The volume of a gas is 24.86 liter at 50.0 Celsius and 0.80 atm, if there are 0.75 moles of the gas present.
The ideal gas law states that the pressure of gas is directly proportional to the volume and temperature of the gas.
PV = nRT
where,
P = Pressure
V = Volume in liters
n = number of moles of gas
R = Ideal gas constant
T = Temperature in kelvin
Here,
P = 0.80 atm
n = 0.75 moles
R = 0.0821 atm.L/mol.K (Ideal gas constant)
T = 50.0 Celsius
Change the temperature (Celsius into Kelvin)
Kelvin = Celsius + 273
= 50.0 + 273
= 323 Kelvin
Now put the value in above formula we get
PV = nRT
(0.80 atm) × (V) = 0.75 mol × 0.0821 atm.L/mol.K × 323 K
V = [tex]\frac{0.75\ \text{mol} \times 0.0821\ \text{atm.L/mol.K} \times 323\ K}{0.80\ \text{atm}}[/tex]
V = [tex]\frac{19.88 L}{0.8}[/tex]
V = 24.86 L
Thus, from the above conclusion we can say that The volume of a gas is 24.86 liter at 50.0 Celsius and 0.80 atm, if there are 0.75 moles of the gas present.
Learn more about the Ideal Gas here: brainly.com/question/1063475
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