Solid zinc metal reacts with sulfuric acid to form hydrogen gas and an aqueous solution of zinc (II) sulfate. Express your answer as a balanced chemical equation. Identify all of the phases in your answer.

Answer : The balanced chemical reaction will be:

Explanation :

Balanced chemical reaction : It is defined as the reaction in which the number of atoms of individual elements present on reactant side must be equal to the product side.

When solid zinc metal reacts with sulfuric acid to then it forms hydrogen gas and an aqueous solution of zinc (II) sulfate as a product.

This reaction is a single displacement reaction in which more reactive metal displaces least reaction metal from its solution.

The balanced chemical reaction will be:

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