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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

Describe two exothermic processes and two endothermic processes.

A 44.0-g sample of an unknown metal at \(99.0^{\circ} \mathrm{C}\) was placed in a constant-pressure calorimeter containing \(80.0 \mathrm{~g}\) of water at \(24.0^{\circ} \mathrm{C}\). The final temperature of the system was found to be \(28.4^{\circ} \mathrm{C}\). Calculate the specific heat of the metal. (The heat capacity of the calorimeter is \(\left.12.4 \mathrm{~J} /{ }^{\circ} \mathrm{C} .\right)\)

A 1.00 -mole sample of ammonia at 14.0 atm and \(25^{\circ} \mathrm{C}\) in a cylinder fitted with a movable piston \(\mathrm{ex}\) pands against a constant external pressure of 1.00 atm. At equilibrium, the pressure and volume of the gas are 1.00 atm and 23.5 L, respectively. (a) Calculate the final temperature of the sample. (b) Calculate \(q, w,\) and \(\Delta E\) for the process. The specific heat of ammonia is \(0.0258 \mathrm{~J} / \mathrm{g} \cdot{ }^{\circ} \mathrm{C}\)

Define these terms: thermochemistry, exothermic process, endothermic process.

Describe how chemists use Hess's law to determine the \(\Delta H_{\mathrm{f}}^{\circ}\) of a compound by measuring its heat (enthalpy) of combustion.
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