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Ch.5 - Thermochemistry
Brown - Chemistry: The Central Science 14th Edition
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232Non è quello che usi tu?Cambia libro di testo
Tutti i libri di testoBrown 14th EditionCh.5 - ThermochemistryProblema 51d
Capitolo 5, Problema 51d

(d) How many kJ of heat are needed to raise the temperature of 5.00 kg of liquid water from 24.6 to 46.2 °C?

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Identify the formula to calculate the heat required: \( q = m \cdot c \cdot \Delta T \), where \( q \) is the heat energy, \( m \) is the mass, \( c \) is the specific heat capacity, and \( \Delta T \) is the change in temperature.
Determine the mass \( m \) of the water, which is given as 5.00 kg.
Use the specific heat capacity \( c \) of liquid water, which is typically \( 4.18 \text{ J/g°C} \). Convert this to \( \text{kJ/kg°C} \) if necessary.
Calculate the change in temperature \( \Delta T \) by subtracting the initial temperature from the final temperature: \( \Delta T = 46.2°C - 24.6°C \).
Substitute the values into the formula to find \( q \): \( q = 5.00 \text{ kg} \times 4.18 \text{ kJ/kg°C} \times \Delta T \).

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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. For water, this value is approximately 4.18 J/g°C. Understanding this concept is crucial for calculating the heat energy needed for temperature changes in substances.
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Heat Capacity

Heat Transfer Equation

The heat transfer equation, often expressed as q = mcΔT, relates the heat energy (q) absorbed or released by a substance to its mass (m), specific heat capacity (c), and the change in temperature (ΔT). This equation is fundamental for solving problems involving temperature changes in materials.
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Heat Capacity

Units of Energy

Energy is commonly measured in joules (J) or kilojoules (kJ), where 1 kJ equals 1000 J. In thermodynamics, it is important to be consistent with units when performing calculations, especially when converting between different energy units to ensure accurate results.
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SI Units
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(a) What amount of heat (in joules) is required to raise the temperature of 1 g of water by 1 kelvin? (b) What amount of heat (in joules) is required to raise the temperature of 1 mole of water by 1 kelvin?

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Two solid objects, A and B, are placed in boiling water and allowed to come to the temperature of the water. Each is then lifted out and placed in separate beakers containing 1000 g of water at 10.0 °C. Object A increases the water temperature by 3.50 °C; B increases the water temperature by 2.60 °C. (b) What can you say about the specific heats of A and B?

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The specific heat of octane, C8H18(l), is 2.22 J•g/K. (b) Which will require more heat, increasing the temperature of 1 mol of C8H18(l), by a certain amount or increasing the temperature of 1 mol of H2O(l) by the same amount?

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The specific heat of octane, C8H18(l), is 2.22 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?

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(b) Calculate the energy needed for this temperature change.

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(c) What is the heat capacity of 185 g of liquid water?

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