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Answer :
Assuming ideal gas behavior, the pressure in the canister at 318 K is approximately 38.06 atm.
The pressure in the canister can be calculated using the ideal gas law equation, which is PV = nRT.
In this equation, P represents pressure, V represents volume, n represents the number of moles of gas, R represents the ideal gas constant, and T represents the temperature in Kelvin.
First, we need to convert the volume of the canister to liters, as the ideal gas law equation uses SI units. 98.1 mL is equivalent to 0.0981 liters.
Next, we need to convert the mass of argon to moles. To do this, we can use the molar mass of argon, which is approximately 39.95 g/mol. By dividing the mass of argon (46.6 g) by the molar mass, we can find the number of moles of argon in the canister.
n = mass / molar mass
n = 46.6 g / 39.95 g/mol
n = 1.167 moles
Now, we have all the necessary values to calculate the pressure. The ideal gas constant, R, is 0.0821 L·atm/(mol·K).
P = (nRT) / V
P = (1.167 mol * 0.0821 L·atm/(mol·K) * 318 K) / 0.0981 L
P = 38.06 atm
Therefore, the pressure in the canister at 318 K is approximately 38.06 atm.
It's important to note that this calculation assumes ideal gas behavior, which may not be completely accurate in real-world situations. However, the ideal gas law is a useful approximation for many systems. Additionally, make sure to double-check the units and values used in calculations to ensure accurate results.
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