David Sang and Graham Jones Solutions for Chapter: Ideal Gases, Exercise 5: Questions

At what temperature (in $\mathrm{K}$ ) will $1.0 \mathrm{mol}$ of a gas occupy $1.0{ \mathrm{m}}^3$ at a pressure of $1.0\times {10}^4 \mathrm{Pa}$ ?

Nitrogen consists of molecules ${\mathrm{N}}_2$. The molar mass of nitrogen is $28 \mathrm{g}{ \mathrm{mol}}^{-1}$. For $100 \mathrm{g}$ of nitrogen, calculate the number of moles.

Nitrogen consists of molecules ${\mathrm{N}}_2$. The molar mass of nitrogen is $28 \mathrm{g}{ \mathrm{mol}}^{-1}$. For $100 \mathrm{g}$ of nitrogen, calculate the volume occupied at room temperature and pressure $\left(20°\mathrm{C};1.01\times {10}^5 \mathrm{Pa}\right)$.

Calculate the volume of $5.0 \mathrm{mol}$ of an ideal gas at a pressure of $1.0\times {10}^5 \mathrm{Pa}$ and a temperature of $200°\mathrm{C}$.

A sample of gas contains $3.0\times {10}^{24}$ molecules. Calculate the volume of the gas at a temperature of $300 \mathrm{K}$ and a pressure of $120\mathrm{kPa}$.

At what temperature would $1.0 \mathrm{kg}$ of oxygen occupy $1.0{ \mathrm{m}}^3$ at a pressure of $1.0\times {10}^5 \mathrm{Pa}$ ? (Molar mass of ${\mathrm{O}}_2=32 \mathrm{g}{ \mathrm{mol}}^{-1}$.)

A cylinder of hydrogen has a volume of $0.100{ \mathrm{m}}^3$. Its pressure is found to be $20$ atmospheres at $20°\mathrm{C}$. Calculate the mass of hydrogen in the cylinder.

A cylinder of hydrogen has a volume of $0.100{ \mathrm{m}}^3$. Its pressure is found to be $20$ atmospheres at $20°\mathrm{C}$. If it were instead filled with oxygen to the same pressure, how much oxygen would it contain? (Molar mass of ${\mathrm{H}}_2=2.0 \mathrm{g}{ \mathrm{mol}}^{-1}$, molar mass of ${\mathrm{O}}_2=32 \mathrm{g}{ \mathrm{mol}}^{-1}$, $1$ atmosphere $=1.01\times {10}^5 \mathrm{Pa}$).