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What amount of heat (in kJ) is required to convert 14.0 g of an unknown liquid (MM = 67.44 g/mol) at 43.5 °C to a gas at 128.2 °C?

- Specific heat capacity of the liquid: 1.18 J/g･°C
- Specific heat capacity of the gas: 0.792 J/g･°C
- ∆Hvap = 30.1 kJ/mol
- Normal boiling point, [tex]T_b[/tex] = 97.4 °C

Answer :

The amount of heat (in kJ) is required to convert 14. 0 g of an unknown liquid

The given data

mass = 14. 0 g

MM = 67. 44 g/mol)

specific heat capacity of liquid = 1. 18 J/g･°C

specific heat capacity of gas = 0. 792 J/g･°C

∆H vap = 30. 1 kJ/mol

Tb = 97. 4°C

The amount of heat will determined by using the formula

Q = MCΔT

Put the value of given data in above equation.

Q = 14. 0 g × 0. 792 J/g･°C × 97. 4°C

Q = 1079 jule/ 1.079 kJ

the amount of heat needed to raise a substance's temperature by one degree Celsius in one gramme, also known as specific heat. Typically, calories as well as joules per gram per degree Celsius are used as the measures of specific heat.

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