When 30.0 g of carbon is heated with silicon dioxide, 28.2 g of carbon monoxide is produced. W

When 30.0 g of carbon is heated with silicon dioxide, 28.2...

Key Concepts

Percent Yield

Percent yield is a measure of the efficiency of a chemical reaction. It is calculated by taking the ratio of the actual yield (the amount of product actually obtained from the reaction) to the theoretical yield (the maximum amount of product that could be generated by the reaction as predicted by the stoichiometry) and multiplying by 100 to convert it into a percentage.

Theoretical Yield

The theoretical yield is the maximum amount of product that could be formed from the given quantities of reactants based on the stoichiometric relationships in a balanced chemical equation. It is calculated under the assumption that the reaction proceeds perfectly without any losses or side reactions.

Stoichiometry

Stoichiometry involves using the coefficients in a balanced chemical equation to determine the relative amounts of reactants and products involved in the reaction. This concept is essential for converting between mass, moles, and number of particles, and for predicting the outcomes of chemical reactions.

Limiting Reactant

The limiting reactant is the substance that is completely consumed in a chemical reaction and therefore limits the amount of product that can be formed. Identifying the limiting reactant is crucial for calculating the theoretical yield and subsequently the percent yield of a reaction.

Transcript

00:01 So this question is asking us the percent yield of carbon monoxide for the reaction of silicon dioxide and carbon.

00:07 And so they actually give us the balanced equation for this reaction, which is going to be silicon dioxide is reacting with carbon to form.

00:23 There's some heat applied to form silicon solid and carbon monoxide gas.

00:35 Okay.

00:37 So this equation is already balanced, thankfully.

00:39 We don't have to do that.

00:41 So it's asking when 30 grams of carbon is heated with silicon dioxide, 28 .2 grams of carbon monoxide is produced.

00:47 It wants the percent yield of carbon monoxide.

00:50 So we need to find the theoretical yield of carbon monoxide.

00:54 So if all 30 grams of carbon reacted theoretically, how much carbon monoxide should we have gotten? so just do that, we're going to start with our 30.

01:05 We're going to start with our 30 grams.

01:07 Grams of carbon, and we are going to need to turn the scrams of carbon into moles of carbon, so we can start relating that to moles of carbon monoxide.

01:20 So to do that, we're just going to look at the periodic table, and we see that the molar mass of carbon is just 12 .01.

01:28 So one mole of carbon weighs 12 .01 grams.

01:32 So these units are now canceling out, and so we are now in moles of carbon, which is better.

01:38 So now we can use our multiple -factor to start getting into our moles of carbon monotone.

01:42 And so to do that, we see that three moles of carbon goes to two moles of carbon monoxide.

01:54 Where did we get this two and the three? we just pulled it straight from the balanced equation.

01:58 And so now these moles of carbon units cancel out.

02:01 And our unit is now in moles of carbon monoxide.

02:04 But we need grams of carbon monoxide.

02:07 So to get from moles of carbon monoxide to grams of carbon monoxide, we're going to need to find carbon monoxide's molar mass.

02:13 And so we know that carbon has a molar or an atomic weight of 12 .01, and oxygen has a molar, an atomic mass of 16.

02:24 And so adding these together, we get that carbon monoxide's molar mass is 28 .01 grams.

02:34 And so one mole of carbon monoxide weighs 28 .01 grams.

02:44 And we put this one on the bottom, the moles on the bottom of this one versus this one, because we need these units to cancel out...

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