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Calculate the internal energy change when 2 moles of water at 0 degrees converts into ice at 0-degree centigrade?
- a)12 KJ per mole
- b)6 KJ per mole
- c)1 KJ per mole
- d)102 KJ per mole
Correct answer is option 'A'. Can you explain this answer?
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Most Upvoted Answer
Calculate the internal energy change when 2 moles of water at 0 degree...
**Solution:**
To calculate the internal energy change when 2 moles of water at 0 degrees Celsius convert into ice at 0 degrees Celsius, we need to consider the heat transfer associated with this phase change.
**Phase Change:**
When a substance undergoes a phase change, such as from a liquid to a solid, there is a change in the internal energy of the system. This change in internal energy is known as the heat of fusion.
**Heat of Fusion:**
The heat of fusion, denoted as ΔHfus, is the amount of heat energy required to change one mole of a substance from a solid to a liquid at a constant temperature and pressure.
In this case, we need to find the heat of fusion for water. The heat of fusion for water is approximately 6 KJ/mol.
**Calculation:**
Given that we have 2 moles of water, we can calculate the internal energy change using the following formula:
ΔU = nΔHfus
where:
ΔU is the internal energy change
n is the number of moles
ΔHfus is the heat of fusion
Plugging in the values, we get:
ΔU = 2 moles * 6 KJ/mol = 12 KJ
Therefore, the internal energy change when 2 moles of water at 0 degrees Celsius convert into ice at 0 degrees Celsius is 12 KJ.
Hence, the correct answer is option 'A' - 12 KJ per mole.
To calculate the internal energy change when 2 moles of water at 0 degrees Celsius convert into ice at 0 degrees Celsius, we need to consider the heat transfer associated with this phase change.
**Phase Change:**
When a substance undergoes a phase change, such as from a liquid to a solid, there is a change in the internal energy of the system. This change in internal energy is known as the heat of fusion.
**Heat of Fusion:**
The heat of fusion, denoted as ΔHfus, is the amount of heat energy required to change one mole of a substance from a solid to a liquid at a constant temperature and pressure.
In this case, we need to find the heat of fusion for water. The heat of fusion for water is approximately 6 KJ/mol.
**Calculation:**
Given that we have 2 moles of water, we can calculate the internal energy change using the following formula:
ΔU = nΔHfus
where:
ΔU is the internal energy change
n is the number of moles
ΔHfus is the heat of fusion
Plugging in the values, we get:
ΔU = 2 moles * 6 KJ/mol = 12 KJ
Therefore, the internal energy change when 2 moles of water at 0 degrees Celsius convert into ice at 0 degrees Celsius is 12 KJ.
Hence, the correct answer is option 'A' - 12 KJ per mole.
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Community Answer
Calculate the internal energy change when 2 moles of water at 0 degree...
Energy change when 1 mol of water at 0-degree centigrade changes into ice at 0 degrees in centigrade is 6 kJ/mol, So the internal energy change when 2 moles of water at 0 degrees converts into ice at 0 degrees is 12 kJ/mole.
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