How much combined energy is required to raise 25.0 g of liquid CCl4 from 0.0 °C to 76.8 °C and then convert it from a liquid to a gas? Group of answer choices44.0 kJ45.7 kJ42.3 kJ1.7 kJ

To answer this question, we need to know the specific heat capacity of CCl4 (carbon tetrachloride) and its heat of vaporization.

Let's assume the specific heat capacity of CCl4 is 0.861 J/g°C and its heat of vaporization is 30.0 kJ/mol.

Step 1: Calculate the energy required to raise the temperature of CCl4 from 0.0 °C to 76.8 °C.

The formula to calculate the heat (q) required to change the temperature (ΔT) of a certain amount of a substance with a specific heat capacity (c) is q = mcΔT.

So, q1 = (25.0 g) * (0.861 J/g°C) * (76.8°C - 0.0°C) = 1653.3 J = 1.6533 kJ.

Step 2: Calculate the energy required to convert CCl4 from a liquid to a gas.

First, we need to convert the mass of CCl4 to moles. The molar mass of CCl4 is about 153.823 g/mol.

So, moles of CCl4 = 25.0 g / 153.823 g/mol = 0.1625 mol.

The heat (q) required to convert a substance from a liquid to a gas is calculated by q = nΔHvap, where n is the number of moles and ΔHvap is the heat of vaporization.

So, q2 = (0.1625 mol) * (30.0 kJ/mol) = 4.875 kJ.

Step 3: Add the energy required for both steps to get the total energy required.

Total energy = q1 + q2 = 1.6533 kJ + 4.875 kJ = 6.5283 kJ.

However, none of the provided answer choices match this result. Please check the values provided in the question.