Question

Calculate the heat required to convert 25. 0g of C2Cl3F3 from a liquid at 5. 00°C to a gas at 82. 00°C. M. M. C2Cl3F3 = 187. 364 g/mol; boiling point = 47. 60°C; Cp liquid = 0. 91 J/g-K; Cp gas = 0. 67 J/g-K; △Hvap = 3. 667 kJ/g

Answer 1

Answer:
To calculate the heat required, we need to consider the heat needed to raise the temperature of the liquid from 5.00°C to its boiling point at 47.60°C, the heat required for the phase change from liquid to gas (vaporization), and the heat needed to raise the temperature of the gas from the boiling point to 82.00°C.

Step-by-step explanation:
1. Heat required to raise the temperature of the liquid from 5.00°C to its boiling point at 47.60°C:
- Mass of C2Cl3F3 = 25.0g
- Specific heat capacity of the liquid (Cp liquid) = 0.91 J/g-K
- Temperature change (ΔT) = 47.60°C - 5.00°C = 42.60°C
- Heat required = mass * Cp * ΔT

2. Heat required for the phase change from liquid to gas (vaporization):
- Mass of C2Cl3F3 = 25.0g
- Heat of vaporization (ΔHvap) = 3.667 kJ/g
- Heat required = mass * ΔHvap

3. Heat required to raise the temperature of the gas from the boiling point to 82.00°C:
- Mass of C2Cl3F3 = 25.0g
- Specific heat capacity of the gas (Cp gas) = 0.67 J/g-K
- Temperature change (ΔT) = 82.00°C - 47.60°C = 34.40°C
- Heat required = mass * Cp * ΔT

To find the total heat required, sum up the heat required from each step.

Answer 2

The heat required to convert 25.0 g of C2Cl3F3 from a liquid at 5.00°C to a gas at 82.00°C can be calculated as follows:

1. The heat required to raise the temperature of the liquid from 5.00°C to 47.60°C is:

```

heat_liquid = 25.0 g * 0.91 J/g-K * (47.60°C - 5.00°C) = 948.5 J

```

2. The heat of vaporization of C2Cl3F3 is:

```

heat_vaporization = 25.0 g * 3.667 kJ/g = 91.675 kJ

```

3. The heat required to raise the temperature of the gas from 47.60°C to 82.00°C is:

```

heat_gas = 25.0 g * 0.67 J/g-K * (82.00°C - 47.60°C) = 338.5 J

```

4. The total heat required is the sum of the three heats calculated above:

total_heat = heat_liquid + heat_vaporization + heat_gas = 948.5 J + 91.675 kJ + 338.5 J = 1378.675 kJ

Therefore, the heat required to convert 25.0 g of C2Cl3F3 from a liquid at 5.00°C to a gas at 82.00°C is 1378.675 kJ.