What happens to the internal energy of an ideal gas when it is heated from 0C to 4C?

a. increases

b. decreases
c. change in number of atoms
d. increase in volume of substance

The internal energy of an ideal gas can be increased by heating it. To determine what happens to the internal energy when a gas is heated from 0°C to 4°C, we need to consider how the internal energy of an ideal gas is related to its temperature.

The internal energy of an ideal gas is directly proportional to its temperature, according to the ideal gas law. This relationship is expressed by the equation:

ΔU = nCvΔT

Where:
ΔU is the change in internal energy of the gas
n is the number of moles of the gas
Cv is the molar specific heat capacity of the gas at constant volume
ΔT is the change in temperature

In this case, we are given the temperature change from 0°C to 4°C. The change in temperature (ΔT) can be calculated as 4°C - 0°C = 4K.

To determine the change in internal energy (ΔU), we need to know the value of the molar specific heat capacity of the gas at constant volume (Cv). For an ideal monoatomic gas, such as helium or neon, Cv is typically 3/2R, where R is the gas constant.

Once we know the values of ΔT and Cv, we can calculate the change in internal energy (ΔU) using the equation mentioned earlier.

So, to answer the question, the internal energy of an ideal gas increases when it is heated from 0°C to 4°C. The exact amount of increase can be calculated using the equation ΔU = nCvΔT, where n is the number of moles of the gas, Cv is the molar specific heat capacity, and ΔT is the change in temperature.