If 0.125 mol of nitrogen gas and 0.125 mol of oxygen gas react, what is the limiting reactant an

If 0.125 mol of nitrogen gas and 0.125 mol of oxygen gas...

Key Concepts

Limiting Reactant

The limiting reactant is the substance in a chemical reaction that gets completely used up first, thus determining the maximum amount of product that can be generated. It is identified by comparing the provided moles of reactants with the stoichiometric coefficients in the balanced chemical equation.

Stoichiometry

Stoichiometry involves the quantitative relationships between reactants and products in a chemical reaction. It uses the mole ratios from the balanced equation to calculate the amount of product formed from given reactant quantities.

Mole Concept

The mole is a fundamental unit in chemistry used to measure the amount of substance. It allows chemists to convert between the number of particles (atoms, molecules, etc.) and the measurable mass of a substance using Avogadro's number.

Theoretical Yield

The theoretical yield is the maximum amount of product that can be produced in a chemical reaction from given quantities of reactants, assuming complete conversion without any side reactions. It is computed based on the stoichiometric relationships once the limiting reactant has been determined.

Transcript

00:01 In this question, we need to identify the limiting reactant when 0 .125 moles of nitrogen gas reacts with 0 .125 moles of oxygen gas.

00:14 And then also calculate the number of moles of nitrogen monoxide that will form.

00:19 Now, we've used exactly the same reaction equation in the previous question.

00:24 So i've just copied the balanced equation here.

00:31 Now, in order to identify the limiting reactant, we will compare two different situations.

00:38 In the first situation, we will calculate the number of moles of nitrogen monoxide that can form from 0 .1 to 5 mils of nitrogen gas.

00:50 And in the second situation, we will calculate the number of moles of nitrogen monoxide forming from 0 .1 to 5 moles of oxygen.

01:01 And then compare these two with each other in order to identify the limiting reactant.

01:08 Now, for this purpose, we will use the mole ratio of nitrogen monoxide to nitrogen gas.

01:18 And in order to do so, we need to work with the stoichiometric coefficients here for nitrogen monoxide.

01:28 It's two for nitrogen gas.

01:30 It is one.

01:31 So the mole ratio of nitrogen monoxide to nitrogen gas will be 2 to 1.

01:39 Therefore, the number of moles of nitrogen monoxide that can form from nitrogen gas in this case will be 2 times the number of moles of nitrogen gas, which is then 2 times 0 .1 .1 .2 .2 times 0 .1.

02:01 2 5 moles and that is equal to 0 .250 .0.

02:16 On the other hand, let's see what's going to happen if we use oxygen gas here as our starting point.

02:27 Now for us to calculate the number of moles of nitrogen monoxide that can form from starting off with 0 .125 moles of oxygen gas.

02:43 We will work with the mole ratio once again...

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