If 5.00 mol of hydrogen gas and 5.00 mol of oxygen gas react, what is the limiting reactant an

If 5.00 mol of hydrogen gas and 5.00 mol of oxygen gas...

If $5.00 \mathrm{~mol}$ of hydrogen gas and $5.00 \mathrm{~mol}$ of oxygen gas react, what is the limiting reactant and how many moles of water are produced from the reaction?
$$2 \mathrm{H}_{2}(g)+\mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{H}_{2} \mathrm{O}(l)$$

Key Concepts

Molar Ratios

Molar ratios are derived from the coefficients of a balanced chemical equation and indicate the proportion of moles of each substance involved in the reaction. They serve as conversion factors to relate the amounts of different chemicals used or produced in the reaction.

Stoichiometry

Stoichiometry is the study of the quantitative relationships between reactants and products in a chemical reaction. It involves using the balanced equation to calculate how much of each reactant is needed or how much product can be formed.

Limiting Reactant

The limiting reactant is the substance in a chemical reaction that is completely consumed first, determining the maximum amount of product that can be formed. It is identified by comparing the mole ratios of the reactants, as provided by the balanced chemical equation, to the actual quantities available.

Transcript

00:01 In problem 53, if 5 mol of hydrogen gas and 5 mole of oxygen gas react, what is the limiting reactant and how many mole of water are produced from the reaction? so this question is from chapter 10, chemical equation calculations.

00:18 So in this question, we have given the reaction in which 2 moles of hydrogen gas are react with the 1 mole of oxygen gas that can form 2 mole of water.

00:29 So we have given that the moles of hydrogen gas that is 5 mole and also moles of oxygen gas that is also 5 mole.

00:56 So this information given in the question.

00:59 So now first of all we understand what is the limiting reactant.

01:03 So the limiting the reactant, the reactant that is the reactant that is the reactant that is completely used up or consume in the chemical reaction and the limiting reactant that is lr determine how much product can be formed so that mean the amount of product can be found from the limiting reactant only so the reactant that is used up first in a chemical reaction it mean the reactant that restrict the amount of product that can be produced that is called the limiting reactant.

02:35 So now coming to the question part, that we have given two moles of hydrogen gas, react with the one mole of oxygen gas that can form two mole of water.

02:49 Okay, so now first of all, we have to identify which is the limiting reactant out of hydrogen and oxygen, which is the limiting reactant.

02:58 So now as we can see that this 1 mole or 2 required 2 mole of hydrogen and for 5 mole o2 required how many moles of hydrogen so it is simply 2 by 1 into 5 so that means 10 mole of hydrogen that is required or consume but present present or given malls or of hydrogen that is 5 moles...

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