A 17.5g sample of a candy bar is burned in a bomb calorimeter. which has a...
8. A 1.0 gram sample of a candy bar was placed in a bomb calorimeter with a heat capacity of 354 kcal/°C. The sample was completely burned, causing the temperature of the calorimeter to rise by 1.36 °C. How many kilocalories of energy were stored in the candy bar?
20. A 1.0 gram sample of a candy bar was placed in a bomb calorimeter with a heat capacity of 3.54 kcal sample was completely burned, causing the temperature of the calorimeter to rise by 1.36°C. How many kilocalories of energy were stored in the candy bar?
A 4.1-g sample of Colorado oil shale is burned in a bomb calorimeter, which causes the temperature of the calorimeter to increase by 5.0 °C. The calorimeter contains 1.00 kg of water (specific heat of water 4.184 J/g°C) and the heat capacity of the empty calorimeter is 0.10 kJ/°C. How much heat is released per gram of oil shale when it is burned? 21 kJ/g 0 kJ/g 0.19 kJ/g 42 kJ/g 5.2 kJ/g
A 1.20-g sample of maleic acid (C4H4O4) is burned in a bomb calorimeter and the temperature increases from 24.70 °C to 27.41 °C. The calorimeter contains 1000 g of water and the bomb has a heat capacity of 839 J/°C. The heat capacity of water is 4.184 J g-1°C-1. Based on this experiment, calculate ΔE for the combustion reaction per mole of maleic acid burned.
A quantity of 1.922 g of methanol (CH3OH) was burned in a constant-volume bomb calorimeter. Consequently, the temperature rose by 5.52°C. If the heat capacity of the bomb plus water was 8.75 kJ / °C, calculate the molar heat of combustion of methanol.
A 0.2075−g sample of solid magnesium is burned in a constant-volume bomb calorimeter that has a heat capacity of 3024 J/°C. The temperature increases by 1.700°C. (a) Calculate the heat given off by the burning Mg in kJ/g. kJ/g (b) Calculate the heat given off by the burning Mg in kJ/mol. kJ/mol
A 0.44 mol sample of a substance is burned in a bomb calorimeter with a heat capacity of 8.87 kJ/C. The temperature increases by 8.36 C. What is ΔHrxn (in kJ/mol) for the combustion of the substance?
Ignition wires heat sample Thermometer Stirrer A bomb calorimeter, or constant volume calorimeter, is a device often used to determine the heat of combustion of fuels and the energy content of foods. Since the "bomb" itself can absorb energy, a separate experiment is needed to determine the heat capacity of the calorimeter This is known as calibrating the calorimeter In the laboratory a student burns a 0.319-g sample of phenanthrene (C14H10 in a bomb calorimeter containing 1070. g of water....
. (15. A 1.600g sample of quinone (C6H,02) was burned in a bomb calorimeter whose total heat capacity is 7.854 kJ/°C. The temperature of the calorimeter increases from 21.34 °C to 32.57 °C. What is the heat of combustion per gram of quinone? Per mole of quinone? (10 pts.)
A sample gives off 2,026 J when burned in a bomb calorimeter. The temperature of the calorimeter increases by 3.73ºC. Calculate the heat capacity of the calorimeter in kJ/ºC.