A sample of He gas (3.0 L)at 5.6 atm and 25 °C was combined with 4.5 L of Ne gas at 3.6 atm and 25 °C at constant temperature in a 9.0 L flask. The total pressure in the flask was ________ atm. Assume the initial pressure in the flask was 0.00 atm and the temperature upon mixing was 25 °C.
A)2.6
B)9.2
C)1.0
D)3.7
E)24

Question

Quizplus · Accepted Answer

To solve this problem, we can use the ideal gas law:

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 in Kelvin.

Since the temperature and amount of gas do not change during the mixing process, we can combine the two gases using the following equation:

(P1V1 + P2V2) / (V1 + V2) = Ptotal

where P1 and V1 are the pressure and volume of the first gas, and P2 and V2 are the pressure and volume of the second gas.

Plugging in the numbers, we get:

((5.6 atm) × (3.0 L) + (3.6 atm) × (4.5 L)) / (3.0 L + 4.5 L) = Ptotal

Ptotal = 3.7 atm

Therefore, the total pressure in the flask is 3.7 atm, or choice D.

A Sample of He Gas (3