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Gay lussac practice worksheet

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 observe set ups (especially in gas laws) that simply omit all the units in the answer. If you undertake 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

Gay-Lussac's Law Worksheet: Exercise Problems

Name: ____________________ Lussac’s Law Worksheet 1. Write the equation for Gay Lussac’s Law. Define the symbols used. 2. What gas statute variable is unchanging in Gay-Lussac’s Law? 3. A rigid container has an initial pressure of 1.50 atm at 294 K. What will the pressure be if the temperature is increased to 394 K? 4. The pressure inside a container is 1.10 atm at a temperature of 330 K. What would the pressure be at 348 K? 5. A rigid container is at a temperature of 65 oC. When heated to 224 oC, the pressure was 2.20 atm. What was the initial pressure? 6. If a gas in a closed container is pressurized from 1520 kPa to 1621 kPa and its original temperature was 298 K, what would the final temperature of the gas be? 7. At -23 oC a gas had a pressure of 0.853 atm. At what temperature would it be at 1.32 atm? 8. The pressure in an automobile tire is 2.00 atm at 300 K. At the end of a road trip the pressure has risen to 2.20 atm. What is the temperature of the air in the tire, assuming the volume has not changed? 9. A balloon is filled with helium gas to a pressure of 1140 mm Hg when the temperature is 295 K. If the temperatu

Gay-Lussac's Law

Gay-Lussac's Law, also recognizable as the pressure-temperature regulation, is one of the gas laws discovered by the French chemist Joseph Louis Gay-Lussac in 1802. This law describes the relationship between the pressure and temperature of a gas at constant volume. The law can be stated as:

Pf / Tf = Pi / Ti

Where Pf and Tf are the final pressure and temperature of the gas, and Pi and Ti are the initial pressure and temperature of the gas, respectively.

Explanation of Gay-Lussac's Law

Gay-Lussac's Law states that the pressure of a given amount of gas held at constant volume is directly proportional to the Kelvintemperature. This means that as the temperature of a gas increases, so does its pressure, and vice versa. Mathematically, this can be expressed as P / T = k, where P is the pressure, T is the temperature in Kelvin, and k is a constant.

Application of Gay-Lussac's Law

This law is particularly important in understanding the behavior of gases in various real-world scenarios. For instance, it helps in predicting how changes in temperature will affect the pressure of a gas in a sealed container, such as a gas cylinder or a balloon. It also forms th

Honors Chemistry Gas Laws Worksheet #2 Name ______________________________ Hour ____ Gay-Lussac’s Law 1. Equation for Gay-Lussac’s Law: 2. How are the two variables related to each other? 3. Why do we use Kelvin when doing calculations that involve gases? 4. A gas in a closed container has a pressure of 300 kPa at 30.2 °C. What will the pressure be if the temperature drops to -172.8 °C? 5. A gas has a pressure of 6.58 kPa at 539 K. What will the pressure be at 211 K if the volume does not change? 6. The pressure in a car tire is 1.84 atm at 27.5 °C. At the end of a trip on a hot, sunny day, the pressure has risen to 2.49 atm. What is the temperature of the atmosphere in the tire? 7. The gas left in a used aerosol can is at a pressure of 103.4 kPa at 25.6 °C. If this can is thrown onto a campfire, what is the pressure of the gas when its temperature reaches 928.1 °C? Combined Gas Law 8. Equation for the Combined Gas Law: 9. How do you determine which variable had a bigger impact on your final answer? 10. The volume of a gas decreased from 2 L to 1 L. The temperature of a gas increased from 20 °C to 100 °C. If the initi