If 5.00 mol of hydrogen gas and 1.50 mol of oxygen gas react, what is the limiting reactant an

If 5.00 mol of hydrogen gas and 1.50 mol of oxygen gas...

If $5.00 \mathrm{~mol}$ of hydrogen gas and $1.50 \mathrm{~mol}$ of oxygen gas react, what is the limiting reactant and how many moles of water are produced according to the equation in Exercise $53 ?$

Key Concepts

Balanced Chemical Equation

A balanced chemical equation represents a chemical reaction with equal numbers of each type of atom on both sides of the equation. This balance provides the stoichiometric coefficients that indicate the mole ratios between reactants and products, which are essential for accurate stoichiometric calculations.

Mole Ratio

Derived from the balanced chemical equation, the mole ratio is the relationship between the moles of any two substances involved in the reaction. This ratio is used as a conversion factor to calculate the amounts of reactants or products, allowing for precise predictions of reaction outcomes.

Stoichiometry

Stoichiometry involves the quantitative relationships between the amounts of reactants and products in a chemical reaction. It enables predictions about the yields of products based on given quantities of reactants, ensuring that the conservation of mass is maintained throughout the reaction.

Limiting Reactant

The limiting reactant is the substance in a chemical reaction that is entirely consumed first, thus dictating the maximum amount of product that can be generated. Its identification is crucial because it determines the extent of the reaction and the final yield of the products.

Transcript

00:01 The reaction equation in this question is based on the same reaction equation that we had in the previous question.

00:10 Now, during this reaction, 5 mils of hydrogen gas reacts with 0 .15 moles of oxygen gas in order to produce a certain amount of water.

00:21 We need to identify the limiting reactant here and also calculate the number of moles of water that can form.

00:30 During this reaction.

00:33 For this purpose, we will look at two different situations in order to identify the limiting reactant first.

00:41 And that is, firstly, we will look at the number of moles of water that can be produced if we start off with 5 moles of hydrogen gas.

00:53 And secondly, we will look at the number of moles of water that can be produced when starting off with 0 .15 0 moles of oxygen gas.

01:04 We will then compare these two situations in order to identify the limiting reactant.

01:10 So firstly, in order to determine the number of moles of water that can form when starting off with 5 moles of hydrogen gas, we need to work with the mole ratio of water to hydrogen gas.

01:26 So for this purpose, we will have a look at the stoichiometric coefficients here.

01:32 For water it is 2.

01:34 For hydrogen gas it is 2.

01:36 So that mole ratio of water over hydrogen gas is 2 over 2.

01:46 We can therefore say that the number of moles of water that can form in this case will be 1 times the number of moles of water.

01:56 Hydrogen gas and this is equal to 1 times 5 moles which is just equal to 5 moles...

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