The airbag is the car works using the Ideal gas law. When an airbag is inflated, the nitrogen gas has a pressure of 23.011 atm, a temperature of 39.00 degreeC, and a volume of 78.00 mL. What is the number of moles of the nitrogen gas? (R =0.08206 L.atm/K.mol).
0.56 moles
56812 moles
0.070 moles
7101.00 moles
0.070 moles (rounded to three significant figures)
To solve this problem, we can use the ideal gas law equation:
PV = nRT
Where:
P = pressure = 23.011 atm
V = volume = 78.00 mL (convert to liters by dividing by 1000: 78.00 mL = 0.078 L)
n = number of moles (unknown)
R = ideal gas constant = 0.08206 L.atm/K.mol
T = temperature in Kelvin (convert from Celsius to Kelvin: 39.00 °C + 273.15 = 312.15 K)
Plugging these values into the equation, we have:
(23.011 atm) * (0.078 L) = n * (0.08206 L.atm/K.mol) * (312.15 K)
1.7928 atm*L = 25.4762 * n
n = (1.7928 atm*L) / (25.4762)
n = 0.070 moles
Therefore, the number of moles of nitrogen gas in the airbag is 0.070 moles. So the correct answer is option C: 0.070 moles.