Question

A 3.00-l flask is filled with gaseous ammonia, nh3. the gas pressure measured at 26.0 ∘c is 1.55 atm . assuming ideal gas behavior, how many grams of ammonia are in the flask?

Answer 1

Answer: -

A 3.00-l flask is filled with gaseous ammonia, NH₃. the gas pressure measured at 26.0 ∘c is 1.55 atm . assuming ideal gas behavior, 3.23 grams of ammonia are in the flask

Explanation: -

Volume V = 3.00 L

Pressure P = 1.55 atm

Temperature T = 26.0 °C + 273 = 299 K

We know the value of Universal gas constant R = 0.082 L atm K−1

mol−1

We use the ideal gas equation

PV = nRT

Number of moles of Ammonia n = $\frac{PV}{RT}$

= $\frac{1.55 atm x 3.00 L}{0.082 L atm K−1 x 299 K}$

= 0.19 mol

Molar mass of NH₃ = 14 x 1 + 1 x 3 = 17 g / mol

Mass of NH₃ = Molar mass of NH₃ x number of moles of NH₃

= 17 g / mol x 0.19 mol

= 3.23 g