# Gay Lussac’s Law

**Definition**: Gay Lussac’s Law describes the *relationship between temperature (T) and Pressure (P)* while number of moles (n) and volume (V) remain constant.

**Relation**: *T and P are directly proportional* so as temperature increases, pressure increases.

T α P

**Equation:**

**Example:**

Imagine you’ve just picked up a bunch of balloons for a party and you leave them in the car while running errands on a hot day. Since the balloons are sealed, the volume (V↔) is held constant so while the temperature inside the car increases (↑T) and gas naturally wants to expand (Boyle’s Law), it cannot. So the pressure inside the balloon increases (P↑) until it becomes too much and balloons pop. Looks like you have one more errands to re-run. True story!

**Problem: **A sample of CO_{2} gas at 10°C has a pressure of 1.2 atm. What is the pressure when the temperature is increased to 25°C?

GIVEN:

T_{1} = 10° → K Conversion Required → 10°C + 273 = 283K

P_{1 }= 1.2 atm

P_{2 }= ?

T_{2 }= 25° → K Conversion Required → 25°C + 273 = 298K

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