 Okay, let's do a gas law problem now. So this one says, a sample of hydrogen gas in a closed container has a temperature of 37 degrees Celsius and a pressure of 2.00 ATM. What will the pressure be if the sample is heated to 127 degrees Celsius? Okay? So this is effectively gain-lose-sax law, so it's one of the laws that you can get from using the ideal gas law. So remember, in this case, as we've got a change, we're going to do pv equals nRT over pv equals nRT, right? So, okay, R never changes. Okay, so look here. Did p change? Did p change? Did p change, guys? Yes. Yes, okay. So can we cancel it out? No. Okay, did p change? No. No, can we cancel it out? Okay, did n change? No. Can we cancel it? No. Did t change? Yes. Can we cancel it? No. So our new equation is p1 over p2 equals t1 over t2. So what are we looking for? p2. So let's rearrange this equation. So p1 t2 equals p2 t1, right? So p2 equals p1 t2 divided by t1. The other thing, these temperatures are in degrees Celsius. So we've got to do what? Convert them to Kelvin. Good job, guys. So 273 plus 37 is going to be 310 Kelvin, and 273 plus 127. So that's 300, 400, p2, p1, 2.00, atm, t1, 310 Kelvin. Divided by t2, 400 Kelvin, divided by t1, 310 Kelvin. 400 divided by 310, and the pressure I get is 2.58. And atm is the unit. Why do we just cancel with Kelvin? Any questions on that? So this is a loose-x law problem.