A gas behaves more closely as an ideal gas at:

1.	low pressure and low temperature
2.	low pressure and high temperature
3.	high pressure and low temperature
4.	high pressure and high temperature

The pressure of an ideal gas is written as \(P= \frac{2E}{3V}\). Here \(E\) refers to:

The energy of a given sample of an ideal gas depends only on its:
1. volume
2. pressure 
3. density
4. temperature.

Which of the following gases has maximum rms speed at a given temperature?
1. hydrogen
2. nitrogen
3. oxygen
4. carbon dioxide

The following figure shows graphs of pressure versus density for an ideal gas at two temperatures \(T_1\) and \(T_2.\)

         
Then:

The mean square speed of the molecules of a gas at absolute temperature \(T\) is proportional to:
1. \(1 \over T\) 
2. \( \sqrt{T} \) 
3. \(T\) 
4. \(T^2\)

The rms speed of oxygen at room temperature is about \(500\) m/s. The rms speed of hydrogen at the same temperature is about:
1.  \(125\) m s^–1
2.  \(2000\) m s^–1
3.  \(8000\) m s^–1
4.  \(31\) m s^–1 

The pressure of a gas kept in an isothermal container is 200 kPa. If half the gas is removed from it, the pressure will be

1.  100 kPa

2.  200 kPa

3.  400 kPa

4.  800 kPa.