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.
Question
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.
Solution
To solve this problem, we need to use the ideal gas law, which is PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the gas constant, and T is the temperature in Kelvin.
First, we need to convert the temperature from Celsius to Kelvin. The formula to convert Celsius to Kelvin is K = °C + 273.15. So, 24.9°C = 24.9 + 273.15 = 298.05 K.
Next, we need to calculate the number of moles for each gas. The formula to calculate the number of moles is n = mass / molar mass.
The molar mass of chlorine pentafluoride (ClF5) is approximately 130.45 g/mol and the molar mass of dinitrogen difluoride (N2F2) is approximately 66.02 g/mol.
So, the number of moles of ClF5 is 5.16 g / 130.45 g/mol = 0.0396 mol and the number of moles of N2F2 is 4.17 g / 66.02 g/mol = 0.0632 mol.
The total number of moles in the tank is 0.0396 mol + 0.0632 mol = 0.1028 mol.
Now we can use the ideal gas law to calculate the pressure. The gas constant R is 0.0821 L·atm/(K·mol) when the pressure is in atmospheres.
So, P = nRT / V = (0.1028 mol * 0.0821 L·atm/(K·mol) * 298.05 K) / 7.00 L = 3.53 atm.
Therefore, the total pressure in the tank is 3.53 atm.
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