Nitroglycerin (C3H5N3O9), a liquid at room temperature (25 °C) and atmospheric pressure (1.01325 x 105 Pa), is used to relieve angina. It may undergo decomposition under these same conditions to form nitrogen, carbon dioxide, oxygen and water, with an enthalpy of decomposition of -1541 kJ mol-¹. The standard enthalpies of formation of water and carbon dioxide are -285.9 and -393.5 kJ mol-1 respectively. (a) Write a balanced equation for the decomposition of nitroglycerin.

Nitroglycerin (C3H5N3O9), a liquid at room temperature (25 °C) and atmospheric pressure (1.01325 x 105 Pa), is used to relieve angina. It may undergo decomposition under these same conditions to form nitrogen, carbon dioxide, oxygen and water, with an enthalpy of decomposition of -1541 kJ mol-¹. The standard enthalpies of formation of water and carbon dioxide are -285.9 and -393.5 kJ mol-1 respectively. (a) Write a balanced equation for the decomposition of nitroglycerin.

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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Nitroglycerin (C3H5N3O9), a liquid at room temperature (25 oC) and atmospheric pressure (1.01325 x 105 Pa) is used to relieve angina. It may undergo decomposition under these same conditions to form nitrogen, carbon dioxide, oxygen and water, with an enthalpy of decomposition of -1541 kJ mol-1.The standard enthalpies of formation of water and carbon dioxide are -285.9 kJ mol-1 and -393.5 kJ mol-1 respectively. Determine the standard enthalpy of formation of 1.0 mole of nitroglycerin.
Determine, at 298 K, AraH°, the standard enthalpy of the reaction (1) between dinitrogen tetraoxide and hydrazine: (1) N204 (g) + 2 N2H4 (I) 3 N2 (g) + 4 H2O (g) Knowing the standard reaction enthalpies, at 298 K, of the following reactions: (2) NH: (g) 1/2 N2 (g) + 3/2 H2 (g) ; A-2Hº = + 46,19 kl . mol1 (3) N204 (g) 2 NO2 (g) ; Ar3H° = + 58,04 kJ . mol (4) 2 NH3 (g) N2H (I) + H2 (g) ; A-4H° = + 142,80 kJ. mol1 (5) 2 NO2 (g) + 4 H2 (g) N2 (g) + 4 H2O (g) ; ArsH° = – 1 033,66 kl.mol
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.
To study the possible amount of energy generated by a person, the person can be roughly viewed as a constant pressure calorimeter using table sugar (sucrose, C12H22O11) as the energy generator. The reaction of table sugar in a calorimeter is given by: C12H22O11(s) + 12O2(g) ----------> 12CO2(g) + 11H2O(g) a. What is the heat released by consuming one mole of sugar (C12H22O11) in this way? b. Calculate the enthalpy of combustion per mole of sugar utilization. c. Does the result of your calculation make sense?
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The combustion of 0.150g of ethanol, CHOH(1) 2 5 releases 4.47kJ of heat. The molar enthalpy of combustion of liquid is?
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
The enthalpy of combustion of benzoic acid (C,H,COOH) is commonly used as the standard for calibrating constant-volume bomb calorimeters; its value has P mol been accurately determined to be -3226.7 - When 2.5311 g of benzoic acid are burned in a calorimeter, the temperature rises from 20.84 °C to 26.67 °C. What is the heat capacity of the bomb? (Assume that the quantity of water surrounding the bomb is exactly 2250 g) Round your answer to 3 significant digits. Note: Reference the Phase change properties of pure substances table for additional information. 0-/2 0.8 X 5 8 @ al P
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…