What is the primary purpose of stirring a solution while it is being heated?

When liquid water is heated, which of the following occurs as it approaches thermal equilibrium with its surroundings?

A 2.0 kg metal weight at 80 °C is placed into 1.0 kg of water at 20 °C in an insulated container. Assuming no heat is lost to the surroundings and the specific heat capacity of the metal is 0.45 J/g·°C and that of water is 4.18 J/g·°C, what is the final temperature of both the weight and the water at thermal equilibrium?

Which of the following statements best describes thermal equilibrium at constant pressure?

When 20.0 g of water at 25 °C is mixed with 30.0 g of water at 80 °C in an insulated container, what is the final temperature of the mixture? (Assume no heat loss to the surroundings and that the specific heat capacity of water is 4.18 J/g·°C.)

When a substance reaches absolute zero temperature, what happens to its molecules?

What is most likely to occur if you continuously increase the temperature of a liquid at atmospheric pressure?

When water is heated above its boiling point without actually boiling, what is this process called?

When ice is placed in hot water, what happens to the temperature of the ice and the water as they reach thermal equilibrium?