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Problem: What is the limiting reactant and theoretical yield if 4.00 grams of hydrogen react with 20.0 grams of oxygen according to the reaction below?

\[
2H_2(g) + O_2(g) \rightarrow 2H_2O(g)
\]

Solution work:
A. 22.5 g of water is the theoretical yield and hydrogen is the limiting reactant.
B. 35.8 g of water is the theoretical yield and oxygen is the limiting reactant.
C. 35.8 g of water is the theoretical yield and hydrogen is the limiting reactant.
D. 22.5 g of water is the theoretical yield and oxygen is the limiting reactant.

Answer :

Final answer:

In the given chemical reaction, oxygen is the limiting reactant as it is consumed before hydrogen. The theoretical yield, the maximum amount of product that can be made in the chemical reaction, is 18.0g of water.

Explanation:

The problem is a basic stoichiometry problem from chemistry. First, we need to identify the limiting reactant, the reactant that gets completely consumed in the chemical reaction and determines the maximum amount of product that can be formed - the theoretical yield. We do this by comparing the mole-to-mole ratio of the reactants. For the reaction 2H2 + O2 → 2H2O, 1 mole of oxygen reacts with 2 moles of hydrogen to produce 2 moles of water.

When we convert grams to moles, using molar masses of hydrogen and oxygen, we see that we have 2 moles of hydrogen and somewhat less than 1 mole of oxygen. Oxygen, therefore, is the limiting reactant. To find out the theoretical yield we multiply the moles of the limiting reactant by the stoichiometric coefficients, which gives us the theoretical amount of water that can be produced in the reaction. Thus, the answer here is 18.0 g water is the theoretical yield and oxygen is the limiting reactant.

Learn more about Stoichiometry here:

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