Consider the reaction: 2 CH3 OH(g)+3 O2(g) →2 CO2(g)+4 H2 O(g) Each of the molecular diagrams re

Consider the reaction: 2 CH3 OH(g)+3 O2(g) →2 CO2(g)+4 H2...

Consider the reaction: $$2 \mathrm{CH}_{3} \mathrm{OH}(g)+3 \mathrm{O}_{2}(g) \rightarrow 2 \mathrm{CO}_{2}(g)+4 \mathrm{H}_{2} \mathrm{O}(g)$$ Each of the molecular diagrams represents an initial mixture of the reactants. How many $\mathrm{CO}_{2}$ molecules would be formed from the reaction mixture that produces the greatest amount of products?

Consider the reaction:
$$2 \mathrm{CH}_{3} \mathrm{OH}(g)+3 \mathrm{O}_{2}(g) \rightarrow 2 \mathrm{CO}_{2}(g)+4 \mathrm{H}_{2} \mathrm{O}(g)$$
Each of the molecular diagrams represents an initial mixture of the reactants. How many $\mathrm{CO}_{2}$ molecules would be formed from the reaction mixture that produces the greatest amount of products?

Key Concepts

Stoichiometry

Stoichiometry involves using the balanced chemical equation to understand the quantitative relationships between reactants and products. It allows us to calculate how the moles of reactants determine the number of molecules or moles of products formed according to the reaction’s stoichiometric coefficients.

Limiting Reactant

The limiting reactant is the substance that is completely used up first in a chemical reaction, thereby determining the maximum amount of product that can be formed. Identifying the limiting reactant by comparing the available quantities with the stoichiometric requirements is crucial for predicting the reaction yield.

Balanced Chemical Equation

A balanced chemical equation provides the exact mole ratios in which reactants combine to form products, ensuring that the conservation of mass is maintained. It is essential for performing stoichiometric calculations and for determining which reactant is limiting in a given reaction.

Mole Ratios

Mole ratios are derived directly from the coefficients in a balanced chemical equation and indicate how many moles of each reactant are needed to produce a given number of moles of product. They serve as the fundamental basis for calculating the amounts of products formed from the reactants available.

Transcript

00:01 In this question we're going to be looking at stoichiometry and of particular interest in this question are the ratio.

00:13 So say we've got a reaction a, b to form c and what we are saying here we're saying b, we're saying b, let's say a is in greater amounts than b.

00:33 We are saying b is the limiting reactant and the limiting reactant is what limits or detainting the amount of products that is going to be formed.

00:43 So if there is a lot of a than b, at the end of the day, we are going to consume all of the b and we'll still have some a that is going to be left.

00:54 So even if we have a, there is no longer any more of b that is going to react to form the product.

01:02 So this is how the b is limiting this creator.

01:07 Because if we still have a lot of a, there is no more.

01:11 B to react anymore to produce any product.

01:14 So at the end of the day, these products depend on the amount of b.

01:18 That is the product depends on the limiting reactant.

01:24 So coming to what we've been given here, say we've got 2ch 3 or h that is relating with 3o2, form 2co2 and 4h2o2.

01:43 So looking at this, we've got three molecules.

01:47 Molecules of o2 and if we are to compare ch3 oh against o2 here we are going to have 3 against 3 so at the end of the day we are going to need 4 .5 molecules of oxygen that is oxygen is the limiting reactant and if we are to use that information and look at oxygen against the amount of co2 that is going to be formed.

02:34 We have 3 here and we have 2 here...

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