A spray can is used until it is empty except for the propellant gas, which has a pressure of 1377 torr at 22°C. If the can is thrown into a fire (T = 463°C), what will be the pressure (in torr) in the hot can?

To solve this problem, we can use the Gay-Lussac's law which states that the pressure of a gas is directly proportional to its absolute temperature, if the volume and the amount of gas remain constant. The formula for Gay-Lussac's law is P1/T1 = P2/T2.

Here's how to solve it step by step:

1. Convert all temperatures to Kelvin. The Kelvin scale is an absolute temperature scale starting at zero, which corresponds to -273.15°C. So, T1 = 22°C = 22 + 273.15 = 295.15 K and T2 = 463°C = 463 + 273.15 = 736.15 K.

2. Substitute the known values into the Gay-Lussac's law equation. P1 is the initial pressure, which is 1377 torr. T1 is the initial temperature, which is 295.15 K. T2 is the final temperature, which is 736.15 K. We're solving for P2, the final pressure.

   So, (P1/T1) = (P2/T2) becomes (1377 torr / 295.15 K) = P2 / 736.15 K.

3. Solve for P2. Multiply both sides of the equation by 736.15 K to get P2 alone on one side of the equation.

   P2 = (1377 torr / 295.15 K) * 736.15 K.

4. Calculate P2. P2 = 3423.6 torr.

So, the pressure in the hot can will be approximately 3424 torr.