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
To determine the calorimeter constant of a coffee-cup calorimeter, 28 g of cold water was placed in the calorimeter. The initial temperature of the cold water and the calorimeter is 19.5ºC. A 28 g of hot water (initially at 62.2ºC) was placed in the calorimeter with cold water. Determine the experimental calorimeter constant, Ccal, if the final temperature after mixing is 37ºC. Use Cp of water = 4.184 J/gºC. Express your answer in 2 decimal places. Round your answer to 2 decimal places.
Johnson and Steele determined the standard enthalpy of combustion of UO2(s) in gaseous fluorine. The products of combustion are UF6(s) and O2(g). The measured value of the enthalpy of combustion is -1112.6 kJ mol-¹ (per mole of UO₂), and the standard enthalpy of formation of UF6(s) is -2197.7 kJ mol-¹. Calculate the standard enthalpy of formation of UO2(s) in kJ mol-¹.
Determine the change in standard enthalpy, in units of kJ mol-1, for the following reaction: C(s, graphite) + 2 H2(g) + ½ O2(g) CH3OH() A,H = ? using the following reaction data: C(s, graphite) + O2(g) CO2(g) ArH = -393.5 kJ mol-1 H2(g) + ½ O2(g) H20() A,H = -285.8 kJ mol-1 2 CH3OH() + 3 O2(g) → 2 CO2(g) + 4 H20() A,H = -1452.8 kJ mol-1
Calculate the standard enthalpies of combustion at 25°C CAH8 cg) + H2cg) -7 C4 H10 (g) Of AH = -2878.6 KJ
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?
Johnson and Steele determined the standard enthalpy of combustion of UO₂(s) in gaseous fluorine. The products of combustion are UF(s) and O2(g). The measured value of the enthalpy of combustion is -1112.6 kJ mol-¹ (per mole of UO₂), and the standard enthalpy of formation of UF(s) is -2197.7 kJ mol-¹. Calculate the standard enthalpy of formation of UO2(s) in kJ mol-¹.
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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