The density of an ideal gas $\mathrm{A}$ is $1.43 \mathrm{g} {\mathrm{L}}^{-1}$ at $\mathrm{STP}$. Determine the density of $\mathrm{A}$ at $17 °\mathrm{C}$ and $700 \mathrm{torr} \left(\mathrm{mm}\right).$ [ Report answer (up to two decimal places) in $\mathrm{g} {\mathrm{L}}^{-1}$]

A container has $3.2$ $\mathrm{g}$ of a certain gas at $\mathrm{NTP}$. What would be the mass of the same gas contained in the same vessel at $200 °\mathrm{C}$ and $16 \mathrm{atm}$ pressure. [ Report answer(up to two decimal places) in gm]

[Hint: molecular weight $\left(\mathrm{M}\right)=\frac{3.2}{\mathrm{V}}\times 22.4; \mathrm{V}=$ volume in $\mathrm{L}$. Apply $\mathrm{pV}=\frac{\mathrm{w}}{\mathrm{M}}\mathrm{RT}$; $\mathrm{w}=$ weight of the gas in $\mathrm{g}$ at $473 \mathrm{K}$ and $16 \mathrm{atm}$.

A sample of nitrogen gas is bubbled through liquid water at $25°\mathrm{C}$ and then collected in a volume of $750 \mathrm{cc}$. The total pressure of the gas which is saturated with water vapour, is found to be $740 \mathrm{mm}$ at $25°\mathrm{C}$. The vapour pressure of water at this temperature is $24 \mathrm{mm}$. How many moles of nitrogen are in the sample?

Give your answer up to four places of decimal.