Thermal Equilibrium
Physics ⇒ Heat and Thermodynamics
Thermal Equilibrium starts at 8 and continues till grade 12.
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A 100 g iron block at 80 °C is placed in 200 g of water at 25 °C. If the specific heat of iron is 0.45 kJ/kg·K and water is 4.18 kJ/kg·K, what is the final temperature at equilibrium?
A 2 kg block of copper at 100 °C is placed in 1 kg of water at 20 °C. If no heat is lost to the surroundings, what is the final temperature at equilibrium? (Specific heat of copper = 0.39 kJ/kg·K, water = 4.18 kJ/kg·K)
A 500 g aluminum block at 60 °C is placed in 200 g of water at 20 °C. If no heat is lost, what is the final temperature? (Specific heat of aluminum = 0.9 kJ/kg·K, water = 4.18 kJ/kg·K)
A metal block at 80 °C is placed in water at 20 °C. After some time, both reach 30 °C. What is the final state called?
A thermometer is placed in a liquid. After a few minutes, the thermometer reading stops changing. What does this indicate?
Describe a real-life example of thermal equilibrium.
Describe what happens when a hot object is placed in a cooler environment.
Explain what would happen if the Zeroth Law of Thermodynamics did not hold true.
Explain why a thermometer works based on the concept of thermal equilibrium.
Explain why the Zeroth Law of Thermodynamics is important for the construction of thermometers.
If object A is in thermal equilibrium with object B, and object B is in thermal equilibrium with object C, what can you say about objects A and C?
If three objects, A, B, and C, are such that A is in thermal equilibrium with B, and B is in thermal equilibrium with C, but A and C are not in contact, are A and C in thermal equilibrium?
Two objects, A and B, are placed in contact. After some time, there is no net heat flow between them. What can you conclude about their temperatures?
What is meant by thermal equilibrium?
Which law states that if two systems are each in thermal equilibrium with a third system, then they are in thermal equilibrium with each other?
A 250 g block of unknown metal at 120 °C is placed in 400 g of water at 25 °C. The final equilibrium temperature is 30 °C. If the specific heat capacity of water is 4.18 kJ/kg·K, calculate the specific heat capacity of the metal. Assume no heat is lost to the surroundings.
A 300 g copper block at 150 °C is dropped into 500 g of oil at 20 °C in an insulated container. The specific heat capacity of copper is 0.39 kJ/kg·K and that of oil is 2.0 kJ/kg·K. Calculate the final equilibrium temperature, assuming no heat is lost to the surroundings.
Describe how the concept of thermal equilibrium is applied in the calibration of thermometers.
Explain, using the concept of microscopic particle motion, why two objects at different temperatures reach thermal equilibrium when placed in contact.
