Sample problem on gay lussacs law
Gay-Lussac's Law
Problems #1 - 10
Ten Examples
KMT & Gas Laws Menu
Problem #1: A 30.0 L sample of nitrogen inside a rigid, metal container at 20.0 °C is placed inside an oven whose temperature is 50.0 °C. The pressure inside the container at 20.0 °C was at 3.00 atm. What is the pressure of the nitrogen after its temperature is increased to 50.0 °C?
Solution:
P1 P2 ––– = ––– T1 T2
3.00 x ––– = ––– 293 323 Solution technique: cross-multiply and divide.
x = 3.31 atm (to three sig figs)
Note: you will notice set ups (especially in gas laws) that simply omit all the units in the resolution. If you act that on a homework problem or test, you may get a deduction. It's not laziness on the part of the person writing the answer, it's simply assuming the reader knows what the units are and how they cancel out to leave the final unit.
Many times, you (as the student) are not allowed that luxury.
Problem #2: Determine the pressure change when a constant volume of gas at 1.00 atm is heated from 20.
The Ideal Gas Law
The Gay-Lussac’s law demonstrates the relationship between the pressure and the temperature of an ideal gas. Let’s illustrate it by using a pump with a barrel that is held at a fixed position to prevent changing the volume. The pump is heated, and we are trying to see how increasing the temperature affects the pressure of the gas. Remember, in the experiment for the Charle’s law, heating the pump resulted in increasing the volume because the barrel could freely move. Now, here because we complete not allow moving the barrel, the volume stays continual, and the pressure of the gas increases instead.
The pressure is directly proportional to the temperature of the gas, so we can write that:
P ~ T
To bring in the equal write instead of the proportional sign, we introduce a constant:
P = constant x T
This can be explained using the example of a car dealership income. The income depends on the number of sales which we can illustrate as:
Income ∼ number of cars
However, we cannot express income = number of cars sold, so to switch an equal indicate, we need to introduce a steady. This can be the price of the car transforming the equation to:
Income =price x numb
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Gay-Lussac’s law or Amonton’s law states that the absolute temperature and pressure of an ideal gas are directly proportional, under conditions of constant mass and volume. In other words, heating a gas in a sealed container causes its pressure to amplify, while cooling a gas lowers its pressure. The reason this happens is that increasing temperature imparts thermal kinetic energy to gas molecules. As the temperature increases, molecules collide more often with the container walls. The increased collisions are seen as increased pressure.
The law is named for French chemist and physicist Joseph Gay-Lussac. Gay-Lussac formulated the rule in 1802, but it was a formal declaration of the relationship between temperature and pressure described by French physicist Guillaume Amonton in the delayed 1600’s.
Gay-Lussac’s law states the temperature and pressure of an ideal gas are directly proportional, assuming steady mass and volume.
Gay-Lussac’s Rule Formula
Here are the three common formulas for Gay-Lussac’s law:
P ∝ T
(P1/T1) = (P2/T2)
P1T2 = P2T1
P stands for pressure, while T is absolute temperature. Be sure to co
Gay-Lussac's Law
Discussion and Ten 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 steady. 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 build 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 advance slower and they will impact the container walls less often. This means the gas pressure inside the container will reduce, since the container has rigid walls (v