The energy released when 0.250 mol of mercury (II) oxide (red) is formed from its elements is

To determine the energy released when 0.250 mol of mercury(II) oxide (HgO) is formed from its elements, we need the enthalpy change of the reaction.

The balanced chemical equation for the formation of mercury(II) oxide from its elements is:

\[ \text{Hg} (l) + \frac{1}{2} \text{O}_2 (g) \rightarrow \text{HgO} (s) \]

The standard enthalpy change of formation (ΔH°f) of HgO is approximately -90.7 kJ/mol.

To calculate the energy released when 0.250 mol of HgO is formed:

\[
\text{Energy released} = \text{moles of HgO} \times \Delta H^\circ_f
\]
\[
\text{Energy released} = 0.250 \, \text{mol} \times (-90.7 \, \text{kJ/mol})
\]
\[
\text{Energy released} = -22.675 \, \text{kJ}
\]

So, the energy released when 0.250 mol of mercury(II) oxide is formed is **-22.675 kJ**.

Would you like more details, or have any questions?

Here are five related questions for further exploration:
1. What is the enthalpy of formation for other oxides like aluminum oxide or carbon dioxide?
2. How does the energy released differ if a different amount of HgO is formed?
3. What factors affect the enthalpy change of a reaction?
4. How is the enthalpy of formation of a compound determined experimentally?
5. How does temperature influence the energy released in chemical reactions?

**Tip:** Remember that the negative sign in enthalpy indicates that the reaction is exothermic, meaning it releases energy.

Discover how to calculate the energy released when forming 0.250 mol of mercury(II) oxide (HgO) from its elements. Understand chemical thermodynamics and enthalpy changes in this detailed problem solution. Suitable for advanced high school and college chemistry students.

Math Problem Statement

Solution

Ask a new question for Free

By Image

Math Problem Analysis

Mathematical Concepts

Formulas

Theorems

Suitable Grade Level

Related Recommendation