When 2.25 mg of anthracene, C₁4H₁0(s), was burned in a bomb calorimeter the temperature rose by 1.75K. Calculate the calorimeter constant. By how much will the temperature rise when 125 mg of phenol, C6H5OH(s) is burned in the calorimeter under the same conditions? AH combustion (anthracene) = -7061 kJ/mol

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When 2.25 mg of anthracene, C₁4H10(s), was burned in a bomb calorimeter the temperature
rose by 1.75K. Calculate the calorimeter constant. By how much will the temperature rise
when 125 mg of phenol, C6H5OH(s) is burned in the calorimeter under the same conditions?
AH combustion (anthracene) = -7061 kJ/mol
Transcribed Image Text:When 2.25 mg of anthracene, C₁4H10(s), was burned in a bomb calorimeter the temperature rose by 1.75K. Calculate the calorimeter constant. By how much will the temperature rise when 125 mg of phenol, C6H5OH(s) is burned in the calorimeter under the same conditions? AH combustion (anthracene) = -7061 kJ/mol
Expert Solution
Step 1: List the Given Data

The mass of anthracene is straight m equals 2.25 space mg equals 0.00225 space straight g.

The change in temperature is 1.75 K.

To find the calorimeter constant.

The heat of combustion is increment straight H subscript combustion equals negative 7061 space kJ divided by mol.

To calculate the temperature rise when the mass of phenol is 125 that is burned in the same bomb calorimeter.

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