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Ch.12 - Liquids, Solids & Intermolecular Forces
Tro - Chemistry: A Molecular Approach 6th Edition
Tro6th EditionChemistry: A Molecular ApproachISBN: 9780137832217Non è quello che usi tu?Cambia libro di testo
Tutti i libri di testoTro 6th EditionCh.12 - Liquids, Solids & Intermolecular ForcesProblema 76
Capitolo 12, Problema 76

How much ice (in grams) would have to melt to absorb 155 kJ of energy?

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1
Identify the heat of fusion for ice, which is the amount of energy required to melt 1 gram of ice. The heat of fusion for ice is approximately 334 J/g.
Convert the energy from kilojoules to joules, since the heat of fusion is given in joules per gram. Remember that 1 kJ = 1000 J.
Use the formula: \( q = m \times \Delta H_f \), where \( q \) is the energy absorbed, \( m \) is the mass of the ice, and \( \Delta H_f \) is the heat of fusion.
Rearrange the formula to solve for the mass \( m \): \( m = \frac{q}{\Delta H_f} \).
Substitute the values for \( q \) (in joules) and \( \Delta H_f \) (334 J/g) into the equation to find the mass of ice that needs to melt.

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Heat of Fusion

The heat of fusion is the amount of energy required to change a substance from solid to liquid at its melting point without changing its temperature. For ice, this value is approximately 334 J/g. Understanding this concept is crucial for calculating how much ice must melt to absorb a specific amount of energy.
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02:19
Heat Capacity

Energy Transfer

Energy transfer refers to the movement of energy from one system to another, often in the form of heat. In this context, when ice melts, it absorbs energy from its surroundings, which is essential for the phase change. Recognizing how energy is absorbed during melting helps in determining the mass of ice needed to absorb a given amount of energy.
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01:26
Nature of Energy

Calculating Mass from Energy

To find the mass of ice that must melt to absorb a certain amount of energy, one can use the formula: mass = energy absorbed / heat of fusion. This calculation allows for the direct conversion of energy (in joules or kilojoules) into mass (in grams), facilitating the solution to the problem presented.
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03:12
Molar Mass Calculation Example
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Nitrogen has a normal boiling point of 77.3 K and a melting point (at 1 atm) of 63.1 K. Its critical temperature is 126.2 K and its critical pressure is 2.55×104 torr. It has a triple point at 63.1 K and 94.0 torr. Sketch the phase diagram for nitrogen. Does nitrogen have a stable liquid state at 1 atm?

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Consider the phase diagram shown here. Identify the states present at points a through g.

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How much energy is released when 75.2 g of water freezes?

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