Discussion and Five Examples

Discovered by Joseph Louis Gay-Lussac in the early 1800's. That is pretty much all the ChemTeam knows. Maybe I'll learn more of the details someday.

Gay-Lussac's Law gives the relationship between pressure and temperature when volume and amount are held constant. In words:

1) If the temperature of a container is increased, the pressure increases.

2) If the temperature of a container is decreased, the pressure decreases.

What makes them true? We can make brief reference to the ideas of kinetic-molecular theory (KMT), which Gay-Lussac did not have access to in the early 1800's. KMT was developed in its modern form about 50 years later.

1) Suppose the temperature is increased. This means gas molecules will move faster and they will impact the container walls more often. This means the gas pressure inside the container will increase, since the container has rigid walls (volume stays constant).2) Suppose the temperature is decreased. This means gas molecules will move slower and they will impact the container walls less often. This means the gas pressure inside the container will decrease, since the container has rigid walls (volume stays constant).

Gay-Lussac's Law is a direct mathematical relationship. This means there are two connected values and when one (either P or T) goes up, the other (either P or T) also increases. The constant K remains the same value.

The mathematical form of Gay-Lussac's Law is:

P ––– = k T

This means that the pressure-temperature fraction will always be the same value if the volume and amount remain constant.

Let P_{1} and T_{1} be a pressure-temperature pair of data at the start of an experiment. If the temperature is changed to a new value called T_{2}, then the pressure will change to P_{2}. Keep in mind that when volume is not discussed (as in this law), it is constant. That means a container with rigid walls.

As with the other laws, the exact value of k is unimportant in our context. It is important to know the PT data pairs obey a constant relationship, but it is not important for us what the exact value of the constant is. Besides which, the value of K would shift based on what pressure units (atm, mmHg, or kPa) you were using.

We know this:

P _{1}––– = k T _{1}

And we know this:

P _{2}––– = k T _{2}

Since k = k, we have this:

P _{1}P _{2}––– = ––– T _{1}T _{2}

Be aware that you can also see this equation written as:

P_{1}/ T_{1}= P_{2}/ T_{2}

or:

P_{1}T_{2}= P_{2}T_{1}

The second one, of course, resulting from cross-multiplication of the equation in fractional form.

Make sure to convert any Celsius temperature to Kelvin before using it in your calculation.

**Example #1:** 10.0 L of a gas is found to exert 97.0 kPa at 25.0 °C. What would be the required temperature (in Celsius) to change the pressure to standard pressure?

**Solution:**

1) Change 25.0 °C to 298.0 K and remember that standard pressure in kPa is 101.325. Insert values into the equation to get:

97.0 kPa 101.325 kPa ––––––– = ––––––––– 298.0 K x x = 311.3 K

2) The question asks for Celsius, so you subtract 273 to get the final answer of 38.3°C. Notice that the volume never enters the problem. This is because the problem is asking about the relationship between pressure and temperature; the volume (as well as the moles) remains constant.

**Example #2:** 5.00 L of a gas is collected at 22.0 °C and 745.0 mmHg. When the temperature is changed to standard, what is the new pressure?

**Solution:**

1) Convert to Kelvin and insert:

P_{1}/ T_{1}= P_{2}/ T_{2}745.0 mmHg / 295.0 K = x / 273 K

2) Cross multiply and divide for the new pressure. Be careful to cross-multiply correctly when you see a set up like the one just above. It's easy to get the numbers mixed up.

Sometimes a problem will give you one pressure in one unit and ask for the new pressure in a different unit. In that case, simply do the problem and then convert the pressure to the different unit.

**Example #3:** What is the new pressure (in atm) when a constant volume of gas is heated from 25.1 °C to 37.5 °C? The starting pressure is 755.0 mmHg.

**Solution:**

1) Set it up and solve:

755.0 mmHg x –––––––––– = ––––––– 298.1 K 310.5 K x = 786.4 mmHg

2) Convert to atm:

(786.4 mmHg) (1 atm / 760.0 mmHg) = 1.035 atm

You could have converted the 755.0 mmHg to atm first, if so desired.

By the way, the real value for standard temperature is 273.15 K. However, when used in gas law problems, 273 K tends to be used. In addition, 273 tends to be the value used when converting Celsius to Kelvin. The technically correct value to use is 273.15, but it is used far less often than 273.

**Example #4:** A constant volume of gas has a pressure of 0.350 atm at 50.0 °C. What is the pressure when the temperature is doubled?

Comment: the problem statement gives Celsius, so it seems obvious that Celsius is intended to double. However, what if Kelvin was what the question writer had in mind?

**Solution for doubling Celsius:**

1) Convert temperatures:

50.0 °C ---> 323 K

100.0 °C ---> 373 K

2) Solve:

(0.350 atm) (373 K) = (x) (323 K)x = 0.404 atm

**Solution for doubling Kelvin:**

P_{1}T_{2}= P_{2}T_{1}(0.350 atm) (646 K) = (x) (323 K)

x = 0.700 atm

The P_{1}T_{2} = P_{2}T_{1} equation is not often used. Be careful, it may just show up without any explanation.

**Example #5:** If a gas in a closed container is pressurized from 15.0 atmospheres to 16.0 atmospheres and its original temperature was 25.0 °C, what would the final temperature of the gas be?

**Solution:**

15.0 atm / 298 K = 16.0 atm / xx = 317.9 K

Changing it to Celsius and three sig figs gives 45.0 °C for the final answer.