Final answer:
To determine the pressure exerted by the SF₆ gas in a 500 mL flask at 25°C, we can use the ideal gas law equation PV = nRT. By substituting the given values and solving the equation, we find that the pressure is approximately 9.37 atm.
Step-by-step explanation:
To determine the pressure exerted by the SF₆ gas, we can use the ideal gas law equation, which states that PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature in Kelvin.
We are given the mass of the gas (5.0 grams) and the volume of the flask (500 mL), which we can convert to liters (0.5 L). We also need to convert the temperature from Celsius to Kelvin by adding 273.15.
Once we have the mass of the gas, we can use the molar mass of SF₆ (146.06 g/mol) to calculate the number of moles. Finally, we can substitute the values into the ideal gas law equation to solve for the pressure.
Using the given values:
n = (5.0 g) / (146.06 g/mol) = 0.034 mol
V = 0.5 L
T = 25°C + 273.15 = 298.15 K
R = 0.0821 L·atm/(mol·K)
Solving the ideal gas law equation for P:
PV = nRT
P(0.5 L) = (0.034 mol)(0.0821 L·atm/(mol·K))(298.15 K)
P = (0.034 mol)(0.0821 L·atm/(mol·K))(298.15 K) / (0.5 L)
P ≈ 9.37 atm
Therefore, the pressure exerted by the SF₆ gas is approximately 9.37 atm.