When heated, lithium reacts with nitrogen to form lithium...

When heated, lithium reacts with nitrogen to form lithium nitride: $$6 \mathrm{Li}(s)+\mathrm{N}_{2}(g) \longrightarrow 2 \mathrm{Li}_{3} \mathrm{~N}(s)$$What is the theoretical yield of $\mathrm{Li}_{3} \mathrm{~N}$ in grams when $12.3 \mathrm{~g}$ of $\mathrm{Li}$ are heated with $33.6 \mathrm{~g}$ of $\mathrm{N}_{2} ?$ If the actual yield of $\mathrm{Li}_{3} \mathrm{~N}$ is $5.89 \mathrm{~g},$ what is the percent yield of the reaction?

When heated, lithium reacts with nitrogen to form lithium nitride:
$$6 \mathrm{Li}(s)+\mathrm{N}_{2}(g) \longrightarrow 2 \mathrm{Li}_{3} \mathrm{~N}(s)$$What is the theoretical yield of $\mathrm{Li}_{3} \mathrm{~N}$ in grams when $12.3 \mathrm{~g}$ of $\mathrm{Li}$ are heated with $33.6 \mathrm{~g}$ of $\mathrm{N}_{2} ?$ If the actual yield of $\mathrm{Li}_{3} \mathrm{~N}$ is $5.89 \mathrm{~g},$ what is the percent yield of the reaction?

Key Concepts

Stoichiometry

Stoichiometry is the quantitative relationship between reactants and products in a chemical reaction, based on the balanced chemical equation. It involves converting grams to moles and using mole ratios to calculate the amount of product formed from given reactant quantities.

Limiting Reactant

The limiting reactant is the substance that is completely consumed first during a chemical reaction, thereby determining the maximum amount of product that can be formed. Calculating the limiting reactant is essential for accurately predicting the theoretical yield of the reaction.

Theoretical Yield

The theoretical yield is the maximum possible amount of product that can be produced in a reaction, as calculated from the stoichiometry of the balanced equation assuming complete conversion of the limiting reactant. It is typically expressed in grams and serves as a benchmark for efficiency comparisons.

Percent Yield

Percent yield is a measure of the efficiency of a reaction and is calculated by dividing the actual yield (the experimentally obtained product amount) by the theoretical yield and then multiplying by 100. It indicates the extent to which the reaction proceeds under given conditions.

Transcript

00:05 We have given information 6 lithium in solid state plus nitrogen in gas state 2 lithium 3 nitrogen in solid state and the mass of lithium is mass of lithium is equal to 12.

01:15 1 .3 gram and the mass of nitrogen is equal to 33 .6 gram.

01:38 The mass and the actual yield of li -3 lithium nitrate is equal to 5 .89 gram.

02:11 We have to find the theoretical yield of li3 and the percent yield.

02:51 So first we have to find the limiting reactant.

03:23 The number of moles of lithium is number of mores of lithium is equal to mass of lithium divided by molar mass of lithium is equal to by putting the mass values 12 .3 gram per mole is the given mass of lithium and 6 .941 gram per mole is the molar mass of lithium is equal to 1 .8 mole.

04:33 Gram gram oh sorry here is only mole because here we we have put the value of oh sorry mass of lithium so mass of lithium the unit of mass of lithium is gram so here we can sell gram gram so mole is left here so the unit of number of moles is equal to member of moles of is equal to 1 .8 mole of lithium and the number of moles of nitrogen is number of of nitrogen is equal to given mass of nitrogen divided by molar mass of nitrogen is equal to given mass of nitrogen is 33 .6.

06:09 Gram and molar mass of nitrogen is 28 .014 gram per mole.

06:20 Here you can sell gram gram and the value is 1 .2 mole with the calculated value and 6 moles of lithium reacts with 1 .3 mole of of nitrogen therefore 1 .8 moles of lithium will react with 1 .8 divided by 6 is equal to 0 .3 moles of nitrogen since there is access so the limiting reactant is lithium.

08:42 Now we will calculate the theoretical yield of lithium nitrate.

09:17 And 6 moles of lithium produce 2 moles of light 3 in...

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