Q.30. Determine, at 298 K, A,„H°, the standard enthalpy of the reaction (1) between dinitrogen tetraoxide and hydrazine: (1) N,O, (g) + 2 N,H, (1) à 3 N, (g) + 4 H,O (g) Knowing the standard reaction enthalpies, at 298 K, of the following reactions: (2) NH3 (g)à 1/2 N, (g) + 3/2 H, (g) ; A„H° = + 46,19 kJ . mol (3) N,O, (g) à 2 NO, (g) ; A„H° =+ 58,04 kJ . mol (4) 2 NH; (g) à N,H (1) + H, (g) ; A,„H° = + 142,80 kJ . mol- (5) 2 NO, (g) + 4 H, (g) à N, (g) + 4 H,O (g) ; A;gH° = – 1 033,66 kJ . mol 1

Q.30. Determine, at 298 K, A,„H°, the standard enthalpy of the reaction (1) between dinitrogen tetraoxide and hydrazine: (1) N,O, (g) + 2 N,H, (1) à 3 N, (g) + 4 H,O (g) Knowing the standard reaction enthalpies, at 298 K, of the following reactions: (2) NH3 (g)à 1/2 N, (g) + 3/2 H, (g) ; A„H° = + 46,19 kJ . mol (3) N,O, (g) à 2 NO, (g) ; A„H° =+ 58,04 kJ . mol (4) 2 NH; (g) à N,H (1) + H, (g) ; A,„H° = + 142,80 kJ . mol- (5) 2 NO, (g) + 4 H, (g) à N, (g) + 4 H,O (g) ; A;gH° = – 1 033,66 kJ . mol 1

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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For the reaction 2N₂(g) + O2(g) → 2N₂O(g) AG = 214 kJ and AS = -148.5 J/K at 334 K and 1 atm. This reaction is product favored under standard conditions at 334 K. The standard enthalpy change for the reaction of 1.51 moles of N₂ (9) at this temperature would be For the reaction 2H₂O(1)→ 2H₂(g) + O₂(g) AG=483 kJ and AH = 572 kJ at 273 K and 1 atm. This reaction is reactant favored under standard conditions at 273 K. The entropy change for the reaction of 2.18 moles of H₂O(1) at this temperature would be kl. J/K.
Calculate the enthalpy change that occurs when 3.20 g of SnCl4 (1) reacts with excess H₂O(l) to form SnO₂ (s) and HCl(aq). Use the following enthalpies of formation: AfH (kJ/mol) Compound HCl(aq) H₂O(l) SnCl4 (l) SnO₂ (s) Enthalpy change = -167.159 -285.83 -511.3 -577.63 kJ
(2B) A heat engine operates between a hot source at 130.°C and a cold sink at 10.°C. How much workcan be done by the engine if 523 kJ of heat are extracted from the hot source?
D
The standard enthalpies of formation of ions in aqueous solutions are obtained by arbitrarily assigning a value of zero to H* ions; that is, AH H* (aq)]=0. H₂O HC1 (g) →H (aq) + Cl¯ (aq) Note: Reference the Thermodynamic properties of pure substances table for additional information. Part 1 of 2 For the following reaction, calculate AH, for the CI ions. Round your answer to 4 significant digits. Part 2 of 2 □ 0x10 X □ 0.0 kJ ΔΗ% = -14.7 mol S Calculate the enthalpy of neutralization when 1 mole of a strong monoprotic acid (such as HCI) is titrated by 1 mole of a strong base (such as KOH) at 25 °C. Round your answer to 3 significant digits. 010
Q.29. Determine, at 298 K, ArH°, the standard enthalpy of the reaction (1) between dinitrogen tetraoxide and hydrazine: (1) N2O4 (g) + 2 N2H4 (1) → 3 N2 (g) +4 H2O (g) Knowing the standard reaction enthalpies, at 298 K. of the following reactions: (2) NH3 (g)→ 1/2 N2 (g) + 3/2 H2 (g) AnH° = + 46,19 kJ . mol (3) N204 (g) → 2 NO2 (g), Ar3H = + 58,04 kJ : mol (4) 2 NH3 (g) → N2H (1) + H2 (g) Ar4H° = (5) 2 NO2 (g) + 4 H2 (g) → N2 (g) + 4 H2O (g) ArsH° = – 1 033,66 kJ. mol 142,80 kJ .mol- %3D
PCI5(s) can be prepared by the reaction PCI3(1) + Cl2(g) - PCI5(s). Calculate the enthalpy change (in kJ) that accompanies the production of 100.0 g of PCI5(s) by the above reaction, given the following data. P4(s) + 6 Cl2(g) - 4 PC|3(1) AH° = -1280 kJ per mole of P4(s) %3D P4(s) + 10 Cl2(g) – 4 PCI5(s) ΔΗ AH° = -1774 kJ per mole of P4(s) +59.3 -59.3 +124 -124 -258
15. Using the standard enthalpies of formation for the chemicals involved, calculate the enthalpy change for the following reaction. (Note: Show the math clearly and provide units in your setup) (AH; Values in kJ/mol are as follows: NO, +32, H,0 -286, HNO3 -207, NO +90) 3NO2(8) + H,Oy O 2HNO3(aq) + NO(g) (g),
Q.30. Determine, at 298 K, Δr1H0, the standard enthalpy of the reaction (1) between dinitrogen tetraoxide and hydrazine: (1) N2O4 (g) + 2 N2H4 (l) à 3 N2 (g) + 4 H2O (g) Knowing the standard reaction enthalpies, at 298 K, of the following reactions: (2) NH3 (g)à 1/2 N2 (g) + 3/2 H2 (g) ; Δr2H0 = + 46,19 kJ . mol–1 (3) N2O4 (g) à 2 NO2 (g) ; Δr3H0 = + 58,04 kJ . mol–1 (4) 2 NH3 (g) à N2H (l) + H2 (g) ; Δr4H0 = + 142,80 kJ . mol–1 (5) 2 NO2 (g) + 4 H2 (g) à N2 (g) + 4 H2O (g) ; Δr5H0 = – 1 033,66 kJ . mol–1
molar enthalpy of formation of H2O(l) from its elements in their standard states (25 oC and 100 kPa)?
The standard heat of formation, AH;, is defined as the enthalpy change for the formation of one mole of Part B substance from its constituent elements in their standard states. Thus, elements in their standard states have AH: = 0. Heat of formation values can be used The combustion of ethene, C2H4, occurs via the reaction to calculate the enthalpy change of any reaction. C2H4 (g) + 302 (g)→2CO2(g) + 2H20(g) Consider, for example, the reaction with heat of formation values given by the following table: 2NΟ (5) + Ο, (s) 2ΝO, (g) ΔΗρ (kJ/mol) Substance with heat of formation values given by the following table: C2H4 (g) 52.47 CO2 (g) -393.5 Substance (kJ/mol) H2O(g) -241.8 NO(g) 90.2 Calculate the enthalpy for the combustion of ethene. 02 (g) Express your answer to four significant figures and include the appropriate units. NO2(g) 33.2 • View Available Hint(s) Then the heat of formation for the overall reaction is ΔΗ ΔΗ (products) -ΔΗ; (reactants ) [2(90.2) + 0] HA ? 2(33.2) -114 kJ/mol…