Exam 18: Temperature, Heat, and the First Law of Thermodynamics

The diagram shows four thermometers, labeled W, X, Y, and Z. The freezing and boiling points of water are indicated. Rank the thermometers according to the size of a degree on their scales, smallest to largest.

In an adiabatic process:

The specific heat of lead is 0.030 cal/g . $\degree$ C. 300 g of lead shot at 100 $\degree$ C is mixed with 100 g of water at 70 $\degree$ C in an insulated container. The final temperature of the mixture is:

Heat is:

Heat has the same units as:

The coefficient of linear expansion of steel is 11 * 10^-6 per C $\degree$ . A steel ball has a volume of exactly 100 cm³ at 0 $\degree$ C. When heated to 100 $\degree$ C, its volume becomes:

Thin strips of iron and zinc are riveted together to form a bimetallic strip which bends when heated. The iron is on the inside of the bend because:

A balloon is filled with cold air and placed in a warm room. It is NOT in thermal equilibrium with the air of the room until

Object A, with heat capacity C_A and initially at temperature T_A, is placed in thermal contact with object B, with heat capacity C_B and initially at temperature T_B. The combination is thermally isolated. If the heat capacities are independent of the temperature and no phase changes occur, the final temperature of both objects is:

The heat capacity of object B is twice that of object A. Initially A is at 300 K and B is at 450 K. They are placed in thermal contact and the combination is isolated. The final temperature of both objects is:

The formation of ice from water is accompanied by:

The zeroth law of thermodynamics allows us to define

A heat of transformation of a substance is:

A metal sample of mass M requires a power input P to just remain molten. When the heater is turned off, the metal solidifies in a time T. The specific latent heat of fusion of this metal is:

When two gases separated by a diathermal wall are in thermal equilibrium with each other:

Of the following which might NOT vanish over one cycle of a cyclic process?

The diagram shows four rectangular plates and their dimensions. All are made of the same material. The temperature now increases. Of these plates:

Fifty grams of ice at 0 $\degree$ C is placed in a thermos bottle containing one hundred grams of water at 6 $\degree$ C. How many grams of ice will melt? The heat of fusion of water is 333 kJ/kg and the specific heat is 4190 J/kg .K.

The diagram shows four slabs of different materials with equal thickness, placed side by side. Heat flows from left to right and the steady-state temperatures of the interfaces are given. Rank the materials according to their thermal conductivities, smallest to largest.

In a certain process a gas ends in its original thermodynamic state. Of the following, which is possible as the net result of the process?