Consider the data about gold metal in Exercise 5.24(b). c. What is the molar heat capacity of Au(s)?

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Identify the given data from Exercise 5.24(b) related to gold (Au), such as its specific heat capacity and molar mass.

Recall the formula for molar heat capacity: \( C_m = c \times M \), where \( c \) is the specific heat capacity and \( M \) is the molar mass.

Substitute the specific heat capacity of gold into the formula. The specific heat capacity is typically given in units of \( \text{J/g} \cdot \text{°C} \).

Substitute the molar mass of gold into the formula. The molar mass of gold is approximately 197 g/mol.

Multiply the specific heat capacity by the molar mass to find the molar heat capacity of gold in units of \( \text{J/mol} \cdot \text{°C} \).

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Molar Heat Capacity

Molar heat capacity is the amount of heat required to raise the temperature of one mole of a substance by one degree Celsius (or one Kelvin). It is an important property that reflects how a substance absorbs and retains heat, influencing its thermal behavior. For solids like gold, this value can vary based on temperature and phase.

Specific Heat Capacity

Specific heat capacity is the heat required to raise the temperature of one gram of a substance by one degree Celsius. While molar heat capacity is expressed per mole, specific heat is often used for practical calculations involving smaller quantities. The relationship between the two can be established through the molar mass of the substance.

Thermodynamic Properties of Metals

The thermodynamic properties of metals, including heat capacity, are influenced by their atomic structure and bonding. Metals typically have high thermal conductivity and specific heat capacities, which affect how they respond to heat. Understanding these properties is essential for applications in materials science and engineering, particularly in processes involving temperature changes.

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The specific heat of ethanol, C₂H₅OH(l), is 2.44 J•g/K. (a) How many J of heat are needed to raise the temperature of 80.0 g of octane from 10.0 to 25.0 °C?

Textbook Question

The specific heat of ethanol, C₂H₅OH(l), is 2.44 J•g/K. b. Which will require more heat, increasing the temperature of 1 mol of C₂H₅OH(𝑙) by a certain amount or increasing the temperature of 1 mol of H₂O(𝑙) by the same amount?

Textbook Question

Consider the data about gold metal in Exercise 5.24(b). b. Suppose that the same amount of heat is added to two 10.0-g blocks of metal, both initially at the same temperature. One block is gold metal, and the other is iron metal. Which block will have the greater rise in temperature after addition of the heat?

Textbook Question

When a 5.10-g sample of solid sodium hydroxide dissolves in 100.0 g of water in a coffee-cup calorimeter (Figure 5.18), the temperature rises from 20.5 to 33.2 °C. a. Calculate the quantity of heat (in kJ) released in the reaction.

Textbook Question

When a 5.10-g sample of solid sodium hydroxide dissolves in 100.0 g of water in a coffee-cup calorimeter (Figure 5.18), the temperature rises from 20.5 to 33.2 °C. b. Using your result from part (a), calculate ΔH (in kJ/mol NaOH) for the solution process. Assume that the specific heat of the solution is the same as that of pure water.

Textbook Question

(b) Is this process endothermic or exothermic?

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