In the chemical reaction below, calcium (ca) and water (h2o) react to form calcium hydroxide (ca(oh)2) and hydrogen gas (h2).ca (s) 2h2o (l) → ca(oh)2 (aq) h2 (
g. calcium and water are the reactants in this chemical reaction, whereas calcium hydroxide and hydrogen gas are the products that are formed. once the reaction reaches completion, finish the
a. the products of the reaction will have changed back into the reactants.
b. the total mass of the products will be greater than the original mass of the reactants.
c. the total mass of the products will be equal to the original mass of the reactants.
d. the total mass of the products will be less than the original mass of the reactants.

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

it should be all of them because it asks if you included all of those in your answer

explanation: