Ethene is converted to ethane by the reaction C2 H4(g)+H2(g) Catalyst ⟶ C2 H6(g) C2 H4 flows int

Ethene is converted to ethane by the reaction C2 H4(g)+H2(g)...

Ethene is converted to ethane by the reaction $$\mathrm{C}_{2} \mathrm{H}_{4}(g)+\mathrm{H}_{2}(g)\stackrel{\text { Catalyst }}{\longrightarrow} \mathrm{C}_{2} \mathrm{H}_{6}(g)$$ $\mathrm{C}_{2} \mathrm{H}_{4}$ flows into a catalytic reactor at 25.0 $\mathrm{atm}$ and $300.^{\circ} \mathrm{C}$ with a flow rate of $1000 . \mathrm{L} / \mathrm{min}$ . Hydrogen at 25.0 $\mathrm{atm}$ and $300 .^{\circ} \mathrm{C}$ flows into the reactor at a flow rate of $1500 . \mathrm{L} / \mathrm{min}$ . If 15.0 $\mathrm{kg}$ $\mathrm{C}_{2} \mathrm{H}_{6}$ is collected per minute, what is the percent yield of the reaction?

Ethene is converted to ethane by the reaction
$$\mathrm{C}_{2} \mathrm{H}_{4}(g)+\mathrm{H}_{2}(g)\stackrel{\text { Catalyst }}{\longrightarrow} \mathrm{C}_{2} \mathrm{H}_{6}(g)$$
$\mathrm{C}_{2} \mathrm{H}_{4}$ flows into a catalytic reactor at 25.0 $\mathrm{atm}$ and $300.^{\circ} \mathrm{C}$ with a flow rate of $1000 . \mathrm{L} / \mathrm{min}$ . Hydrogen at 25.0 $\mathrm{atm}$ and $300 .^{\circ} \mathrm{C}$ flows into the reactor at a flow rate of $1500 . \mathrm{L} / \mathrm{min}$ . If 15.0 $\mathrm{kg}$ $\mathrm{C}_{2} \mathrm{H}_{6}$ is collected per minute, what is the percent yield of the reaction?

Key Concepts

Ideal Gas Law

The Ideal Gas Law (PV = nRT) is a fundamental relationship used to convert between the physical conditions (pressure, volume, and temperature) of a gas and its amount in moles. This is particularly important in reactions involving gases, as it enables accurate calculation of reactant quantities from volumetric flow rates under specified conditions.

Percent Yield

Percent yield is a measure of the efficiency of a chemical reaction, calculated by dividing the actual yield of product obtained by the theoretical yield predicted by stoichiometry, and then multiplying by 100. It helps assess how closely a reaction proceeds to the ideal case and indicates losses or side reactions occurring during the process.

Limiting Reagent

The limiting reagent is the reactant that is completely consumed first in a chemical reaction, thereby restricting the amount of product that can be formed. Identifying the limiting reagent is crucial because it determines the maximum yield possible from the reaction, regardless of the amounts of other reactants present.

Chemical Reaction Stoichiometry

Stoichiometry involves using the balanced chemical equation to relate the quantities (in moles) of reactants and products. It provides the coefficients that denote the proportion in which reactants combine and products form, allowing one to predict the theoretical yield of a reaction based on given amounts of reactants.

Transcript

00:01 For this question, we are trying to figure out the percent yield of a particular reaction that involves ethene plus hydrogen gas producing ethane.

00:17 And so we have the equation c2h4 plus h2 yields c2h6, and we know some information about our ethene and about our hydrogen gas.

00:29 We know that the temperature is 300 degrees celsius, the pressure is 25 atm for both of them.

00:37 They both have the same temperature and pressure.

00:40 And we know the rate at which they're flowing into the catalytic reactor.

00:46 So the c2h4 is flowing in at a rate of 1 ,000 liters per minute, and the hydrogen gas is flowing at a rate of 1 ,500 liters per minute.

00:55 We're also told that we get a total.

01:00 Of 15 kilograms per minute of our c2h6 of our f -a.

01:12 So we're trying to figure out what is the percent yield of this situation.

01:16 So first thing we have to do is figure out which one is the limiting factor.

01:20 And in order to do that, we need to figure out how many moles we have.

01:28 Before we can figure out our moles, we also want to make sure we change our temperature into kelvin.

01:36 So if it's 300 degrees celsius, that's going to be 300 plus 273, which gives the temperature of 573 kelvin.

01:47 And this is the same for both our c2h4 and rh2, because they're both at 300 degrees celsius.

01:58 We're already in atm, so we don't have to worry about that.

02:02 But what we're going to go ahead and do now is to figure out which one is our limiting factor.

02:09 So if we take our equation, which is pv equals n r t, and we want to solve it for moles.

02:20 So we're going to rearrange that so that moles equals pv divided by r t, then we can figure out the moles for each one of these.

02:33 So let's do c2h4 first.

02:37 So our moles of c2h4 is going to be our pressure, which is 25, times the volume, which is 1 ,000 liters per minute.

02:48 So we get 1 ,000 liters per minute for our volume.

02:53 And we're going to divide that by r, which is 0 .082606 times our temperature, which is not two as we changed it, to 573, which gives us a total mole value of 531 .7 moles of c2h4...

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