172k views
3 votes
Container a holds 767 ml of ideal gas at 2.30 atm. container b holds 164 ml of ideal gas at 4.20 atm. if the gases are allowed to mix together, what is the resulting pressure?

User Yuanyuan
by
8.4k points

2 Answers

7 votes

Final answer:

To find the resulting pressure, use the ideal gas law equation P1V1 + P2V2 = (n1 + n2)RT, where P is pressure, V is volume, n is the number of moles, R is the ideal gas constant, and T is temperature. Plug in the given values and solve for (n1 + n2). Divide the total number of moles by the total volume to find the resulting pressure.

Step-by-step explanation:

In order to find the resulting pressure, you need to use the ideal gas law equation: PV = nRT. Since the containers are allowed to mix and there is no change in volume, the equation becomes P1V1 + P2V2 = (n1 + n2)RT. Plugging in the given values, we have (2.30 atm)(767 ml) + (4.20 atm)(164 ml) = (n1 + n2)(0.0821 atm L/mol K)(273 K). Solve for (n1 + n2) to find the total number of moles and then divide by the total volume to find the resulting pressure.

User Jay Kominek
by
7.6k points
5 votes
Maybe 2.30 am not right I may be wrong
User Shelan Perera
by
9.0k points