A 21.0 l cylinder contains nitrogen gas at 14.4°C in 701 tour how many moles of nitrogen are in the cylinder

Answer 1

To solve this problem, we can use the ideal gas law equation:

PV = nRT

Where:
P = pressure (in atm)
V = volume (in liters)
n = number of moles
R = ideal gas constant (0.0821 L·atm/mol·K)
T = temperature (in Kelvin)

First, we need to convert the temperature from Celsius to Kelvin:

T(K) = T(°C) + 273.15
T(K) = 14.4 + 273.15
T(K) = 287.55 K

Next, we need to convert the pressure in torr to atm:

1 atm = 760 torr
701 torr / 760 torr = 0.9237 atm

Now our equation becomes:

(0.9237 atm)(21.0 L) = n(0.0821 L·atm/mol·K)(287.55 K)

19.497 L·atm = 23.589 n
n = 19.497 L·atm / 23.589 mol
n ≈ 0.827 moles

Therefore, there are approximately 0.827 moles of nitrogen in the cylinder.