What happens to the internal energy of an ideal gas when it is heated from 0C to 4C?
When an ideal gas is heated from 0°C to 4°C, the internal energy of the gas increases. The internal energy of a gas depends on its temperature, and as the temperature of the gas increases, so does its internal energy. The increase in temperature causes the gas molecules to move faster and have more kinetic energy, which contributes to the increase in internal energy. Therefore, the internal energy of an ideal gas increases when it is heated from 0°C to 4°C.
To understand what happens to the internal energy of an ideal gas when it is heated, we need to consider the ideal gas law and the concept of temperature.
The ideal gas law states that for a given amount of gas, the product of pressure (P) and volume (V) is directly proportional to the product of the number of moles (n) and the absolute temperature (T). Mathematically, this can be expressed as:
PV = nRT
where R is the ideal gas constant.
Now, let's consider the concept of temperature. Temperature is a measure of the average kinetic energy of the gas particles. When a gas is heated, the average kinetic energy of its particles increases.
In this case, we are given that the gas is heated from 0 degrees Celsius (C) to 4 degrees Celsius (C). To convert temperatures from Celsius to Kelvin (K), we need to add 273.15 to the Celsius value. Therefore, the initial temperature is 0 + 273.15 = 273.15 K, and the final temperature is 4 + 273.15 = 277.15 K.
As the temperature of the gas increases, the average kinetic energy of its particles also increases. The increase in kinetic energy leads to an increase in the internal energy of the gas. Therefore, the internal energy of the ideal gas will increase when it is heated from 0°C to 4°C.
In conclusion, the internal energy of an ideal gas increases when it is heated from 0°C to 4°C.