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) + Energy Molar Heat of Combustion =    kJ/mol

An electrical heater is used to add 19.75 kJ of heat to a constant-volume calorimeter. The temperature of the calorimeter increases by 4.76°C. When 2.00 g of methanol (CH3OH) is burned in the same calorimeter, the temperature increases by 10.92°C. Calculate the molar heat of combustion for methanol (in kJ).

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 0.8608 g sample of glutaric acid (C3HgO4) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1.029x103 g of water. During the combustion the temperature increases from 25.01 to 27.84 °C. The heat capacity of water is 4.184 J gl°c-!. The heat capacity of the calorimeter was determined in a previous experiment to be 839.5 J°C. Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of glutaric acid based on these data. C;HgO4(s) + 50,(g) 4 H,O(1) + 5 CO,(g) + Energy Molar Heat of Combustion = kJ/mol

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 1.4710 g sample of maleic acid (C4H4O4) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1159 g of water. During the combustion the temperature increases from 22.46 to 25.59 °C.   The heat capacity of the calorimeter, not including the surrounding water, was determined in a previous experiment to be 852.2 J/°C.   Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of maleic acid based on these data.   Assuming that no energy is lost to the surroundings, what is the molar heat of combustion of maleic acid, based on these data? (in kJ/mol).   C4H4O4(s) + 3O2(g) → 2 H2O(l) + 4 CO2(g) + Energy

When 0.0901 mol of an unknown hydrocarbon is burned in a bomb calorimeter, the calorimeter increases in temperature by 2.19°C. If the heat capacity of the bomb calorimeter is 1.229 kJ/°C, what is the heat of combustion for the unknown hydrocarbon?

When 1.836 grams of sucrose (Molar mass 342.3 g/mol) is burned in a bomb calorimeter, the temperature of the calorimeter increases from 22.41°C to 26.63°C. If the heat capacity of the calorimeter is 4.900 kJ/°C, what is the heat of combustion of sucrose?

Solid calcium chloride dissolves in water according to the equation below.CaCl2 (s) ➝ Ca+2 (aq) + 2 Cl – (aq)      ΔHº = –81.3 kJ/mol8.00 grams of solid CaCl2 dissolves in 45.0 grams of water initially at a temperature of 20.00 ºC in a perfect calorimeter. Calculate the final temperature of the solution in the calorimeter.[You may assume that no heat escapes the calorimeter and that all solutions have the same specific heat capacity as pure water (4.184 J/g·ºC)]Tfinal = Answer ºC

When a solid dissolves in water, heat may be evolved or absorbed. The heat of dissolution (dissolving) can be determined using a coffee cup calorimeter. In the laboratory a general chemistry student finds that when 0.79 g of KOH(s) are dissolved in 104.10 g of water, the temperature of the solution increases from 24.69 to 26.63 °C. The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.58 J/°C. Based on the student's observation, calculate the enthalpy of dissolution of KOH(s) in kJ/mol. Assume the specific heat of the solution is equal to the specific heat of water. kJ/mol AH dissolution = BrookaCom Cengage Leaming Thermometer Cardboard or Styrofoam lid Nested Styrofoam cups Reaction occurs in solution.

When a solid dissolves in water, heat may be evolved or absorbed. The heat of dissolution (dissolving) can be determined using a coffee cup calorimeter. In the laboratory a general chemistry student finds that when 3.95 g of CuCl2(s) are dissolved in 108.60 g of water, the temperature of the solution increases from 23.05 to 26.27 °C. The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.86 J/°C. Based on the student's observation, calculate the enthalpy of dissolution of CuCl,(s) in kJ/mol. Assume the specific heat of the solution is equal to the specific heat of water. AHdissolution kJ/mol