A balloon contains 0.950 mol of nitrogen gas and has a volume of 25.5 L. How many grams of N2 should be released from the balloon to bring the volume to 17.3 L?
Answer: Mass released = 8.6 g Explanation: Given data: Initial number of moles nitrogen= 0.950 mol Initial volume = 25.5 L Final mass of nitrogen released = ? Final volume = 17.3 L Solution: Formula: V₁/n₁ = V₂/n₂ 25.5 L / 0.950 mol = 17.3 L/n₂ n₂ = 17.3 L× 0.950 mol/25.5 L n₂ = 16.435 L.mol /25.5 L n₂ = 0.644 mol Initial mass of nitrogen: Mass = number of moles × molar mass Mass = 0.950 mol × 28 g/mol Mass = 26.6 g Final mass of nitrogen: Mass = number of moles × molar mass Mass = 0.644 mol × 28 g/mol Mass = 18.0 g Mass released = initial mass - final mass Mass released = 26.6 g - 18.0 g Mass released = 8.6 g
