Ethylene (C2 H4), an important industrial organic chemical,...

Ethylene $\left(\mathrm{C}_{2} \mathrm{H}_{4}\right),$ an important industrial organic chemical, can be prepared by heating hexane $\left(\mathrm{C}_{6} \mathrm{H}_{14}\right)$ at $800^{\circ} \mathrm{C}:$$$\mathrm{C}_{6} \mathrm{H}_{14} \longrightarrow \mathrm{C}_{2} \mathrm{H}_{4}+\text { other products }$$ If the yield of ethylene production is 42.5 percent, what mass of hexane must be reacted to produce $481 \mathrm{~g}$ of ethylene?

Ethylene $\left(\mathrm{C}_{2} \mathrm{H}_{4}\right),$ an important industrial organic chemical, can be prepared by heating hexane $\left(\mathrm{C}_{6} \mathrm{H}_{14}\right)$ at $800^{\circ} \mathrm{C}:$$$\mathrm{C}_{6} \mathrm{H}_{14} \longrightarrow \mathrm{C}_{2} \mathrm{H}_{4}+\text { other products }$$
If the yield of ethylene production is 42.5 percent, what mass of hexane must be reacted to produce $481 \mathrm{~g}$ of ethylene?

Key Concepts

Stoichiometry

Stoichiometry is the quantitative relationship between reactants and products in a chemical reaction. It allows one to determine the amounts of substances consumed and produced based on the balanced chemical equation and the mole ratios of reactants to products.

Molar Mass Calculation

Molar mass is the mass of one mole of a given substance, expressed in grams per mole. It is crucial for converting between the mass of a substance and the number of moles, which is necessary for performing stoichiometric calculations.

Percent Yield

Percent yield is a measure of the efficiency of a chemical reaction and is calculated by comparing the actual yield (the amount of product obtained) to the theoretical yield (the maximum amount of product expected based on stoichiometry). This concept is key when determining the required amount of reactants needed to obtain a desired quantity of product.

Transcript

00:04 Given information for the above problem, basan is c6h14 is reactant and product is c2h4 plus other products.

00:35 Other products.

00:44 The percentage yield of yield of c2h4 is 42 .5.

01:04 5 % the actual yield of c2h4 is 4 81 gram we have to find the mass of c6 h14 first we have to find the mass of c6 h14 first we have to find the theoretical yield yield and number of moles of c to h4 percent yield is equal to the actual yield divided by the theoretical yield multiply hundred percent so the actual yield the theoretical yield is equal to the theoretical yield divided by percent yield multiply 100 percent so the value of actual yield is 4 at 1 gram divided by value of percent yield is 42 .5 percent multiply hundred percent is equal to 113 one is equal to 113 1 .76 gram percent is cancelled with percent and that is gram the molar mass of molar mass of c2h4 is molar mass of c2h4 is equal to 2 2 into molar mass of carbon plus 4 into molar mass of hydrogen so molar molar mass of carbon is 2 into 12 .0 .01 gram per mole plus 4 into in molar mass of hydrogen is 1 .008 gram per mole is equal to 28 .054 gram per mole.

05:54 Therefore, the number of malls of c2h4 is, number of mall is denoted by n, n, c2h4 is equal to the theoretical yield divided by molar mass of c2h4.

06:40 So the value of theoretical yield is 1131 .76 gram divided by molar mass of c2, h4 is 28 .05 gram per mole.

07:07 Is equal to gram is cancelled with gram, 40 .3 mole.

07:26 1 mole of 0 of c6h14 produces 1 mole of c2h4 therefore 40 .34 moles of c2h4 will be produced by 40 .34 malls of c2h4 will be produced by 40 .34 malls of c2h4...

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