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Is a gas at 1.4 atm pressure and 15 L volume, at -10 degrees Celsius and 1 mole the gas, an ideal gas, why or why not (Ideal gas constant is 0.0820574)
To determine whether or not the gas can be considered ideal, we can use the ideal gas law equation:
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.
First, we need to convert the temperature from Celsius to Kelvin. The conversion formula is: Kelvin = Celsius + 273.15.
So, -10 degrees Celsius is equal to -10 + 273.15 = 263.15 Kelvin.
Now, let's substitute the given values into the ideal gas law equation:
(1.4 atm) * (15 L) = (1 mole) * (0.0820574 L.atm/mol.K) * (263.15 K)
21 atm.L = 21.58911 atm.L
The value on the left side of the equation is equal to the value on the right side, indicating that the gas follows the ideal gas behavior. Therefore, the gas at 1.4 atm pressure, 15 L volume, -10 degrees Celsius, and 1 mole can be considered an ideal gas.