A sample of H₂ gas (2.0 L)at 3.5 atm was combined with 1.5 L of N₂ gas at 2.6 atm pressure at a constant temperature of 25 °C into a 7.0 L flask. The total pressure in the flask is ________ atm. Assume the initial pressure in the flask was 0.00 atm and the temperature upon mixing was 25 °C. A)0.56 B)2.8 C)1.0 D)1.6 E)24

Question

Quizplus · Accepted Answer

First, we need to calculate the number of moles of each gas using the ideal gas law: n(H₂) = (3.5 atm) x (2.0 L) / (0.0821 L atm/mol K) x (298 K) = 0.311 mol n(N₂) = (2.6 atm) x (1.5 L) / (0.0821 L atm/mol K) x (298 K) = 0.284 mol Next, we can use Dalton's law of partial pressures to find the total pressure in the flask: P(total) = P(H₂) + P(N₂) P(total) = (0.311 mol / 3.5 L) + (0.284 mol / 1.5 L) P(total) = 0.073 + 0.189 P(total) = 0.262 atm However, we need to remember that the final volume of the gas mixture is 7.0 L, not just the sum of the initial volumes. So we need to adjust the partial pressures accordingly: P(H₂) = (0.073 / 2.0 L) x 7.0 L = 0.256 atm P(N₂) = (0.189 / 1.5 L) x 7.0 L = 0.948 atm Therefore, the total pressure in the flask is: P(total) = 0.256 atm + 0.948 atm = 1.204 atm, which is closest to choice D (1.6 atm).

A Sample of H2 Gas (2

A Sample of H₂ Gas (2