Consider the following equilibrium reaction at a given temperature: A (aq) + 3 B (aq) ⇌ C (aq) + 2 D (aq) Kc = 178. If initially the concentrations of the chemical species are as follows: [A]o = 0.364 M [B]o = 0.170 M [C]o = 0.132 M [D]o = 0.932 M to which direction will the reaction run to reach equilibrium?

The reaction proceed toward product side or in forward direction.

Explanation:

is the constant of a certain reaction at equilibrium while is the quotient of activities of products and reactants at any stage other than equilibrium of a reaction.

For the given chemical reaction:

The expression of for above equation follows:

We are given:

Putting values in above equation, we get:

We are given:

There are 3 conditions:

As, , the reaction will be favoring product side.

Hence, the reaction proceed toward product side or in forward direction.

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

a corroding iron, if that's one of your choices