Seema Saini Solutions for Chapter: States of Matter, Exercise 2: DPP 4.2

$0.553 \mathrm{g}$ of a boron-hydrogen compound created a pressure of $0.658 \mathrm{atm}$ in a bulb of $407 \mathrm{mL}$ at $100°\mathrm{C}$. Analysis showed it to be $85.7\%$ boron. Calculate its molecular formula.

Calculate the $\%$ of 'free volume' available in $1 \mathrm{mol}$gaseous water at $1.0 \mathrm{atm}$ and $100°\mathrm{C}$. Density of liquid water at $100°\mathrm{C}$ is $0.958 \mathrm{g}/\mathrm{mol}$. 

A mixture of ${\mathrm{NH}}_3 \left(\mathrm{g}\right)$ and ${\mathrm{N}}_2{\mathrm{H}}_4 \left(\mathrm{g}\right)$ is placed in a sealed container at $300 \mathrm{K}$. The pressure within the container is $0.6 \mathrm{atm}$. The container is heated to $1000 \mathrm{K}$ where, the two gases undergo decomposition reactions. 

$2{\mathrm{NH}}_3 \left(\mathrm{g}\right)\to {\mathrm{N}}_2 \left(\mathrm{g}\right)+3{\mathrm{H}}_2 \left(\mathrm{g}\right)$ and ${\mathrm{N}}_2{\mathrm{H}}_4 \left(\mathrm{g}\right)\to {\mathrm{N}}_2 \left(\mathrm{g}\right)+2{\mathrm{H}}_2 \left(\mathrm{g}\right)$ 

The pressure of the container at this stage become $4.8 \mathrm{atm}$. What was the mole percent of ${\mathrm{NH}}_3 \left(\mathrm{g}\right)$ in the original mixture?

At $10°\mathrm{C}$, the density of a fixed mass of an ideal gas divided by its pressure is $\mathrm{X}$. At $110°\mathrm{C}$, this ratio would be: 

Which of these gases exhibits behavior that deviates most significantly from that expected from an ideal gas?

Ten moles of an ideal gas is filled in a closed vessel. The vessel has cylinder and piston type arrangement and pressure of the gas remains constant at $0.821 \mathrm{atm}$. Which of the following graph represents the correct variation of $\log \mathrm{V}$ vs $\log \mathrm{T}$? ($\mathrm{V}=$Volume in litre and $\mathrm{T}=$Temperature in kelvin)
 

For a definite amount of gas, the pressure and volume are increased to triple of the initial amount. Therefore, 

The equations of state of an ideal gas is/are: