NH3 gas is pumped into the reservoir of a
refrigeration unit at a pressure of 2.20 atm.
The capacity of the reservoir is 20.4 L. The
temperature is 26.1◦C. What is the mass of
the gas?
Answer in units of g
Use PV = nRT and solve for n = mols of gas, then n = grams/molar mass and solve for g.
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To find the mass of NH3 gas, 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.
First, we need to convert the given pressure from atm to Pa (Pascals) and the temperature from Celsius to Kelvin.
1 atm = 101325 Pa
Temperature in Kelvin (K) = 26.1 + 273.15
Given:
Pressure (P) = 2.20 atm = 2.20 * 101325 Pa
Volume (V) = 20.4 L
Temperature (T) = 26.1 ◦C = 26.1 + 273.15 K
Now, let's rearrange the ideal gas law equation to solve for n (number of moles):
n = PV / RT
Substituting the given values into the equation:
n = (2.20 * 101325) * (20.4 / 1000) / (8.314 * (26.1 + 273.15))
Simplifying the equation:
n = 0.182909
To find the mass of the gas, we need to know the molar mass of NH3, which is 17.031 g/mol.
Now, we can calculate the mass of the gas:
Mass = number of moles (n) * molar mass (m)
Mass = 0.182909 * 17.031
The mass of the NH3 gas is approximately 3.116 grams.