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Chapter 6: Problem 8

Stoichiometry is based on the law of conservation of mass. On what law is thermochemistry based?

Short Answer

Expert verified
Thermochemistry is based on the First Law of Thermodynamics, which is also known as the Law of Energy Conservation.

Step by step solution

01

Understanding Thermochemistry

Thermochemistry is the branch of chemistry that studies how heat energy is involved in chemical reactions. It focuses on understanding the energy changes that take place during these reactions.
02

Identifying the Fundamental Law

The law fundamental to thermochemistry is the First Law of Thermodynamics, also known as the Law of Energy Conservation. This law states that energy cannot be created or destroyed, only transferred or changed from one form to another.

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Most popular questions from this chapter

Calculate the standard enthalpy of formation for diamond, given that $$\begin{array}{l} \text { C(graphite) }+\mathrm{O}_{2}(g) \longrightarrow \mathrm{CO}_{2}(g) \\ \qquad \begin{aligned} \Delta H^{\circ} &=-393.5 \mathrm{~kJ} / \mathrm{mol} \\ \mathrm{C}(\text { diamond })+\mathrm{O}_{2}(g) \longrightarrow & \mathrm{CO}_{2}(g) \\ \Delta H^{\circ} &=-395.4 \mathrm{~kJ} / \mathrm{mol} \end{aligned} \end{array}$$

\(\mathrm{Mg}^{2+}\) is a smaller cation than \(\mathrm{Na}^{+}\) and also carries more positive charge. Which of the two species has a larger hydration energy (in \(\mathrm{kJ} / \mathrm{mol}\) ) ? Explain.

The standard enthalpy change \(\Delta H^{\circ}\) for the thermal decomposition of silver nitrate according to the following equation is \(+78.67 \mathrm{~kJ}\) : $$\mathrm{AgNO}_{3}(s) \longrightarrow \mathrm{AgNO}_{2}(s)+\frac{1}{2} \mathrm{O}_{2}(g)$$ The standard enthalpy of formation of \(\mathrm{AgNO}_{3}(s)\) is \(-123.02 \mathrm{~kJ} / \mathrm{mol} .\) Calculate the standard enthalpy of formation of \(\mathrm{AgNO}_{2}(s)\)

From the following data, $$ \begin{array}{c} \mathrm{C} \text { (graphite) }+\mathrm{O}_{2}(g) \longrightarrow \mathrm{CO}_{2}(g) \\ \Delta H_{\mathrm{rxn}}^{\circ}=-393.5 \mathrm{~kJ} / \mathrm{mol} \\ \mathrm{H}_{2}(g)+\frac{1}{2} \mathrm{O}_{2}(g) \longrightarrow \mathrm{H}_{2} \mathrm{O}(l) \\ \Delta H_{\mathrm{rxn}}^{\circ}=-285.8 \mathrm{~kJ} / \mathrm{mol} \\ 2 \mathrm{C}_{2} \mathrm{H}_{6}(g)+7 \mathrm{O}_{2}(g) \longrightarrow 4 \mathrm{CO}_{2}(g)+6 \mathrm{H}_{2} \mathrm{O}(l) \\ \Delta H_{\mathrm{rxn}}^{\circ}=-3119.6 \mathrm{~kJ} / \mathrm{mol} \end{array} $$ calculate the enthalpy change for the reaction $$ 2 \mathrm{C}(\text { graphite })+3 \mathrm{H}_{2}(g) \longrightarrow \mathrm{C}_{2} \mathrm{H}_{6}(g) $$

Decomposition reactions are usually endothermic, whereas combination reactions are usually exothermic. Give a qualitative explanation for these trends.
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