The ideal gas law has some conditions that must be met, conditions that certainly cannot be met in the real world. These conditions include that the gases cannot interact with one another, gases must be moving in a random straight-line fashion, gas molecules must not take up any space, and gases must be in perfect elastic collisions with the walls of the container. These conditions minimize the effect that gas molecules have on one other, allowing a prediction based on completely random and unimpeded molecular movement. In reality, these conditions are impossible. All real gas molecules have a molecular volume and some degree of intermolecular attraction forces.

In this case, two variables are changed between the initial and final containers: volume and temperature. Since we are looking for the final pressure on the container, we can use the combined gas law in order to solve for the final pressure:

When using the ideal gas law, remember that temperature must be in Kelvin, not Celsius, so we will need to convert.

Use the given values to solve for the final pressure.

Once again, we can use the ideal gas law in order to solve for the unknown gas. We will start again with the ideal gas law:

Density has the units of mass over volume, which means that we can rearrange the ideal gas law so that density is on one side of the equation. However, we need to substitute one of the values so mass is also in the equation. Remember that moles are equal to mass divided by molar mass, so we can rewrite "n" in order to solve for density:

STP means that the container is at 1 atmosphere of pressure and 273 Kelvin. Knowing this, we can solve for molar mass:

Fluorine gas has a molar mass of 38.00 grams per mol. As a result, we determine that fluorine gas is the unknown gas in the container.

In order to determine the gas being contained, we are going to need to rewrite the ideal gas law. The ideal gas law is written as follows:

The number of moles of a gas can be rewritten as the mass of the gas divided by its molar mass. Knowing this, we can rewrite the equation, and solve for the molar mass of the gas.

Use the given values in this equation to solve for the molar mass. Remember to first convert degree Celsius to Kelvin!

Now that we have solved for the molar mass, we can see which gas has this molar mass on the periodic table. Argon has a molar mass of 39.95 grams per mole, so we can determine that argon is the gas in the container. 

The combined gas law takes Boyle's, Charles's, and Gay-Lussac's law and combines it into one law.

It is able to relate temperature, pressure, and volume of one system when the parameters for any of the three change.

Boyle's law relates pressure and volume:

Charles's law relates temperature and volume:

Gay-Lussac's law relates temperature and pressure:

The ideal gas law relates temperature, pressure, volume, and moles in coordination with the ideal gas constant:

This question requires the combined equation of the individual gas laws:

To use this equation, we first need to convert the given temperatures to Kelvin.

We now know the initial pressure, volume, and temperature, allowing us to solve the left side of the equation.

Use the given values for the final temperature and pressure to solve for the final volume.

This question requires s to use the combined gas law:

We know the initial pressure, temperature, and volume, allowing us to solve for the left side of the equation.

We are also given the final pressure and temperature. Using these values on the right side of the equation we can solve for the final volume.

The ideal gas law is used to identify values in a given state (for the values of pressure, volume, number of moles, and temperature) for an ideal, hypothetical gas. Because no gases are truly ideal, this only works as an approximation, and some gases are more ideal than others.

First we need to remember what STP means since it's important. This is "standard temperature and pressure".  Because we are looking for the number of moles we need the ideal gas law.

At STP we will take the temperature to be  and the pressure to be . Solving for the number of moles gives

Notice that the units of the gas constant R mean we must have a volume in liters. The volume was given in mL and therefore had to be converted.

We have a lot going on in this problem. Since both temperature and volume change and we want to know the final pressure, the combined gas law will be used:

Since the gas is at STP to start we know the pressure () and the temperature (). Standard pressure has multiple values depending on the units, but we want pressure in atm for our final answer so we will choose the appropriate value and units for STP. Solving for the final pressure gives:

Plugging in everything gives:

We expect that raising the temperature will increase the pressure as well as reducing the volume. Since both actions will increase the pressure we must have a final pressure greater than the initial pressure.