A 75.0 L steel tank at 20.0°C contains acetylene gas,C₂H₂,at a pressure of 1.39 atm.Assuming ideal behavior,how many grams of acetylene are in the tank?

Question

Quizplus · Accepted Answer

First, we need to convert the pressure from atm to Pa:

1.39 atm x 101325 Pa/atm = 140236 Pa

Using the Ideal Gas Law equation, we can calculate the number of moles of acetylene in the tank:

PV = nRT

n = (PV) / (RT)

n = (140236 Pa)(75.0 L) / [(8.31 J/mol*K)(293 K)]

n = 4.05 mol

Finally, we can convert moles to grams using the molar mass of acetylene:

4.05 mol x 26.04 g/mol = 105.02 g, rounded to 113 g.

A 750 L Steel Tank at 20