Question

Can can someone lease check my answers and tell me if im right???

You have four fixed-volume containers at STP. Container A has 0.5 mol of gas in 11.2 L. Container B has 2 mol of gas in 22.4 L. Container C has 1 mol of gas in 22.4 L. Container D has 2 mol of gas in 11.2 L. Which of the four containers have equal pressures?
(Points : 3)
A and C

A and B

B and C

C and D
*****MY answer is A

Answer 1

Technically, this question is badly worded. If all 4 containers were at STP, then all 4 containers would have the same pressure. So I'll assume instead that all 4 containers are at the same temperature, and then use the ideal gas law to determine the relative internal pressures of each container.

The idea gas law is
PV = nRT
where
P = Pressure
V = Volume
n = number of moles
R = Ideal gas constant
T = Absolute temperature

Since all the containers are at the same temperature, we can ignore the R and T parts of the formula and substitute some value K for constant. So we get PV = nK

Now solve for P
PV = nK
P = nK/V

From the above, you can see that the pressure is proportional to the number of moles divided by the volume. So let's calculate that value for each container.
Container A: 0.5 / 11.2 = 0.044642857
Container B: 2 / 22.4 = 0.089285714
Container C: 1 / 22.4 = 0.044642857
Container D: 2 / 11.2 = 0.178571429
So as you can see, the pressures in containers A and C are the same, which is the first available option, so you are correct.