A 55.0-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 to units of Pascals:
1.39 atm x 101,325 Pa/atm = 140,130 Pa

Next, we can use the ideal gas law equation to solve for the number of moles of acetylene gas in the tank:
PV = nRT
n = PV/RT
n = (140,130 Pa)(55.0 L)/(8.31 J/mol•K)(293 K)
n = 6.86 mol

Finally, we can convert moles to grams using the molar mass of acetylene gas:
m = nM
m = (6.86 mol)(26.04 g/mol)
m = 178.5 g

Therefore, the answer is C) 82.8 g.

A 550-L Steel Tank at 20