alculate to three significant digits the density of chlorine pentafluoride gas at exactly 0°C and exactly 1atm. You can assume chlorine pentafluoride gas behaves as an ideal gas under these conditions.gL
Question
alculate to three significant digits the density of chlorine pentafluoride gas at exactly 0°C and exactly 1atm. You can assume chlorine pentafluoride gas behaves as an ideal gas under these conditions.gL
Solution
To calculate the density of chlorine pentafluoride gas at exactly 0°C and exactly 1atm, we can use the ideal gas law equation, which is PV = nRT.
Step 1: Convert the temperature to Kelvin. The Kelvin scale starts at absolute zero, which is -273.15°C. So, 0°C is 273.15K.
Step 2: Rearrange the ideal gas law equation to solve for n/V, which gives us the number of moles per volume. This is essentially the density. The rearranged equation is n/V = P/RT.
Step 3: Plug in the values. The pressure P is 1 atm, the gas constant R is 0.0821 L·atm/(K·mol), and the temperature T is 273.15K. So, n/V = 1 atm / (0.0821 L·atm/(K·mol) * 273.15K) = 0.0446 mol/L.
Step 4: Convert moles to grams to get the density in g/L. The molar mass of chlorine pentafluoride (ClF5) is about 130.45 g/mol. So, the density is 0.0446 mol/L * 130.45 g/mol = 5.82 g/L.
So, to three significant digits, the density of chlorine pentafluoride gas at exactly 0°C and exactly 1atm is 5.82 g/L.
Similar Questions
Calculate to three significant digits the density of boron trifluoride gas at exactly 25°C and exactly 1atm. You can assume boron trifluoride gas behaves as an ideal gas under these conditions.
Calculate to three significant digits the density of carbon monoxide gas at exactly 30°C and exactly 1atm. You can assume carbon monoxide gas behaves as an ideal gas under these conditions.
Calculate to three significant digits the density of carbon dioxide gas at exactly 20°C and exactly 1atm. You can assume carbon dioxide gas behaves as an ideal gas under these conditions.
A 7.00L tank at 24.9°C is filled with 5.16g of chlorine pentafluoride gas and 4.17g of dinitrogen difluoride gas. You can assume both gases behave as ideal gases under these conditions.Calculate the total pressure in the tank. Round your answer to the correct number of significant digits.
A 10.0L tank at 0.89°C is filled with 13.2g of chlorine pentafluoride gas and 16.0g of sulfur tetrafluoride gas. You can assume both gases behave as ideal gases under these conditions.Calculate the mole fraction and partial pressure of each gas in the tank. Be sure your answers have the correct number of significant digits.chlorine pentafluoride mole fraction: partial pressure: atmsulfur tetrafluoride mole fraction: partial pressure: atm
Upgrade your grade with Knowee
Get personalized homework help. Review tough concepts in more detail, or go deeper into your topic by exploring other relevant questions.