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In an experiment, a 0.4117 g sample of heptadecanoic acid (C17H34O2) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1.205!10^3 g of water. During the combustion the temperature increases from 22.81 to 25.38 °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 943.3 J/°C. Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of heptadecanoic acid based on these data. C17H34O2(s) + (49/2) O2(g) → 17 H2O(l) + 17 CO2(g) + Energy Molar Heat of Combustion = kJ/mol Combustion (bomb) calorimeter.

          In an experiment, a 0.4117 g sample of heptadecanoic acid (C17H34O2) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1.205!10^3 g of water. During the combustion the temperature increases from 22.81 to 25.38 &#176;C. The heat capacity of water is 4.184 J g^-1&#176;C^-1. The heat capacity of the calorimeter was determined in a previous experiment to be 943.3 J/&#176;C. Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of heptadecanoic acid based on these data. C17H34O2(s) + (49/2) O2(g) &#8594; 17 H2O(l) + 17 CO2(g) + Energy Molar Heat of Combustion = kJ/mol Combustion (bomb) calorimeter.

In an experiment, a 0.4117 g sample of heptadecanoic acid (C17H34O2) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1.205!10^3 g of water. During the combustion the temperature increases from 22.81 to 25.38 #176;C. The heat capacity of water is 4.184 J g^-1 #176;C^-1. The heat capacity of the calorimeter was determined in a previous experiment to be 943.3 J/ #176;C. Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of heptadecanoic acid based on these data. C17H34O2(s) + (49/2) O2(g) #8594; 17 H2O(l) + 17 CO2(g) + Energy Molar Heat of Combustion = kJ/mol Combustion (bomb) calorimeter.

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