred when 40.0 g of CH3OH(g) are decomposed by this reaction at constant pressure.H = kJ(c) If the enthalpy change is 20.0 kJ, how many grams of hydrogen gas are produced? g(d) How many kilojoules of heat are released when 12.5 g of CO(g) reacts completely with H2(g) to form CH3OH(g) at constant pressure?H = kJ(e) Calculate E when 880.0 g of CH3OH(g) completely reacts at a constant temperature of 300 K and constant pressure of 0.95 atm. R = 8.314 J/mol*K and R = 0.08206 atm*L/mol*K kJ HopHelpCh5N1
Find the enthapy change for the reaction below in kJ . 4NH3(g) + 5O2(g) --> 4NO(g) + 6H2O(g) ΔH= ? Given : (NH3(g)) = -46.1, (NO(g)) = + 90.3 kJ/mol and (H2O(g)) = -241.8 kJ/mol.
A student runs two experiments with a constant-volume "bomb" calorimeter containing 1300. g of water (see sketch at right). thermometer stirrer First, a 6.000 g tablet of benzoic acid (C,H,C0,H) is put into the "bomb" and burned completely in an excess of water oxygen. (Benzoic acid is known to have a heat of combustion of 26.454 kJ/g.) The temperature of the water is insulation observed to rise from 13.00 °C to 40.13 °C over a time of 10.0 minutes. Next, 5.200 g of ethane (C,H) are put into the "bomb" and similarly completely burned in an excess of oxygen. This time the temperature of the water rises from 13.00 °C to 53.96 °C. chemical reaction "bomb" Use this information, and any other information you need from the ALEKS Data resource, to answer the questions below about this reaction: A "bomb" calorimeter. 2C,H,(g) + 70,(g) 4CO,(g) + 6 H,0 (g) Be sure any of your answers that are calculated from measured data are rounded to the correct number of significant digits. Note for advanced…
Sulfur dioxide, SO2(g), can react with oxygen to produce sulfur trioxide, SO3(g), by the reaction 2 SO2(g) + O2(g) → 2 SO3(g) The standard enthalpies of formation for SO2(g) and SO3(g) are AH; [SO2(g)] = -296.8 kJ/mol AH; [SO3(g)] = -395.7 kJ/mol Calculate the amount of energy in the form of heat that is produced when a volume of 2.25 L of SO2(g) is converted to 2.25 L gas behavior. of SO3(g) according to this process at a constant pressure and temperature of 1.00 bar and 25.0 °C. Assume ideal AH= kJ
A student runs two experiments with a constant-volume "bomb" calorimeter containing 1100. g of water (see sketch at right). thermometer stirrer First, a 5.500 g tablet of benzoic acid (C,H,CO, H) is put into the "bomb" and burned completely in an excess of water oxygen. (Benzoic acid is known to have a heat of combustion of 26.454 kJ/g.) The temperature of the water is observed insulation to rise from 15.00 °C to 42.56 °C over a time of 10.3 minutes. Next, 5.720 g of acetaldehyde (C2H,O} are put into the "bomb" and similarly completely burned in an excess of oxygen. This time the temperature of the water rises from 15.00 °C to 40.53 °C. chemical reaction "bomb" Use this information, and any other information you need from the ALEKS Data resource, to answer the questions below about this reaction: A "bomb" calorimeter. 2C,H,0(g) + 50, (g) 4CO, (g) + 4H,0 (g) Be sure any of your answers that are calculated from measured data are rounded to the correct number of significant digits. Note…
Consider the balanced reaction 4 A + 9 B → 8 C + 8 D and the enthalpies of formation provided in the table below. AH Compound (kJ/mol) A 170.8 231.1 D -98.4 Suppose that the AH of the overall reaction is -2,029.3 kJ/molxn. Calculate the value of the AHf of C in kJ/mol. Report your answer to three decimal places (ignore significant figures).
Using the provided table, determine the enthalpy (in kJ/ mol) for the reaction 2 NH3 (g) + 3 N,0 (g)→ 4 N, (g) + З Н,0 () Substance AH{ (kJ/mol) NH3 (g) -46.2 N20 (g) 81.6 N2 (g) H2O (1) -285.8
Please don't provide handwritten solution ....
Sulfur dioxide, SO, (g), can react with oxygen to produce sulfur trioxide, SO, (g), by the reaction 2 SO, (g) + 0,(g) → 2 SO,(g) The standard enthalpies of formation for SO,(g) and SO, (g) are AH; [SO,() = -296.8 kJ/mol AH; SO,( = -395.7 kJ/mol Calculate the amount of energy in the form of heat that is produced when a volume of 4.10 L of SO, (g) is converted to 4.10 L of SO, (g) according to this process at a constant pressure and temperature of 1.00 bar and 25.0 °C. Assume ideal gas behavior. kJ AL = 18.249 incbrcect