Question

1. Define the ff:
A. Heat-

B. Heat capacity-

2. Why is it desirable to have the water a few degrees colder than room temperature when the initial temperature is taken?

3. Why is the mass of the outer shell of the calorimeter and the insulating ring not included in taking data for Calorimetry?

6. Why should the hot metal be dry before it is introduced into the cold water? 837 calories of heat are required to heat 100.00 grams of copper from 0.0 C to 100.0 C. What is the specific heat of copper?

***Determining specific heat through insulating through coffee cup. Aluminum is heated and then immediately put in a thermal cup containing water.. Shaked.. then Final Temperature is determined.

4. What does this experiment show about the specific heat of water?

5. How does the conductivity of the metal used in this experiment affect the accuracy of the results?

Answer 1

1Ans:

Heat is one form of energy that flows as a result in the difference of temperature. Its units are Joules.

Heat capacity: It is the amount of heat energy that is required to raise the temperature of a given quantity of the substance by one degree Celsius.

2Ans:

According to the Second Law of Thermodynamics, heat flows from hotter to colder objects. Ideally, water needs to be a few degrees colder than the room temperature in order that heat will flow to the system because it is colder than the surroundings, making the system more efficient in absorbing heat.

3Ans:

Because they are not part of the isolated system, making their masses irrelevant in the computation of specific heat.

6Ans:
The hot metal should be dry before it is introduced into the cold water in order tomaximize the direct contact between the surface of the metal and the molecules of water,thereby improving the heat exchange.