Answer :
The pressure in the 4.50 L tank with 2.00 moles of oxygen at 39.3 °C is approximately 11.57 bar.
To calculate the pressure in bar of a gas, we can use the ideal gas law equation:
PV = nRT,
where P represents 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.
First, let's convert the temperature from Celsius to Kelvin:
T = 39.3 °C + 273.15 = 312.45 K.
Now, let's substitute the given values into the ideal gas law equation:
P * 4.50 L = 2.00 mol * 0.08314 L·bar/mol·K * 312.45 K.
Simplifying the equation:
P * 4.50 L = 52.04644 bar.
Finally, we can isolate the pressure by dividing both sides of the equation by 4.50 L:
P = 52.04644 bar / 4.50 L.
Calculating this value:
P ≈ 11.57 bar.
Therefore, the pressure in the 4.50 L tank with 2.00 moles of oxygen at 39.3 °C is approximately 11.57 bar.
It's important to note that the ideal gas law assumes that the gas behaves ideally, meaning that there are no intermolecular forces or volume occupied by the gas molecules themselves.
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