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How Many Moles of Iron Will Be Produced if 3.3mol of Hydrogen Gas Reacts With 1.5mol of Iron Oxide?
In chemical reactions, the stoichiometry of a reaction determines the ratio in which reactants combine to form products. This ratio can be used to calculate the number of moles of products produced when given the number of moles of reactants. In this article, we will explore how to determine the number of moles of iron produced when 3.3 moles of hydrogen gas react with 1.5 moles of iron oxide.
To understand this reaction, let’s first take a look at the balanced chemical equation:
3 Fe2O3 + 9 H2 → 6 Fe + 9 H2O
According to this equation, three moles of iron(III) oxide (Fe2O3) react with nine moles of hydrogen gas (H2) to produce six moles of iron (Fe) and nine moles of water (H2O). From this balanced equation, we can deduce that the stoichiometric ratio between iron oxide and hydrogen gas is 1:3.
Now, let’s calculate the number of moles of iron produced when 3.3 moles of hydrogen gas react with 1.5 moles of iron oxide.
Given:
Number of moles of hydrogen gas (H2) = 3.3 mol
Number of moles of iron oxide (Fe2O3) = 1.5 mol
Since the stoichiometric ratio between iron oxide and hydrogen gas is 1:3, we can use this ratio to determine the number of moles of iron produced. We know that for every mole of iron oxide, three moles of hydrogen gas are required to react.
Number of moles of iron oxide (Fe2O3) = 1.5 mol
Number of moles of hydrogen gas required = 1.5 mol * 3 = 4.5 mol
As we have an excess of hydrogen gas (3.3 mol), we can use the moles of hydrogen gas available to calculate the number of moles of iron produced. Since three moles of hydrogen gas react with one mole of iron, we can set up a proportion to solve for the number of moles of iron:
3 mol H2/1 mol Fe = 3.3 mol H2/x mol Fe
Cross-multiplying, we get:
3 * x = 3.3 * 1
3x = 3.3
x = 3.3/3
x ≈ 1.1 mol
Therefore, approximately 1.1 moles of iron will be produced when 3.3 moles of hydrogen gas react with 1.5 moles of iron oxide.
FAQs:
Q: What is stoichiometry?
A: Stoichiometry is the branch of chemistry that deals with the quantitative relationships between reactants and products in a chemical reaction. It allows us to determine the amount of products formed from given reactants.
Q: How is stoichiometry useful in chemical reactions?
A: Stoichiometry helps us understand the amounts of reactants needed and the amounts of products formed in a chemical reaction. It allows us to make predictions about the quantities of substances involved in a reaction and helps in determining the limiting and excess reactants.
Q: What is a limiting reactant?
A: A limiting reactant is the reactant that is entirely consumed in a chemical reaction, thus limiting the amount of product that can be formed. It determines the maximum amount of product that can be obtained.
Q: What is an excess reactant?
A: An excess reactant is the reactant that is not entirely consumed in a chemical reaction. It is present in excess and remains after the limiting reactant is completely used up.
Q: How can stoichiometry be used in solving chemical problems?
A: Stoichiometry can be used to calculate the amounts of reactants and products in a chemical reaction, determine the limiting and excess reactants, and predict the yield of a reaction. It helps in understanding the relationship between reactants and products on a molecular level.
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