Curious Carl and his lab partner were handed a 2 liter sealed flask containing two gases, neon and argon. The partial of each gas was 101.3 kPa. Carl and his partner then forced the gases into a smaller, 1 liter container.
What is the new partial pressure of each gas and the total pressure exerted on the container?
es
A)
50.65 kPa; 101.3 kPa
B)
101.3 kPa; 202.6 kPa
C)
202.6 kPa; 405.2 kPa
D)
202.6 kPa; 202.6 kPa

it's difficult but i think the answer is

first, consult an activity series chart to determine if al is more reactive than fe. it is, so it will replace the fe. now, one can continue with the problem.

next, make sure you have a correctly balanced equation.

3feo + 2al ==> 3fe + al2o3

now, determine which reactant (feo or al) is in limiting supply.

moles feo present = 125 g x 1 mole/71.8 g = 1.74 moles

moles al present = 25.0 g x 1 mole/26.98 g = 0.927 moles

since from the balanced equation, it take 3 mol feo for every 2 mol al, al will be limiting.

you can determine this simply by dividing moles of each by their coefficient in the balanced equation. for example: 1.74/3 = 0.58 and 0.927/2 = 0.464. al is less, so it is limiting.

finally, using the stoichiometry in the balanced eq. determine mass of fe that can be produced from 0.927 moles of al.

0.927 moles al x 3 moles fe/2 moles al x 55.8 g/mole = 77.6 g

the answers would be

the first one and the second one