Chemistry, 15.07.2019 02:30 maggie123456751

How much heat is required to vaporize 33.8 g of water at 100 ∘c?

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Answer from: AquaNerd5706

The heat required to vaporize 33.8 g of water at ${\text{100 }}^\circ{\text{C}}$ is $\boxed{76.353{\text{2 kJ}}}$ .

Further explanation:

Properties are categorized into two types:

1. Intensive properties:

These properties depend on the nature of the substance and not on the size of the system. If the system is further divided into a number of subsystems, the values of intensive properties remain unchanged. Temperature, refractive index, molarity, concentration, pressure, and density are some of the examples of intensive properties.

2. Extensive properties:

These properties depend on the amount of the substance. These are additive in nature if a single system is divided into several subsystems. Mass, heat, enthalpy, volume, energy, size, weight, and length are some of the examples of extensive properties.

Heat of vaporization:

It is the amount of heat that is needed to convert a unit mass of the liquid into its vapors. It is also known as the enthalpy of vaporization or heat of evaporation. It is represented by $\Delta {H_{{\text{vap}}}}$ . Its unit is kJ/mol or J/mol.

The formula to calculate the moles of water is as follows:

${\text{Moles of water}}=\frac{{{\text{Given mass of water}}}}{{{\text{Molar mass of water}}}}$ …… (1)

The given mass of water is 33.8 g.

The molar mass of water is 18.01 g/mol.

Substitute these values in equation (1).

$\begin{aligned}{\text{Moles of water}}&=\left({{\text{33}}{\text{.8 g}}}\right)\left({\frac{{{\text{1 mol}}}}{{{\text{18}}{\text{.01 g}}}}}\right)\\&=1.87{\text{6 mol}}\\\end{aligned}$

The heat of vaporization of water at ${\text{100 }}^\circ{\text{C}}$ is 40.7 kJ/mol. This implies 40.7 kJ of energy is required to convert 1 mole of water into vapors. So the heat required to convert 1.876 moles of water is calculated as follows:

$\begin{aligned}{\text{Heat required}}&=\left( {{\text{1}}{\text{.876 mol}}}\right)\left({\frac{{{\text{40}}{\text{.7 kJ}}}}{{{\text{1 mol}}}}}\right)\\&=76.353{\text{2 kJ}}\\\end{aligned}$

Therefore the heat required to vaporize 33.8 g of water at ${\text{100 }}^\circ{\text{C}}$ is 76.3532 kJ.

Learn more:

1. Calculate the enthalpy change using Hess’s Law:

2. Find the enthalpy of decomposition of 1 mole of MgO:

Answer details:

Grade: Senior School

Subject: Chemistry

Chapter: Thermodynamics

Keywords: heat of vaporization, enthalpy of vaporization, heat of evaporation, 33.8 g, water, 40.7 kJ/mol, 76.3532 kJ, heat, intensive, extensive, molar mass of water, 18.01 g/mol, 1.876 mol.

Answer from: Quest

Ajava

Answer from: Quest

High-energy and unstable.

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