Chlorine forms from the reaction of hydrochloric acid with manganese(IV) oxide. The balanced equ

Chlorine forms from the reaction of hydrochloric acid with...

Key Concepts

Theoretical Yield

The theoretical yield is the maximum amount of product that can be generated by a reaction, as predicted by stoichiometric calculations assuming complete conversion of the limiting reactant. It is often expressed in grams and serves as a benchmark for reaction efficiency.

Limiting Reactant

The limiting reactant is the reactant that is completely consumed first in a chemical reaction, thereby limiting the amount of product that can be formed. Identifying it is key to calculating the theoretical yield, as only the moles of the limiting reactant determine the maximum possible amount of product.

Percent Yield

Percent yield is a measure of the efficiency of a reaction, calculated by comparing the actual yield (the amount of product actually obtained from the reaction) to the theoretical yield. It is expressed as a percentage and indicates how closely the experimental outcome approaches the ideal prediction.

Stoichiometry

Stoichiometry involves using the balanced chemical equation to understand the quantitative relationships among reactants and products in a chemical reaction. It allows calculation of how much product is formed from given amounts of reactants based on their mole ratios.

Balanced Equation

A balanced chemical equation reflects the conservation of mass by having an equal number of each type of atom on both sides of the reaction. This is crucial for accurately applying stoichiometry since the mole ratios used in calculations are derived from the coefficients in the balanced equation.

Transcript

00:01 We are given the balanced chemical equation for the reaction between manganis 4 oxide and hydrochloric acid to obtain manganis chloride, manganis 2 chloride, chlorine, and water.

00:33 We need to calculate the theoretical yield, that is the hystochometric amount or the expected amount of chlorine okay if 86 grams of manganese four oxide are mixed with 50 grams of hydroclotic acid so this would be the theoretical yield that we need to calculate and also we need to calculate the percent yield if 20 grams of chlorine of chlorine are obtained these 20 grams of chlorine are the experimental or actual yield.

01:40 Remember that the percent yield is calculated by dividing the experimental yield by the theoretical yield, and multiplying by 100%.

02:04 So, in order to find the theoretical yield of chlorine, we need first to find which one is the limiting.

02:14 Reagent, manganis -4 oxide or hydrochloric acid? because that's the substance that's going to determine the theoretical yield because it's the one that is going to completely react because it's in limiting amount.

02:28 In order to find which one is a limiting reagent, we need to establish the theoretical ratio.

02:37 And what we have is that one mole of manganis -4 oxide react with four moles of hydroxide, hydraulic acid.

02:57 We need to convert these two grams as everything is given in grams.

03:03 One mole of manganese, photoxide is 55.

03:08 We need to multiply by the molar mass of manganic peroxide, which is 55, the atomic weight of manganis plus 2 times 16, which is the atomic weight of oxygen, that's 32 grams per mole.

03:27 And then the molar mass of hydroplotidic acid which is one the atomic weight of hydrogen plus 35 .5 the atomic weight of clothing.

03:43 Okay, so we are left with grams after we cancel the moles and because this is a mass ratio that we are trying to get.

03:57 So 55 plus 32 is 87 grams of magnesium of magnesium.

04:09 Is for oxide and then here it would be 36 .5 times 4, 146 grams of hydrochloric acid.

04:27 This ratio is 87 divided by 146.

04:32 It is 0 .6.

04:37 Now we have to calculate the experimental ratio in order to compare and determine which which one is a limiting reaction.

04:47 Experimental ratio is the grams of manganese for oxide that are mixed with the grams of hydrochloric acid.

04:59 And what we have is 86 grams divided by 50 grams.

05:12 And the ratio is 1 .72.

05:19 So the theoretical ratio is less than the experimental ratio because experimental ratio is greater than the theoretical ratio, we need to decrease the experimental ratio.

05:36 We need to decrease this number to make it close or equal to the theoretical ratio.

05:43 The way we decrease this number, we decrease this ratio is by decreasing the denominator.

05:49 When you decrease, sorry, by increasing the denominator.

05:53 So by increasing this number here, this denominator, we decrease the ratio...

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