A gas occupies 210 mL at -73°C. To have the same gas occupy 360 mL, should the temperature be increased or decreased?

To solve this problem, we can use the combined gas law which states that the ratio of the product of pressure and volume to the temperature of a system remains constant. In this case, we are not given any information about the pressure, so we can use Charles's Law which is a special case of the combined gas law where the pressure is constant. Charles's Law states that the volume of a gas is directly proportional to its absolute temperature.

Here are the steps to solve the problem:

1. Convert the temperatures from Celsius to Kelvin. The Kelvin scale is the standard system used in these types of physics problems. The conversion formula is K = °C + 273.15.

   So, -73°C = -73 + 273.15 = 200.15 K.

2. Apply Charles's Law, which can be written as V1/T1 = V2/T2, where V1 is the initial volume, T1 is the initial temperature, V2 is the final volume, and T2 is the final temperature.

   We know that V1 = 210 mL, T1 = 200.15 K, and V2 = 360 mL. We need to find T2.

3. Substitute the known values into the equation and solve for T2:

   210 mL / 200.15 K = 360 mL / T2 T2 = (360 mL * 200.15 K) / 210 mL T2 = 343.2 K

4. Convert T2 back to Celsius: °C = K - 273.15 T2 = 343.2 K - 273.15 = 70.05°C

So, to have the gas occupy 360 mL, the temperature should be increased to approximately 70°C.