A 9 L tank at 20.6°C is filled with 5.25 g of chlorine pentafluoride gas, and 8.81 g of carbon dioxide gas. you can assume both gases, behave as ideal gases under these conditions calculate the partial pressure of each gas in the tank round each of your answers to three significant digits.
To calculate the partial pressure of each gas, we can use the ideal gas law equation:
PV = nRT
Where:
P = pressure
V = volume
n = moles
R = gas constant
T = temperature
First, we need to calculate the number of moles for each gas:
For chlorine pentafluoride (ClF5):
molar mass (ClF5) = 1(35.45) + 5(18.99) = 130.4 g/mol
moles (ClF5) = mass (ClF5) / molar mass (ClF5) = 5.25 g / 130.4 g/mol = 0.0403 mol
For carbon dioxide (CO2):
molar mass (CO2) = 1(12.01) + 2(16.00) = 44.01 g/mol
moles (CO2) = mass (CO2) / molar mass (CO2) = 8.81 g / 44.01 g/mol = 0.1999 mol
Next, we need to convert the temperature from Celsius to Kelvin:
T(K) = T(°C) + 273.15
T(K) = 20.6°C + 273.15 = 293.75 K
Now we can calculate the partial pressures of each gas.
Using the ideal gas law equation, rearranging for pressure:
P = nRT/V
For chlorine pentafluoride (ClF5):
P(ClF5) = (0.0403 mol)(0.0821 L·atm/(mol·K))(293.75 K) / 9 L = 0.105 atm
For carbon dioxide (CO2):
P(CO2) = (0.1999 mol)(0.0821 L·atm/(mol·K))(293.75 K) / 9 L = 0.528 atm
Therefore, the partial pressure of chlorine pentafluoride gas is 0.105 atm, and the partial pressure of carbon dioxide gas is 0.528 atm.