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The heat of combustion of liquid C2H60 is -1460.4 kJ/mol at 298K. Thermodynamic tables Note, tolerance...
At constant volume, the heat of combustion of a particular compound is −3796.0 kJ/mol.−3796.0 kJ/mol. When 1.277 g1.277 g of this compound (molar mass=107.98 g/mol)(molar mass=107.98 g/mol) was burned in a bomb calorimeter, the temperature of the calorimeter, including its contents, rose by 4.263 ∘C.4.263 ∘C. What is the heat capacity (calorimeter constant) of the calorimeter?
the combustion of 1.00 mol of glucose, C6H12O6, releases 2820 kJ of heat. If 2.0g of glucose is burned in a calorimeter containing 1.0 kg of water, and the temperature increases by 3.5°C, what is the heat capacity of the calorimeter?
Determine the heat of combustion of sucrose (C12H22O11) in kJ/mol if 2.00g of sucrose is burned in a bomb calorimeter, and the temperature of the calorimeter rose from 25.33C to 28.17C. The heat capacity of the calorimeter is 11.6kJ/C.
At constant volume, the heat of combustion of a particular compound, compound A, is −3294.0 kJ/mol. When 1.127 g of compound A (molar mass = 109.35 g/mol) is burned in a bomb calorimeter, the temperature of the calorimeter (including its contents) rose by 7.283 °C. What is the heat capacity (calorimeter constant) of the calorimeter? Suppose a 3.157- g sample of a second compound, compound B, is combusted in the same calorimeter, and the temperature rises from 23.23 °C to...
The heat of combustion of liquid cumene (C9H12) is -5215.5 kJ/mol at 1 atm and 298 K a) What is the energy of combustion at 1 atm and 298 K? Ecomb = kJ/mol b) Use Thermodynamic Properties to determine its heat of formation. Hf = kJ/mol
The heat of combustion of octane is -5430 kJ/mol. 1.000 g sample of octane (C8H18) is burned in a bomb calorimeter at an initial temperature of 25.00ºC. The heat capacity of the calorimeter (also known as the “calorimeter constant”) is 837 J/ºC. Calculate E for the combustion of octane. (You will need a balanced chemical equation to find H) What is the final temperature of the calorimeter?
At constant volume, the heat of combustion of a particular compound is -3952.0 kJ/mol. When 1.211 g of this compound (molar mass = 130.08 g/mol) was burned in a bomb calorimeter, the temperature of the calorimeter (including its contents) rose by 4.453 ◦C. What is the heat capacity (calorimeter constant) of the calorimeter?-qrxn = qcalorimeterWhat is the formula for heat (q) for the calorimeter?___________________Did the calorimeter absorb/release heat? Circle your answer.Calculate the energy absorbed by the calorimeter.Solve:
7A) Butane has a heat of combustion of -2882 kJ/mol. If a 10.09 g sample of butane is burned in a bomb calorimeter containing 2.610 kg of water initially at 20.13 degrees C, find the final water temperature. 7B) A sample of ethanol (CH3CH2OH) increases the temperature of the bomb calorimeter in Question 7A by 4.71 degrees C. If the heat of combustion of ethanol is -1407 kJ/mol, what was the mass of the ethanol sample? I only need the...
The heat liberated by the combustion of glutaric acid is 2154 KJ/mol. A 1.50 g sample of glutaric acid is burned in excess O2(g) in a calorimeter that contains 1250 g of water. The temperature of the calorimeter and its contents increases from 20.00C to 23.69 C. What is the heat capacity of the calorimenter (J/C)?
When 1.034g of naphthalene (C10H8) is burned in a constant-volume bomb calorimeter at 298K, 41.56 kJ of heat is evolved. Calculate the change in U and w for the reaction on a molar basis.