Question
The air inside a balloon is at a temperature of 300 K and a pressure of 2.00 atm. If the balloon contains 1.60 mol of air, what is its volume?
R= 0.0821 L atm/mol K
PV = nRT
R= 0.0821 L atm/mol K
PV = nRT
Answers
GPT 3.5
To find the volume of the balloon, we can use the ideal gas law equation:
PV = nRT
Where:
P = pressure = 2.00 atm
V = volume (unknown)
n = number of moles = 1.60 mol
R = gas constant = 0.0821 L atm/mol K
T = temperature = 300 K
Plugging in the values:
(2.00 atm)(V) = (1.60 mol)(0.0821 L atm/mol K)(300 K)
Simplifying:
2.00V = 39.312 L atm
Dividing both sides by 2.00:
V = 19.656 L
Therefore, the volume of the balloon is approximately 19.656 L.
PV = nRT
Where:
P = pressure = 2.00 atm
V = volume (unknown)
n = number of moles = 1.60 mol
R = gas constant = 0.0821 L atm/mol K
T = temperature = 300 K
Plugging in the values:
(2.00 atm)(V) = (1.60 mol)(0.0821 L atm/mol K)(300 K)
Simplifying:
2.00V = 39.312 L atm
Dividing both sides by 2.00:
V = 19.656 L
Therefore, the volume of the balloon is approximately 19.656 L.
a
19.7 L
b
1.7 L
c
7.70 L
d
30.8 L
GPT 3.5
The correct answer is a) 19.7 L.