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of 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 0.3514 g sample of phenanthrene (C₁4H10) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1.072x10³ g of water. During the combustion the temperature increases from 26.05 to 28.56 "C. The heat capacity of water is 4.184 3 g ¹0c-1. The heat capacity of the calorimeter was determined in a previous experiment to be 811.9 3/°C. Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of phenanthrene based on these data. C14H10(s) + (33/2) O₂(g) 5 H₂O(1) + 14 CO₂(g) + Energy Molar Heat of Combustion - kJ/mol
1 pt 1 pt 1 pt 1 pt 1 pt 1 pt dpt pt Given the standard enthalpy changes for the following two reactions: (1) 4C(s) + 5H₂(9) C4H10(9) AH = -125.6 kJ (2) C₂H₂(g)2C(s) + H₂(g) AH = -226.7 kJ what is the standard enthalpy change for the reaction: (3) 2C₂H₂(g) + 3H₂(9) C4H10 (9) AH° = ? kJ
Using standard heats of formation, calculate the standard enthalpy change for the following reaction.. 2H₂O(1) 2H₂(g) + O₂(g) ANSWER: k3
A scientist measures the standard enthalpy change for the following reaction to be 35.9 k CO₂(g) + H₂(g)CO(g) + H₂O(g) K3/mol Based on this value and the standard enthalpies of formation for the other substances, the standard enthalpy of formation of CO(9) is
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