Chlorine gas reacts with fluorine gas to form chlorine...

Chlorine gas reacts with fluorine gas to form chlorine trifluoride. $$\mathrm{Cl}_{2}(g)+3 \mathrm{F}_{2}(g) \longrightarrow 2 \mathrm{ClF}_{3}(g)$$ A 2.00 -L reaction vessel, initially at 298 $\mathrm{K}$ , contains chlorine gas at a partial pressure of 337 $\mathrm{mm} \mathrm{Hg}$ and fluorine gas at a partial pressure of 729 $\mathrm{mm} \mathrm{Hg}$ . Identify the limiting reactant and determine the theoretical yield of $\mathrm{ClF}_{3}$ in grams.

Chlorine gas reacts with fluorine gas to form chlorine trifluoride.
$$\mathrm{Cl}_{2}(g)+3 \mathrm{F}_{2}(g) \longrightarrow 2 \mathrm{ClF}_{3}(g)$$
A 2.00 -L reaction vessel, initially at 298 $\mathrm{K}$ , contains chlorine gas at a
partial pressure of 337 $\mathrm{mm} \mathrm{Hg}$ and fluorine gas at a partial pressure of
729 $\mathrm{mm} \mathrm{Hg}$ . Identify the limiting reactant and determine the theoretical
yield of $\mathrm{ClF}_{3}$ in grams.

Key Concepts

Ideal Gas Law and Partial Pressures

The Ideal Gas Law relates pressure, volume, temperature, and the number of moles in a gas. When dealing with gaseous reactants, partial pressures can be used to determine the number of moles present by applying the Ideal Gas Law, which is essential for translating pressure data into usable quantities for stoichiometric calculations.

Stoichiometry

Stoichiometry deals with the quantitative relationships between reactants and products in a chemical reaction. It involves using the coefficients from a balanced chemical equation to compute how much of each substance is involved and to predict the amounts of products formed from given reactants.

Theoretical Yield

The theoretical yield is the maximum amount of product that can be generated in a chemical reaction based on the complete consumption of the limiting reactant. It is calculated using stoichiometry and represents an ideal scenario where the reaction goes to completion with no losses.

Limiting Reactant

The limiting reactant is the substance in a chemical reaction that is completely consumed first, thus limiting the amount of product that can be formed. Its determination involves comparing the mole ratios of the reactants as dictated by the balanced chemical equation, ensuring that the reactant available in the smallest quantity (relative to its required stoichiometric coefficient) determines the reaction's extent.

Transcript

0:00 All right.

00:01 So in this question, we have a reaction of chlorine and fluorine gas to form chlorine trifluoride.

00:10 And we're asked to determine what is the limiting reactant and also what's the theoretical yield.

00:15 So starting, first thing to do is figure out the number of moles that we have of both these things.

00:22 Using the ideal gas law, we can just say that n is equal to pv over rt.

00:30 So from there we calculate n, let's say, of cl2, which is going to be equal first to the pressure, which it tells us the problem is 337 millimeters mercury, and the volume which tells us a 2 .0 liter vessel.

00:47 Over r, 62 .36 is going to be the value we use, since it's just in millimeters of mercury.

00:54 Units are going to be millimeters of mercury times liters over mole times kelvin.

01:03 And lastly, a temperature of 298 kelvin.

01:08 All right, so all of our units check out, and we should get moles from this.

01:11 If we do that, we're going to have 0 .0362 moles.

01:17 We can do the exact same thing for fluorine, right? we can say moles of f2.

01:21 And this time i'm going to leave off the units just for sake of time, since we already made sure all the units check out.

01:27 So we're going to have 729 for the pressure, 2 again for the volume, 62.

01:36 0 .36 again for r and 298 again for temperature, giving us 0 .05 to 3 moles...

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