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## Warm-up

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**Warm-up**Convert the following: 4.5 atm = _____ kPa 845.6 torr = _____ kPa 103.5 kPa = _____ mm Hg**Boyle’s Law: P and V**• as one increases, • the other decreases • inversely proportional P1 = P2 V2 V1**Example: Boyle’s Law**Consider a 1.53-L sample of gaseous SO2 at a pressure of 5.6 x 103 Pa. If the pressure is changed to 1.5 x 104 Pa at constant temperature, what will be the new volume of the gas?**Charles’ Law: V and T**• if P is constant, gases expand when heated • when T increases, gas molecules move faster and collide with the walls more often and with greater force • to keep the P constant, the V must increase**Charles’ Law: V and T**• Charles’ Law: the V of fixed mass of gas at constant P varies directly with Kelvin T. • V = kT • k is a constant for a certain sample of gas that depends on the mass of gas and P • What kind of graph is V vs. T?**Charles’ Law: V and T**• discovered by French physicist, Jacques Charles in 1787 • first person to fill balloon with hydrogen gas and make solo balloon flight**Example: Charles’ Law & Temp.**A sample of gas at 15°C and 1 atm has a volume of 2.58 L. What volume will this gas occupy at 38°C and 1 atm?**Gay-Lussac’s Law: P and T**• Gay-Lussac’s Law: the P of fixed mass of gas at constant V varies directly with Kelvin T. • What kind of graph is P vs. T?**Example: Gay-Lussac’s Law**The gas in an aerosol can is at a pressure of 3.00 atm at 25°C. Directions on the can warn the user not to keep the can in a place where temperature exceeds 52°C. What would the gas pressure be in the can at 52°C?**Way to remember which law goes with P,V and T**Boyle’s P V T Gay-Lussac’s Charles’**Combined Gas Law**• P1V1 = P2V2 T1 T2**A cylinder of a gas is kept at a constant volume, as the**temperature increases from 24.1 C to 326.4 C. If the initial pressure was 1.10 atm, what is the final pressure in mm Hg?