Heat and Internal Energy
Physics ⇒ Heat and Thermodynamics
Heat and Internal Energy starts at 7 and continues till grade 12.
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A 100 g sample of water is heated from 25°C to 75°C. If the specific heat capacity of water is 4,200 J/kg·K, calculate the heat absorbed.
A 2 kg block of iron is heated from 20°C to 50°C. If the specific heat capacity of iron is 450 J/kg·K, how much heat is required?
A gas is compressed by doing 150 J of work on it, and 50 J of heat is removed from it. What is the change in internal energy?
A metal block at 80°C is placed in water at 20°C. In which direction does heat flow?
A system absorbs 400 J of heat and does 100 J of work. What is the change in internal energy?
Describe what happens to the internal energy of a gas when it is compressed rapidly without heat exchange.
Describe what happens to the internal energy of a system when it is cooled.
Explain the difference between heat and internal energy.
Explain why metals are good conductors of heat.
If 500 J of heat is added to a system and the system does 200 J of work, what is the change in internal energy of the system?
State the First Law of Thermodynamics in your own words.
What is the main difference between heat and temperature?
Which law states that energy cannot be created or destroyed, only transferred or converted from one form to another?
A 0.5 kg block of copper at 150 °C is placed in 1 kg of water at 20 °C. Assuming no heat is lost to the surroundings and the specific heat capacities are 390 J/kg·K for copper and 4,200 J/kg·K for water, calculate the final equilibrium temperature of the system.
A 250 g sample of a substance requires 5,000 J of heat to raise its temperature from 30 °C to 70 °C. Calculate the specific heat capacity of the substance.
A system releases 300 J of heat to the surroundings and has 200 J of work done on it. What is the change in internal energy of the system?
Describe how the internal energy of a system can change without any heat transfer.
Explain why the internal energy of an ideal gas does not change during an isothermal expansion, even though the gas does work on its surroundings.
A 0.3 kg piece of aluminum at 100 °C is dropped into 0.7 kg of oil at 20 °C in an insulated container. The specific heat capacity of aluminum is 900 J/kg·K and that of oil is 2,000 J/kg·K. Calculate the final equilibrium temperature of the mixture, assuming no heat is lost to the surroundings.
A 400 g sample of a metal at 120 °C is placed in 600 g of water at 25 °C. The final temperature of the mixture is 30 °C. If the specific heat capacity of water is 4,200 J/kg·K, calculate the specific heat capacity of the metal. (Assume no heat loss to the surroundings.)
