Methanol, CH3 OH, is made by using a catalyst to react...

Methanol, $\mathrm{CH}_{3} \mathrm{OH},$ is made by using a catalyst to react carbon monoxide with hydrogen at high temperature and pressure. Assuming that 450.0 $\mathrm{mL}$ of $\mathrm{CO}$ and 825 $\mathrm{mL}$ of $\mathrm{H}_{2}$ are allowed to react, answer the following questions. (Hint: First write the balanced chemical equation for this reaction.) a. Which reactant is in excess? b. How much of that reactant remains when the reaction is complete? c. What volume of $\mathrm{CH}_{3} \mathrm{OH}(g)$ is produced?

Methanol, $\mathrm{CH}_{3} \mathrm{OH},$ is made by using a
catalyst to react carbon monoxide with
hydrogen at high temperature and pressure.
Assuming that 450.0 $\mathrm{mL}$ of $\mathrm{CO}$ and 825 $\mathrm{mL}$
of $\mathrm{H}_{2}$ are allowed to react, answer the
following questions. (Hint: First write the balanced chemical equation for this reaction.)
a. Which reactant is in excess?
b. How much of that reactant remains
when the reaction is complete?
c. What volume of $\mathrm{CH}_{3} \mathrm{OH}(g)$ is produced?

Key Concepts

Stoichiometry

Stoichiometry involves using the balanced chemical equation to calculate the relationships between the reactants and products. It allows for the determination of how much product will form from given amounts of reactants, as well as identifying which reactant will be consumed first.

Gas Volume Relationships

Under constant temperature and pressure, gases obey Avogadro's law, which states that equal volumes of gases contain equal numbers of moles. This principle allows the direct use of volume ratios, as obtained from measurements, in stoichiometric calculations for gas-phase reactions.

Excess Reagent

The excess reagent is the reactant that remains after the reaction is complete, having been supplied in greater amount than necessary according to the stoichiometric ratios. The quantity remaining can be calculated by comparing its initial amount with the amount used up reacting with the limiting reagent.

Balanced Chemical Equation

A balanced chemical equation represents the reaction in which the numbers of atoms for each element are equal on both sides. It provides the stoichiometric coefficients necessary to relate the amounts of each reactant and product, laying the groundwork for all subsequent quantitative calculations in the reaction.

Limiting Reagent

The limiting reagent is the reactant that is completely consumed first during the reaction, thereby determining the maximum amount of product that can be formed. Its identification is essential to stoichiometric calculations as it limits the extent of the reaction.

Transcript

0:00 Hello.

00:01 Today we'll be talking about chapter 12, question 63, which asks us to consider the process here used for industrially making methanol from carbon monoxide and hydrogen gas using a catalyst, which have abbreviated cat.

00:19 And so we're told that given a situation using this catalyst, we have 450 milliliters of carbon monoxide of carbon monoxide of carbon monoxide gas.

00:33 And additionally, we have 825 milliliters of hydrogen gas.

00:43 And so we're asked a couple of things, and we're asked first to determine the limiting reagent, which reagent is in excess.

00:52 And so we know from the law of volumes of gases that gases at the same temperature and pressure will basically be the same numbers of moles depending on their volumes.

01:05 So 450 mils of co is the same number of moles as 450 mils of h2, it's 450 mils of argon, etc, assuming that all of these gases are in the same pressure, or the same pressure and temperature.

01:22 And so from our balanced equation, we know that every mole of co needs two moles of hydrogen gas to produce methanol.

01:32 And so given this, we can say that the amount of needed hydrogen, so needed h2, is equal to two times the volume of the carbon monoxide that we have, which means we need 900 mils of hydrogen to react with all of the co.

01:54 If we look at it from the point of view of the hydrogen, needed co is equal to one -half the volume of the volume of.

02:05 Hydrogen, which in this case is equal to 40012 .5 milliliters of co.

02:18 And so we don't have 900 mils of hydrogen.

02:22 Thus, we can't react with all of the co...

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