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Consider that, a ball is immersed in water at room temperature and then taken out having 18 grams of water on it, how much amount of energy is required to dry that water at room temperature?
- a)41.43 KJ/mol
- b)49.53 KJ/mol
- c)41.3 KJ/mol
- d)41.53 KJ/mol
Correct answer is option 'D'. Can you explain this answer?
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Consider that, a ball is immersed in water at room temperature and the...
Heat required to eliminate water : n x ΔvapH– = (1 mol) × (44.01 kJ mol–1) = 44.01 kJ mol-1. Δvapor = ΔvapH – ΔnRT = 44.01 kJ mol-1 – 1×8.314 J/K-mol x 298 k x 10-3 = 41.53 KJ/mol. So the amount of energy needed is 41.53 KJ/mol.
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Consider that, a ball is immersed in water at room temperature and the...
Calculation:
To determine the amount of energy required to dry the water from the ball, we need to consider the heat required for the phase change from liquid to gas and the specific heat capacity of water.
Phase change:
The heat required for the phase change from liquid to gas is given by the equation:
Q = m × ΔHvap
Where:
Q is the heat energy
m is the mass of water
ΔHvap is the enthalpy of vaporization
The enthalpy of vaporization of water is 40.7 kJ/mol.
The molar mass of water (H2O) is 18 g/mol.
So, the amount of energy required for the phase change is:
Q = (18 g) / (18 g/mol) × (40.7 kJ/mol)
Q = 40.7 kJ
Specific heat capacity:
The heat required to raise the temperature of the water from room temperature to its boiling point and then to vaporize it is given by the equation:
Q = m × Cp × ΔT
Where:
Q is the heat energy
m is the mass of water
Cp is the specific heat capacity of water
ΔT is the change in temperature
The specific heat capacity of water is 4.18 J/g°C.
The change in temperature is the boiling point of water (100°C) minus the room temperature.
Q = (18 g) × (4.18 J/g°C) × (100°C - room temperature)
Converting the units from J to kJ:
Q = (18 g) × (4.18 J/g°C) × (100°C - room temperature) / 1000
Total energy:
The total energy required is the sum of the energy required for the phase change and the energy required for the temperature change:
Total energy = Phase change energy + Specific heat energy
Total energy = 40.7 kJ + [(18 g) × (4.18 J/g°C) × (100°C - room temperature) / 1000]
Answer:
The correct answer is option D) 41.53 kJ/mol.
To determine the amount of energy required to dry the water from the ball, we need to consider the heat required for the phase change from liquid to gas and the specific heat capacity of water.
Phase change:
The heat required for the phase change from liquid to gas is given by the equation:
Q = m × ΔHvap
Where:
Q is the heat energy
m is the mass of water
ΔHvap is the enthalpy of vaporization
The enthalpy of vaporization of water is 40.7 kJ/mol.
The molar mass of water (H2O) is 18 g/mol.
So, the amount of energy required for the phase change is:
Q = (18 g) / (18 g/mol) × (40.7 kJ/mol)
Q = 40.7 kJ
Specific heat capacity:
The heat required to raise the temperature of the water from room temperature to its boiling point and then to vaporize it is given by the equation:
Q = m × Cp × ΔT
Where:
Q is the heat energy
m is the mass of water
Cp is the specific heat capacity of water
ΔT is the change in temperature
The specific heat capacity of water is 4.18 J/g°C.
The change in temperature is the boiling point of water (100°C) minus the room temperature.
Q = (18 g) × (4.18 J/g°C) × (100°C - room temperature)
Converting the units from J to kJ:
Q = (18 g) × (4.18 J/g°C) × (100°C - room temperature) / 1000
Total energy:
The total energy required is the sum of the energy required for the phase change and the energy required for the temperature change:
Total energy = Phase change energy + Specific heat energy
Total energy = 40.7 kJ + [(18 g) × (4.18 J/g°C) × (100°C - room temperature) / 1000]
Answer:
The correct answer is option D) 41.53 kJ/mol.
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Consider that, a ball is immersed in water at room temperature and then taken out having 18 grams of water on it, how much amount of energy is required to dry that water at room temperature?a)41.43 KJ/molb)49.53 KJ/molc)41.3 KJ/mold)41.53 KJ/molCorrect answer is option 'D'. Can you explain this answer?
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Consider that, a ball is immersed in water at room temperature and then taken out having 18 grams of water on it, how much amount of energy is required to dry that water at room temperature?a)41.43 KJ/molb)49.53 KJ/molc)41.3 KJ/mold)41.53 KJ/molCorrect answer is option 'D'. Can you explain this answer? for NEET 2024 is part of NEET preparation. The Question and answers have been prepared according to the NEET exam syllabus. Information about Consider that, a ball is immersed in water at room temperature and then taken out having 18 grams of water on it, how much amount of energy is required to dry that water at room temperature?a)41.43 KJ/molb)49.53 KJ/molc)41.3 KJ/mold)41.53 KJ/molCorrect answer is option 'D'. Can you explain this answer? covers all topics & solutions for NEET 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for Consider that, a ball is immersed in water at room temperature and then taken out having 18 grams of water on it, how much amount of energy is required to dry that water at room temperature?a)41.43 KJ/molb)49.53 KJ/molc)41.3 KJ/mold)41.53 KJ/molCorrect answer is option 'D'. Can you explain this answer?.
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