9.0 g of iron is reacted with 9.0 g of water according to the chemical equation shown below.Which one of the following statements is FALSE?
3 Fe(s) + 4 H₂O(l) → Fe₃O₄(s) + 4 H₂(g)

Question

9.0 g of iron is reacted with 9.0 g of water according to the chemical equation shown below.Which one of the following statements is FALSE? 3 Fe(s)+ 4 H₂O(l)→ Fe₃O₄(s)+ 4 H₂(g)

Quizplus · Accepted Answer

To determine the limiting reactant, we need to calculate the amount of product each reactant can produce. Using the given masses, we can calculate the moles of each reactant: 
moles of Fe = 9.0 g / 55.85 g/mol = 0.161 moles 
moles of H2O = 9.0 g / 18.015 g/mol = 0.499 moles

Using the balanced equation, we can determine that 3 moles of Fe react with 4 moles of H2O to produce 1 mole of FeS13O4. Therefore, the amount of product that can be formed from the available reactants is:

- Fe: 0.161 moles Fe x (1 mol FeS13O4 / 3 mol Fe) = 0.0537 moles FeS13O4
- H2O: 0.499 moles H2O x (1 mol FeS13O4 / 4 mol H2O) = 0.125 moles FeS13O4

Since Fe can only produce 0.0537 moles of product while H2O can produce 0.125 moles, H2O is the limiting reactant. This means that Fe is in excess and there will be some Fe left over after the reaction is complete.

Using the amount of limiting reactant (0.499 moles H2O) and the stoichiometry of the balanced equation, we can calculate the theoretical yield of FeS13O4:

- 0.499 moles H2O x (1 mol FeS13O4 / 4 mol H2O) x 232.14 g/mol = 29.2 g FeS13O4

Therefore, the correct answer is D) Water is the limiting reactant. Statement A is true based on the stoichiometry of the equation and the amount of excess Fe can be calculated using the same approach as above. Statement B is false because all of the H2O is consumed in the reaction. Statement C is true because mass is always conserved in a chemical reaction.

90 G of Iron Is Reacted with 9