3. Determine if the following system is at equilibrium. If not, in which direction will the system need to shift to reach equilibrium? SO2Cl2(g) ⇌ SO2(g)+Cl2(g) [SO2Cl2] = 0.12 M, [Cl2] = 0.16 M and [SO2] = 0.050 M. Kc for the reaction is 0.078.

The system need to shift to the right

Explanation:

For the reaction:

SO2Cl2(g) ⇌ SO2(g)+Cl2(g)

Reaction quotient, Q, is:

Q = [SO2] [Cl2] / [SO2Cl2]

If Q = Kc, the system is in equilibrium, if Q > Kc, the system need to shift to the left, if Q < Kc,  the system need to shift to the right.

Replacing:

Q = 0.050 M×0.16 M / 0.12 M

Q = 0.067

As Kc = 0.078, Q < Kc, the system need to shift to the right.

I hope it helps!

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