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Ch.5 - Thermochemistry
Brown - Chemistry: The Central Science 14th Edition
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Tutti i libri di testoBrown 14th EditionCh.5 - ThermochemistryProblema 106a
Capitolo 5, Problema 106a

A coffee-cup calorimeter of the type shown in Figure 5.18 contains 150.0 g of water at 25.1°C A 121.0-g block of copper metal is heated to 100.4°C by putting it in a beaker of boiling water. The specific heat of Cu(s) is 0.385 J/g-K The Cu is added to the calorimeter, and after a time the contents of the cup reach a constant temperature of 30.1°C. (a) Determine the amount of heat, in J, lost by the copper block.

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Identify the initial and final temperatures of the copper block: \(T_{\text{initial, Cu}} = 100.4^\circ\text{C}\) and \(T_{\text{final, Cu}} = 30.1^\circ\text{C}\).
Calculate the change in temperature for the copper block: \(\Delta T_{\text{Cu}} = T_{\text{final, Cu}} - T_{\text{initial, Cu}}\).
Use the formula for heat transfer: \(q = m \cdot c \cdot \Delta T\), where \(m\) is the mass of the copper block, \(c\) is the specific heat capacity of copper, and \(\Delta T\) is the change in temperature.
Substitute the known values into the formula: \(m = 121.0\, \text{g}\), \(c = 0.385\, \text{J/g-K}\), and \(\Delta T\) calculated in step 2.
Calculate the heat lost by the copper block, \(q\), using the substituted values.

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Specific Heat Capacity

Specific heat capacity is the amount of heat required to raise the temperature of one gram of a substance by one degree Celsius (or one Kelvin). It is a material-specific property that varies between different substances. In this problem, the specific heat of copper is given as 0.385 J/g-K, which will be used to calculate the heat lost by the copper block as it cools down.
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Heat Capacity

Heat Transfer

Heat transfer refers to the movement of thermal energy from one object or substance to another due to a temperature difference. In this scenario, the copper block loses heat to the water in the calorimeter until thermal equilibrium is reached. The principle of conservation of energy dictates that the heat lost by the copper will equal the heat gained by the water.
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Heat Capacity

Calorimetry

Calorimetry is the science of measuring the heat of chemical reactions or physical changes. In this context, a coffee-cup calorimeter is used to measure the heat exchange between the copper block and the water. By applying the formula Q = mcΔT, where Q is heat, m is mass, c is specific heat, and ΔT is the change in temperature, we can determine the heat lost by the copper.
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Constant-Volume Calorimetry
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A coffee-cup calorimeter of the type shown in Figure 5.18 contains 150.0 g of water at 25.1°C A 121.0-g block of copper metal is heated to 100.4°C by putting it in a beaker of boiling water. The specific heat of Cu(s) is 0.385 J/g-K The Cu is added to the calorimeter, and after a time the contents of the cup reach a constant temperature of 30.1°C (b) Determine the amount of heat gained by the water. The specific heat of water is 4.184 J/1gK.

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A coffee-cup calorimeter of the type shown in Figure 5.18 contains 150.0 g of water at 25.1°C A 121.0-g block of copper metal is heated to 100.4°C by putting it in a beaker of boiling water. The specific heat of Cu(s) is 0.385 J/g-K The Cu is added to the calorimeter, and after a time the contents of the cup reach a constant temperature of 30.1°C (d) What would be the final temperature of the system if all the heat lost by the copper block were absorbed by the water in the calorimeter?

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