Every question from past board papers on Equation of state of a perfect gas, work done on compressing a gas, newest paper first. Open any question for its full worked answer.
An oxygen cylinder of volume 30 litre has 18.20 moles of oxygen. After some oxygen is withdrawn from the cylinder, its gauge pressure drops to 11 atmospheric pressure at temperature 27\(^\circ\)C. The mass of the oxygen withdrawn from the cylinder is nearly equal to :
[Given, \(R = \frac{100}{12}\) J mol\(^{-1}\)K\(^{-1}\), and molecular mass of O\(_2\) = 32, 1 atm pressure = \(1.01\times10^5\) N/m]
A container has two chambers of volumes \(V_1 = 2\) litres and \(V_2 = 3\) litres separated by a partition made of a thermal insulator. The chambers contains \(n_1 = 5\) and \(n_2 = 4\) moles of ideal gas at pressures \(p_1 = 1\) atm and \(p_2 = 2\) atm, respectively. When the partition is removed, the mixture attains an equilibrium pressure of :
The following graph represents the T-V curves of an ideal gas (where T is the temperature and V the volume) at three pressures \(P_1\), \(P_2\) and \(P_3\) compared with those of Charles's law represented as dotted lines.
Then the correct relation is:
A cylinder contains hydrogen gas at pressure of 249 kPa and temperature \(27^\circ\)C.
Its density is : (R = 8.3 J mol\(^{-1}\) K\(^{-1}\))
