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Chapter 12 – Section 2 - The Gas Laws

Chapter 12 – Section 2 - The Gas Laws. In this section, you will study the relationships between the measurable properties of a gas, represented by the variables shown below. P = pressure exerted V = total volume occupied by the gas T = temperature in Kelvin's.

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Chapter 12 – Section 2 - The Gas Laws

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  1. Chapter 12 – Section 2 -The Gas Laws In this section, you will study the relationships between the measurable properties of a gas, represented by the variables shown below. P = pressure exerted V = total volume occupied by the gas T = temperature in Kelvin's Pressure-Volume Relationships In 1662, the English scientist Robert Boyle studied the relationship between the volume and the pressure of a gas. He found that as pressure on a gas increases in a closed container, the volume of the gas decreases. In fact, the product of the pressure and volume, PV, remains almost constant if the temperature remains the same.

  2. In the closed system below when the piston is lowered the pressure increases as the volume decreases. The amount of gas does not change but the distance between the particles decreases.

  3. Boyle’s Law The inverse relationship between pressure and volume is known as Boyles Law. If the temperature and number of particles are not changed, the PV product remains the same, as shown in the equation below. P1V1 = P2V2 The relationship between pressure and volume is a inverse relationship. This means as one variable is increased the other will decrease.

  4. When using Boyles law please keep in mind that: - the most commonly used units for volume are liters and milliliters. - in regents chemistry we will use kPa and atm units for pressure. -standard pressure is 1.0 atm or 101.3 kPa

  5. Charles’s Law The direct relationship between temperature and volume is known as Charle’s law. The kinetic-molecular theory states that gas particles move faster on average at higher temperatures, causing them to hit the walls of their container with more force. Repeated strong collisions cause the volume of a flexible container, such as a balloon, to increase. If the Kelvin temperature is reduced by half, then the average kinetic energy is reduced by half, and the particles will strike the walls with half of the energy they had at the higher temperature. In that case, the volume of the gas will be reduced to half of the original volume if the pressure remains the same.

  6. The direct relationship between temperature and volume is known as Charles Law. If the pressure and number of particles are not changed, the quotient remains the same, as shown in the equation below. V1 V2 T1 T2 = The relationship between temperature and volume is a direct relationship. This means as one variable is increased the other will increase.

  7. Combined Gas Law Both Boyles and Charles law can be combined into a single formula. The combined gas law is given in the Reference table and shown below. You can use the combined gas law to obtain either Boyles or Charles law. Removing any variable that is constant from the combined gas law will produce the formula needed.

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