A sample of H₂gas (2.0 L) at 3.5 atm was combined with 1.5 L of N₂gas 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. A) 24 B) 0.56 C) 1.6 D) 1.0 E) 2.8

Question

Quizplus · Accepted Answer

We can use the ideal gas law to solve this problem: PV=nRT where P is the pressure, V is the volume, n is the number of moles, R is the gas constant, and T is the temperature. Since the temperature and the number of moles are constant, we can combine the two gases to find the total pressure in the flask: PTotal = (n1+n2)RT/VTotal where n1 and n2 are the number of moles of the first and second gases, respectively. To find the number of moles, we can use the molar mass of each gas and the given volume: n1 = V1/Vm1 n2 = V2/Vm2 where Vm1 and Vm2 are the molar volumes of each gas at STP (standard temperature and pressure). Then we can substitute these expressions into the equation for PTotal: PTotal = ((V1/Vm1)+(V2/Vm2))RT/VTotal Now we can plug in the values given in the problem: V1 = 2.0 L Vm1 = 22.4 L/mol (for H₂gas) V2 = 1.5 L Vm2 = 22.4 L/mol (for N₂gas) VTotal = 7.0 L P1 = 3.5 atm P2 = 2.6 atm R = 0.0821 L·atm/(mol·K) T = 25 °C = 298 K Plugging these values into the equation, we get: PTotal = ((2.0/22.4)+(1.5/22.4))×0.0821×298/7.0 PTotal = 1.6 atm Therefore, the answer is choice C, 1.6.

A Sample of H2 gas (2

A Sample of H₂gas (2