The volume of a balloon is 2.85 L at 1.00 atm. What pressure is required to compress the balloon to a volume of 1.70 L? The use of chlorofluorocarbons (CFCS) as refrigerants and propellants in aerosol cans has been discontinued as a result of concerns about the ozone layer. If an aerosol can contained 350 mL of CFC gas at a pressure of 5.0 atm, what volume would this gas occupy at 1.0 atm?

A sample of neon gas occupies a volume of 750 ml at 25°C. What will the gas occupy at 50°C if the pressure remains constant?

A sample of methane occupied 18.95 L at 41.03 °C. When the volume changed to 11.60 L at 16.59 °C, the pressure was 2.044 atm. Calculate the original pressure (atm). Write out the problem on paper in order to answer the questions related to the setup and the calculation for this problem. Identify all of the terms in this problem and enter the numerical values (without units) in the appropriate blanks. Convert temperature(s) to K, and enter with proper s.f. If the term doesn't apply in this problem enter 0. Enter a question mark for the variable being calculated. Do not leave any blank empty. P1 =  V1 =  T1= n1= P2= V2= T2= n2=   Rearrange the gas law equation needed to solve for the variable of interest. Identify which terms are in the numerator and which terms are in the denominator after rearranging. Do not leave any blank empty. Enter a zero "0" if the blank is not needed. Use the following abbreviations: pressures = P1, P2; volumes = V1, V2; temperatures = T1, T2, moles = n1, n2…

Refrigerators are usually kept at about 5ﾟC, when Room temperature is about 20ﾟC. If you were to take an empty 2 liter soda bottle at Room temperature and place it in the fridge, would you expect it to contract to 1/4 its original volume?