Gas Laws and the steps to solve them

The Gas Laws Boyle’s Law: P1V1=P2V2 (Temp and moles constant) Guy Lusaac’s Law: P1/T1=P2/T2 ( Volume and Moles are constant) Charles’ Law: V1/T1=V2/T2 (Pressure and Moles are Constant) Combined Gas Law: (P1V1 )/T1=(P2V2 )/T2

Steps to solve: Standard temp = 0°C or 273K Understand & identify the units for each variable Read Problem and write down variables Change or convert units Pick the Gas Law you are going to use Plug in your known values Solve for the unknown variable Add Units to Answer NOTE: Standard Pressure= 1atm Standard temp = 0°C or 273K

Deflategate On the day of the 2015 AFC championship game between the NE Patriots and the Indianapolis Colts the pressure in 12 out of 13 of the Patriot’s footballs was discovered to be underinflated. (A football should have a pressure of 12.5-13.5 psi) When the footballs were inflated in the locker room prior to the kickoff the temperature was 294K. Let’s assume that the footballs were inflated to 13 psi. During half time the pressure of the Patriot’s 13 football’s were checked for pressure and it was discovered that on average, their pressure was 11.5 psi. The air temperature during the game was 278K Which Gas Law equation can we use to prove this? What should the pressure in the footballs be at halftime if they were inflated correctly?

A gas has a temperature of 287 0K, and a volume of 4. 5 liters A gas has a temperature of 287 0K, and a volume of 4.5 liters. If the temperature is raised to 302 0K and the pressure is not changed, what is the new volume of the gas?

There is 1.00 L of a gas at standard temperature and pressure is compressed to 4.73 L. What is the new pressure of the gas?

A gas that has a volume of 28 liters, a temperature of 45 0C, and an unknown pressure has its volume increased to 34 liters and its temperature decreased to 35 0C. If I measure the pressure after the change to be 2.0 atm, what was the original pressure of the gas?