26. Nitroglycerin, C;H5(NO3)3(1), is an explosive most often used in mine or quarry blasting. It is a powerful explosive because four gases (N2, O2, CO2, and steam) are formed when nitroglycerin is detonated. In addition, 6.26 kJ of heat are given off per gram of nitroglycerin detonated. (a) Write a balanced thermochemical equation for the reaction. (b) What is AH when 4.65 mol of products are formed?

26. Nitroglycerin, C;H5(NO3)3(1), is an explosive most often used in mine or quarry blasting. It is a powerful explosive because four gases (N2, O2, CO2, and steam) are formed when nitroglycerin is detonated. In addition, 6.26 kJ of heat are given off per gram of nitroglycerin detonated. (a) Write a balanced thermochemical equation for the reaction. (b) What is AH when 4.65 mol of products are formed?

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

A bomb calorimetry experiment is performed with xylose, CsH10Os (s), as the combustible substance. The data obtained are: mass of xylose burned: 1.764g; heat capacity of calorimeter: 4.728 kJ/°C; initial calorimeter temperature: 23.29°C; final calorimeter temperature 27.19°C. What is the heat of combustion of xylose, in kilojoules per mole? Lütfen birini seçin: O a.-1.57x10 kJ/mol O b.-5.64x10 kJ/mol O c.-3.17x10 kJ/mol O d -3.34x10 kJ/mol O e. -2.38x10 kJ/mol
thermochemical equations as needed to find the heat of formation of diamond:
7.) Use the following thermochemical equations as needed to find the heat of formation of diamond: C(diamond) + O;(g) →CO;(g) AH = -395.4 kJ %3D 2 CO:(g) → 2 CO(g) + O; (g) AH = 566.0 kJ C(graphite) + O;(g)→ CO:(g) AH = -393.5 kJ 2 CO(g)→ C(graphite) + CO,(g) AH = -172.5 kJ %3D
A bomb calorimeter, or a constant volume calorimeter, is a device often used to determine the heat of combustion of fuels and the energy content of foods. In an experiment, a 1.5880 g sample of fumaric acid (C4H404) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1.380x10³ g of water. During the combustion the temperature increases from 21.68 to 24.27 °C. The heat capacity of water is 4.184 ) g1c¹. The heat capacity of the calorimeter was determined in a previous experiment to be 954.8 J/°C. Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of fumaric acid based on these data. C₂H4O4(s) + 30₂(g) 2 H₂O(1) + 4 CO₂(g) + Energy Molar Heat of Combustion = kJ/mol
metal X =48.1g; specific heat capacity =0.228 J/C If metal X is heated to 95.1C and put into a calorimeter containing water (she=4.18 J/g°C ) at 22.3C. The final temperature of the water becomes 31C. What is the mass of water?
How many joules of energy would be required to raise the temperature of 3.2 grams of mercury 4.2ºC? The specific heat of mercury is 0.14 J/(g·ºC).
Consider the hypothetical thermochemical equation 3 A+B 2 C for which AH = 84.3 kJ/mol. If you have 5.30 moles of A, what quantity of heat, in kJ, would be absorbed?
Q1
A bomb calorimeter, or a constant volume calorimeter, is a device often used to determine the heat of combustion of fuels and the energy content of foods. In an experiment, a 1.0220 g sample of β-D-fructose (C6H12O6) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1.186×103 g of water. During the combustion the temperature increases from 26.62 to 29.46 °C. The heat capacity of water is 4.184 J g-1°C-1.The heat capacity of the calorimeter was determined in a previous experiment to be 906.4 J/°C.Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of β-D-fructose based on these data.C6H12O6(s) + 6O2(g) 6 H2O(l) + 6 CO2(g) + EnergyMolar Heat of Combustion = kJ/mol
What is q of H2O?
Octane (CgH18) is a component of gasoline and combusted according to the reaction below. Is the reaction exothermic or endothermic and what is the change in heat energy if 34.5 g of octane is combusted with excess oxygen? (Note: the molar mass of octane is 114.2 g/mol) 2C3H18 (1) + 2502 (g) → 16CO2 (g) + 18H2O (g) AH= -10860 kJ endothermic, -3280 kJ exothermic, -10860 kJ O exothermic, -3280 kJ O endothermic, -1640 kJ exothermic, -1640 kJ df journal.part3 (1).docx journal.part3.docx to search
Unit 10 Q#17 When a 25.0 g sample of ethyl alcohol is burned, how much energy is released as heat? C,H̟OH(1) + 30,(g) 2 '5 O 2 CO,(g) + 3 H,() AHrxn = - 1.37 x 103 kJ/mol