If 1.00 mol of ethane gas and 3.00 mol of oxygen gas react, what is the limiting reactant and

If 1.00 mol of ethane gas and 3.00 mol of oxygen gas...

If $1.00 \mathrm{~mol}$ of ethane gas and $3.00 \mathrm{~mol}$ of oxygen gas react, what is the limiting reactant and how many moles of water are produced according to the equation in Exercise $55 ? ?$

Key Concepts

Limiting Reactant

The limiting reactant is the substance in a chemical reaction that is completely used up first, thereby preventing the reaction from continuing and limiting the amount of product that can be formed. Understanding which reactant is limiting is essential for predicting the maximum yield of a reaction.

Balanced Chemical Equations

A balanced chemical equation has the same number of atoms of each element on both sides of the reaction. It provides the necessary stoichiometric coefficients that indicate the mole ratios in which reactants combine and products form, ensuring the conservation of matter during the reaction.

Mole Ratios

Mole ratios are derived from the coefficients in a balanced chemical equation. They indicate the proportion in which reactants are consumed and products are produced, allowing for the conversion between amounts of different substances in the reaction.

Stoichiometric Calculations

Stoichiometric calculations involve using the mole ratios from a balanced chemical equation to determine the amounts of reactants needed or products formed. This concept is key for predicting yields, identifying the limiting reactant, and performing quantitative analysis in chemical reactions.

Transcript

00:01 This question is based on the equation that was used in the previous question.

00:06 I've copied the balanced equation onto this page.

00:11 And here we need to identify the limiting reactant when reacting one mole of ethanol gas with three moles of oxygen gas and then determine the number of moles of water that can be produced in this case.

00:26 So in order to compare, in order to identify the level of oxygen gas, limiting reactant, we will compare the number of moles of water that can be formed when starting off with one mole of ethanol gas, with the number of moles that can be formed in starting off with three moles of oxygen gas.

00:47 So let's first calculate the number of moles of water that can be produced when starting off with one mole of ethanol gas.

00:56 We will use the mill ratio here.

00:59 So the mil ratio of water to ethan gas will be 6 to 2, 2, which is equal to 3.

01:12 Therefore, we can say that the number of moles of water that can form is 3 times the number of moles of ethane gas.

01:21 And we know that we started off with 1 mole of ethanol gas.

01:27 So in this case, we will get an answer of three moles of water.

01:40 Now let's move on and have a look at the number of moles of water that can be produced if we start off with three moles of oxygen.

01:50 So once again, we will make use of the mole ratio year of 6 to 7 in this case.

01:57 So the mole ratio of water to oxygen is 6 to 6...

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