When 1653 J1653 J of heat energy is added to 38.3 g38.3 g of ethanol, C2H6O,C2H6O, the temperature increases by 17.6 ∘C.17.6 ∘C. Calculate the molar heat capacity of C2H6O.

100. mL of 0.100M Ca(OH)2(aq) at 25.0 °C is combined with 100. mL of 0.100M HCl(aq) at 25.0 °C in a constant-pressure calorimeter. Given that the complete neutralization of 1.00 mol of Ca(OH)2 with HCl has ∆H = -110. kJ, and that the specific heat capacity and density of the resulting solution is ~equal to that of water, what is the temperature of the final solution?

A 1.655 g1.655 g sample of a new organic material is combusted in a bomb calorimeter. The temperature of the calorimeter and its contents increase from 24.99 ∘C24.99 ∘C to 29.70 ∘C.29.70 ∘C. The heat capacity (calorimeter constant) of the calorimeter is 41.47 kJ/ ∘C,41.47 kJ/ ∘C, what is the heat of combustion per gram of the material?

4b. Combustion of 3.500 g of butane gas (C4H10; Mm = 58.12 g/mol) causes a temperature rise (AT) of 29.09°C in a constant-pressure calorimeter that has a heat capacity (C,) of 5.500 kJ/°C. o Use calorimetry to calculate the heat (q,) released by the combustion of 3.500 g of butane gas in the calorimeter Яр [ Select ] kJ / 3.500 g of C4H10 o Use the heat (qp) released by the combustion of 3.500 g of butane gas, calculated in part (a) to calculate the change in enthalpy (AHrxn) for the following reaction. (for 1 mole of butane gas): C4H10(9) + 13/2 02(9) → 4 CO2(9) + 5 H20(g) AHrxn [ Select ] kJ / mol of C4H10 • Use the heats of formation (AH¢°) to calculate the change in enthalpy (AHrxn) for the same reaction. (for 1 mole of butane gas): Heats of Formation: CO2 (g) - A H°f = -393.5 kJ/mol H2O(g) - A H°f = -241.8 kJ/mol O2 (9) - A H°f 0.0 kJ/mol C4H10 (g) - A H°f = -125.6 kJ/mol C4H10(g) + 13/2 02(g) → 4 CO2(9) + 5 H20(g) ΔΗη [ Select ] kJ / mol of C4H10

Part B 2.0000 g of the unknown compound is burned in a bomb calorimeter. During the combustion, the temperature of the calorimeter increases from 23.125°C to 28.997 °C. During calibration, the heat capacity of the calorimeter was found to be 9.9897kJ °C-1. In the previous experiment, the molar mass of the substance was found to be 148.16 gmol-1. What is AcombU for the unknown compound? να ΑΣφ ? kJ mol1 Submit Request Answer

The molar heat capacity at constant pressure for CO2 is 36.61 J mol-1 K-1. How much heat in J is to be released in order to lower the temperature of a 35.99 g sample by 20.71 K. Atomic Mass of CO2: 44.01 g/mol.

When 1.720×103 J1.720×103 J of heat energy is added to 36.9 g36.9 g of ethanol, C2H6O,C2H6O, the temperature increases by 19.0 ∘C.19.0 ∘C. Calculate the molar heat capacity of C2H6O. (Answer should be in mol X degrees C)

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 1.1250 g sample of β-D-fructose (C6H12O6) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1.200×103 g of water. During the combustion the temperature increases from 23.58 to 26.40 °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 979.8 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

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What is the specific heat capacity of a substance of mass 159.5 g that increases in temperature from 22.2 °C to 25.2 °C after absorbing 1.15 kJ of energy in the form of heat? Express your answer in J g-1 °C-1. Do not try to identify the substance.