Suppose a pot of water is heated on the stove. After the temperature of the wate

Question

Suppose a pot of water is heated on the stove. After the temperature of the water has risen a certain amount, the water IS NOT boiling, but the temperature stops rising even though heat continues to be transferred. Explain how it is possible to transfer heat without changing the temperature of the water. Imagine you transfer a certain amount of heat to a known amount of a liquid in a perfectly insulated cup and the temperature changes. Then, you decide to alter the experiment in several different ways. For each of the alterations listed below, state whether the change in temperature will be larger, smaller or the same as that measured before the alteration. Briefly explain each answer. Transfer more heat Heat for a longer time but transfer the same total heat Put more liquid in the cup Increase the temperature outside of the cup Start with warmer liquid Change to an equal mass of liquid with a larger specific heat capacity Use the same volume of a denser liquid with the same specific heat capacity You have two perfectly insulated cups. One contains water and the other contains an equal volume f another liquid that has half the density of water and two times the specific heat capacity. You heat the water from 10 to 20 degree C and the other liquid from 80 to 90 degree C. Compare the amount of heat energy transferred to raise the temperature of the other liquid to the amount transferred to raise the temperature of the water. Explain how you got your answer. How many calories of heat would it take to heat 200 ml of water from 20 degree C to 80 degree C? Show your calculations. calories

Explanation / Answer

8)We know that,

Q = m c delta T

density = mass/vol

mass = density x volume

mass = 1000 x 0.0002 = 0.2 kg

Q = 0.2 x 4186 x (80 - 20) = 50232 J

Hence, Q = 50232 J = 12.06 cal

[since 1 cal = 4184 J]

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