At the sea level, the dry air mass percentage composition is given as nitrogen gas: 70.0 , oxygen gas: 27.0 and argon gas: 3.0 . If total pressure is 1.15 atm , then calculate the ratio of following respectively:
(i) partial pressure of nitrogen gas to partial pressure of oxygen gas
(ii) partial pressure of oxygen gas to partial pressure of argon gas
(Given: Molar mass of N, O and Ar are 14, 16 and $40 \mathrm{~g} \mathrm{~mol}^{-1}$ respectively.)
Arrange the following gases in increasing order of van der Waals constant 'a'
A. Ar
B. $$\mathrm{CH}_{4}$$
C. $$\mathrm{H}_{2} \mathrm{O}$$
D. $$\mathrm{C}_{6} \mathrm{H}_{6}$$
Choose the correct option from the following.
For 1 mol of gas, the plot of pV vs. p is shown below. p is the pressure and V is the volume of the gas
What is the value of compressibility factor at point A ?
Which amongst the given plots is the correct plot for pressure (p) vs density (d) for an ideal gas?
