With regard to the gaseous state of matter which of the following statements are correct ?
Which of the following figures does not represent 1 mole of dioxygen gas at STP?
Under which of the following conditions applied together, a gas deviates most from the ideal behaviour?
Which of the following changes decrease the vapour pressure of water kept in a sealed vessel ?
If 1 g of each of the following gases are taken at STP, which of the gases will occupy (a) greatest volume and (b) smallest volume?
$$\mathrm{CO}, \mathrm{H}_2 \mathrm{O}, \mathrm{CH}_4, \mathrm{NO}$$
From Avogadro's law, we know that
Volume of 1 mole of the gas = graw molecular mass $=22.4 \mathrm{~L}$ at STP
Volume occupied by $28 \mathrm{~g} \mathrm{CO}(1 \mathrm{~mol} \mathrm{CO})=22.4 \mathrm{~L}$ at STP
$\left(\because\right.$ Molar mass of $\left.\mathrm{CO}=12+16=28 \mathrm{~g} \mathrm{~mol}^{-1}\right)$
$\therefore \quad$ Volume occupied by $1 \mathrm{~g} \mathrm{~CO}=\frac{22.4}{28} \mathrm{~L}$ at STP
Similarly, volume occupied by $1 \mathrm{~g} \mathrm{~H}_2 \mathrm{O}=\frac{22.4}{18} \mathrm{~L}$ at STP
$\left(\because\right.$ Molar mass of $\left.\mathrm{H}_2 \mathrm{O}=(2 \times 1)+16=18 \mathrm{~g} \mathrm{~mol}^{-1}\right)$
Volume occupied by $1 \mathrm{~g} \mathrm{CH}_4=\frac{22.4}{16} \mathrm{~L}$ at STP
$\left(\because\right.$ Molar mass of $\left.\mathrm{CH}_4=12+(4 \times 1)=16 \mathrm{~g} \mathrm{~mol}^{-1}\right)$
Volume occupied by $1 \mathrm{~g} \mathrm{NO}=\frac{22.4}{30} \mathrm{~L}$ at STP
$\left(\because\right.$ Molar mass of $\left.\mathrm{NO}=14+16=30 \mathrm{~g} \mathrm{~mol}^{-1}\right)$
Thus, $1 \mathrm{~g} \mathrm{CH}_4$ will occupy maximum volume while 1 g of NO will occupy minimum volume at STP.