Answer :
The energy used in the distillation of 20 g of acetic acid from 25°C to 130°C is 14809.76 J.
To calculate the energy used in the distillation of acetic acid, we first need to divide the process into two steps: heating the acetic acid from 25°C to its boiling point (118°C) and then vaporizing it. We'll use the specific heat equation Q = mcΔT to calculate the energy used in heating, and the heat of vaporization equation Q = nΔH to calculate the energy used in vaporization.
First, let's calculate the energy required to heat the acetic acid using the specific heat equation:
Q1 = mcΔT
Q1 = 20g × 2.043 J/g×K × (118°C - 25°C)
Q1 = 1919.76 J
Next, let's calculate the energy required for vaporization:
Convert the mass of acetic acid (20g) to moles: 20g / 60.05 g/mol = 0.333 mol
Q2 = nΔH
Q2 = 0.333 mol × 39.1 kJ/mol
= 12.99 kJ
= 12990 J
The total energy used in the distillation is the sum of Q1 and Q2: 1919.76 J + 12990 J = 14809.76 J
In conclusion, the total energy used in the distillation is the sum of Q1 and Q2 is 14809.76 J
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