Carbon monoxide gas reacts with hydrogen gas to form methanol. CO(g)+2 H2(g) ⟶CH3 OH(g) A 1.50-

Carbon monoxide gas reacts with hydrogen gas to form...

Carbon monoxide gas reacts with hydrogen gas to form methanol. $$\mathrm{CO}(g)+2 \mathrm{H}_{2}(g) \longrightarrow \mathrm{CH}_{3} \mathrm{OH}(g)$$ A $1.50-$ L reaction vessel, initially at 305 $\mathrm{K}$ , contains carbon monoxide gas at a partial pressure of 232 $\mathrm{mmH} \mathrm{g}$ and hydrogen gas at a partial pressure of 397 $\mathrm{mm} \mathrm{H} \mathrm{g} .$ Identify the limiting reactant and determine the theoretical yield of methanol in grams.

Carbon monoxide gas reacts with hydrogen gas to form methanol.
$$\mathrm{CO}(g)+2 \mathrm{H}_{2}(g) \longrightarrow \mathrm{CH}_{3} \mathrm{OH}(g)$$
A $1.50-$ L reaction vessel, initially at 305 $\mathrm{K}$ , contains carbon monoxide gas at a partial pressure of 232 $\mathrm{mmH} \mathrm{g}$ and hydrogen gas at a partial pressure of 397 $\mathrm{mm} \mathrm{H} \mathrm{g} .$ Identify the limiting reactant and determine the theoretical yield of methanol in grams.

Key Concepts

Theoretical Yield

The theoretical yield is the maximum amount of product that could be formed from a given quantity of reactants, based on the reaction's stoichiometry and assuming complete conversion of the limiting reactant. It serves as a benchmark for comparing actual product yields in a chemical reaction.

Ideal Gas Law

The ideal gas law, represented by the equation PV = nRT, relates pressure, volume, temperature, and the number of moles of a gas. This relationship is crucial for converting between pressure measurements and the moles of gas involved in a reaction, especially under specified temperature and volume conditions.

Partial Pressure

Partial pressure is the pressure exerted by an individual gas in a mixture of gases. It is used in conjunction with the ideal gas law to calculate the number of moles of that specific gas, which is necessary for accurate stoichiometric analysis in reactions involving gases.

Limiting Reactant

The limiting reactant is the substance in a chemical reaction that is entirely consumed first, thereby determining the maximum amount of product that can be formed. Identifying the limiting reactant is essential in stoichiometric calculations to ensure that predictions of product formation are accurate.

Reaction Stoichiometry

Reaction stoichiometry involves using the balanced chemical equation to understand the quantitative relationships between reactants and products. It allows one to determine how much product can be produced from given amounts of reactants and is fundamental in calculating theoretical yields.

Transcript

00:01 All right, so in this question, i've got the reaction of carbon monoxide and hydrogen gas to form methanol.

00:08 And what we're asked to do is determine what the limiting reactant is and also what the theoretical yield is.

00:14 All right, so first thing we're going to do is convert everything in the balls.

00:17 We want to find the number of moles both of carbon monoxide and of hydrogen gas, determine which one is the limiting reagent.

00:23 So how we're going to do that is just using the ideal gas law.

00:26 We can say that n is equal to pv over r t.

00:30 So we can say that n for carbon monoxide is equal to the partial pressure, which it tells us, sorry about that, it's equal to the partial pressure, which it tells us is 232 millimeters of mercury, times the volume, which it tells us we're in a 1 .50 liter container over r, which in this case is going to be 62 .36.

01:00 The unit's going to be millimeters mercury times liters over mole kelvin.

01:06 And then it tells us the temperature, which is 305 kelvin.

01:13 So with all the information, we can calculate that the moles of carbon monoxide are 0 .0183.

01:21 All right.

01:21 So similarly, we can calculate the n for the hydrogen and gas.

01:26 And it's going to be almost identical.

01:28 The only difference is going to be one of these numbers.

01:30 It's going to be the 397 millimeters of mercury is the only difference between these.

01:36 All right, so everything else, i can just add kind of copy -pasted from the other side.

01:57 And then doing this calculation, it's going to give us a value of 0 .0313.

02:08 Okay, so now what we can do is we convert both of those numbers to moles of our methanol product...

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