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Chapter 6: Problem 50

Suggest ways (with appropriate equations) that would enable you to measure the \(\Delta H_{\mathrm{f}}^{\circ}\) values of \(\mathrm{Ag}_{2} \mathrm{O}(s)\) and \(\mathrm{CaCl}_{2}(s)\) from their elements. No calculations are necessary.

Short Answer

Expert verified
The \(\Delta H_{\mathrm{f}}^{\circ}\) values of \(\mathrm{Ag}_{2} \mathrm{O}(s)\) and \(\mathrm{CaCl}_{2}(s)\) can be measured by performing their formation reactions in a calorimeter and observing the temperature change. The reactions for the formation are \[2Ag(s) + 1/2 O_{2}(g) \rightarrow Ag_2 O(s)\] and \[Ca(s) + Cl_{2}(g) \rightarrow CaCl_2(s)\].

Step by step solution

01

Identifying the Elements

Identify the elements of \(\mathrm{Ag}_{2} \mathrm{O}(s)\) and \(\mathrm{CaCl}_{2}(s)\). Silver oxide is composed of silver (Ag) and oxygen (O), and calcium chloride is composed of calcium (Ca) and chlorine (Cl).
02

Formulation of Formation Reactions

Write down the standard formation reaction for each compound. Silver oxide is formed by the reaction of silver and oxygen, while calcium chloride is formed by the reaction of calcium and chlorine. The reactions are as follows: \[2Ag(s) + 1/2 O_{2}(g) \rightarrow Ag_2 O(s)\] and \[Ca(s) + Cl_{2}(g) \rightarrow CaCl_2(s)\].
03

Use of Calorimetry

Suggest the use of calorimetry to measure the \(\Delta H_{\mathrm{f}}^{\circ}\) values. In calorimetry, the heat evolved or absorbed in a chemical reaction is measured by observing the temperature change in an isolated environment. The reactions are carried out in a calorimeter. The temperature change is used to calculate the enthalpy change of formation (\(\Delta H_{\mathrm{f}}^{\circ}\)).

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Most popular questions from this chapter

Calculate the internal energy of a Goodyear blimp filled with helium gas at \(1.2 \times 10^{5} \mathrm{~Pa}\). The volume of the blimp is \(5.5 \times 10^{3} \mathrm{~m}^{3} .\) If all the energy were used to heat 10.0 tons of copper at \(21^{\circ} \mathrm{C},\) calculate the final temperature of the metal. (Hint: See Section 5.6 for help in calculating the internal energy of a gas. 1 ton \(\left.=9.072 \times 10^{5} \mathrm{~g} .\right)\)

A gas expands and does \(P-V\) work on the surroundings equal to \(325 \mathrm{~J}\). At the same time, it absorbs \(127 \mathrm{~J}\) of heat from the surroundings. Calculate the change in energy of the gas.

Consider two metals A and B, each having a mass of \(100 \mathrm{~g}\) and an initial temperature of \(20^{\circ} \mathrm{C}\). The specific heat of \(A\) is larger than that of \(B\). Under the same heating conditions, which metal would take longer to reach a temperature of \(21^{\circ} \mathrm{C} ?\)

Ice at \(0^{\circ} \mathrm{C}\) is placed in a Styrofoam cup containing \(361 \mathrm{~g}\) of a soft drink at \(23^{\circ} \mathrm{C}\). The specific heat of the drink is about the same as that of water. Some ice remains after the ice and soft drink reach an equilibrium temperature of \(0^{\circ} \mathrm{C}\). Determine the mass of ice that has melted. Ignore the heat capacity of the cup. (Hint: It takes 334 J to melt \(1 \mathrm{~g}\) of ice at \(\left.0^{\circ} \mathrm{C} .\right)\)

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 \(\mathrm{AgNO}_{2}(s)\).
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