Since the volume of the gas is the only variable that has changed, we can use Boyle's law in order to find the final pressure. Since pressure and volume are on the same side of the ideal gas law, they are inversely proportional to one another. In other words, as one increases, the other will decrease, and vice versa.

Boyle's law can be written as follows:

\(\displaystyle P_{1}V_{1} = P_{2}V_{2}\)

Use the given volumes and the initial pressure to solve for the final pressure.

\(\displaystyle (3atm)(3L) = (2L)P_{2}\)

\(\displaystyle P_{2} = 4.5atm\)

Boyle's law relates the pressure and volume of a system, which are inversely proportional to one another. When the parameters of a system change, Boyle's law helps us anticipate the effect the changes have on pressure and volume.

\(\displaystyle P_1V_1=P_2V_2\)

Charles's law relates temperature and volume: \(\displaystyle \frac{V_1}{T_1}=\frac{V_2}{T_2}\)

Gay-Lussac's law relates temperature and pressure: \(\displaystyle \frac{P_1}{T_1}=\frac{P_2}{T_2}\)

The combined gas law takes Boyle's, Charles's, and Gay-Lussac's law and combines it into one law: \(\displaystyle \frac{P_{1}V_{1}}{T_{1}}=\frac{P_{2} V_{2}}{T_{2}}\)

The ideal gas law relates temperature, pressure, volume, and moles in coordination with the ideal gas constant: \(\displaystyle PV=nRT\)

To solve this question we will need to use Boyle's law:

\(\displaystyle P_1V_2=P_2V_2\)

We are given the final pressure and volume, along with the initial volume. Using these values, we can calculate the initial pressure.

\(\displaystyle P_1(735mL)=(0.8atm)(1286mL)\)

\(\displaystyle P_1=\frac{(0.8atm)(1286mL)}{735mL}\)

\(\displaystyle P_1=1.4atm\)

Note that the pressure at sea level is equal to \(\displaystyle 1.0atm\). A pressure greater than \(\displaystyle 1.0atm\) simply indicates that the ground level is below sea level at this point.

The graph shows that there is an inverse relationship between the volume and pressure of a gas, when kept at a constant temperature. This was described by Robert Boyle and can be represented mathematically as Boyle's law:

\(\displaystyle P_1V_1=P_2V_2\)

Gay-Lussac's law shows the relationship between pressure and temperature. Charles's law shows the relationship between volume and temperature. Hund's rule (Hund's law) is not related to gases, and states that electron orbitals of an element will be filled with single electrons before any electrons will form pairs within a single orbital.

To solve this question we will need to use Boyle's law:

\(\displaystyle P_1V_2=P_2V_2\)

We are given the initial pressure and volume, along with the final pressure. Using these values, we can calculate the final volume.

\(\displaystyle (1.12atm)(225mL)=(0.98atm)V_2\)

\(\displaystyle V_2=\frac{(1.12atm)(225mL)}{0.98atm}\)

\(\displaystyle V_2=257mL\)

Use Boyle's Law:

\(\displaystyle P_1*V_1 = P_2*V_2\)

Plug in known values and solve for final volume.

\(\displaystyle 5L+1atm=3.5atm*V_2\)

\(\displaystyle V_2=1.43L\)

Use Boyle's law and plug in appropriate parameters:

\(\displaystyle P_1V_1=P_2V_2\)

\(\displaystyle .666L*1.03atm=5.68atm*V_2\)

\(\displaystyle \frac{.666L*1.03atm}{5.68L}=V_2\)

\(\displaystyle .121L=V_2\)

Boyle's Law is:

\(\displaystyle P_{1} V_{1}=P_{2} V_{2}\)

The initial volume (\(\displaystyle V_{1}\)) and pressure (\(\displaystyle P_{1}\)) of the gas is given. The volume changes to a new volume (\(\displaystyle V_{2}\)). Our goal is to find the new pressure (\(\displaystyle P_{2}\)). Solving for the new pressure gives:

\(\displaystyle \frac{P_{1} V_{1}}{V_{2}}=\frac{P_{2} V_{2}}{V_{2}}\rightarrow P_{2}=\frac{P_{1} V_{1}}{V_{2}}\)

\(\displaystyle P_{2}=\frac{(1.05\, atm)(30\, mL)}{15\, mL}=2.10\, atm\)

Notice the answer has 3 significant figures.