Methanol, CH3 OH, is made by causing carbon monoxide and...

Methanol, $CH_{3} OH,$ is made by causing carbon monoxide and hydrogen gases to react at high temperature and pressure. If $4.50 \times 10^{2} \mathrm{mL} CO$and $8.25 \times 10^{2} mL H_{2}$ are mixed, a. which reactant is present in excess? b. how much of that reactant remains after the reaction? c. what volume of $CH_{3} OH$ is produced, assuming the same pressure?

Methanol, $CH_{3} OH,$ is made by causing carbon monoxide and hydrogen gases to react at high temperature and pressure. If $4.50 \times 10^{2} \mathrm{mL} CO$and $8.25 \times 10^{2} mL H_{2}$ are mixed,

a. which reactant is present in excess?
b. how much of that reactant remains after the reaction?
c. what volume of $CH_{3} OH$ is produced, assuming the same pressure?

Key Concepts

Reaction Stoichiometry

Reaction stoichiometry involves using balanced chemical equations to determine the proportional relationships between reactants and products. In reactions involving gases, the coefficients in the balanced equation indicate the mole ratios, which, in turn, under constant temperature and pressure, correspond directly to the volume ratios of the gases involved.

Limiting Reactant

The limiting reactant is the substance that is completely consumed first in a chemical reaction, thereby preventing further reaction from occurring. Identifying the limiting reactant is essential to calculating the amount of product formed, as the quantities of reactants determine how much product can be made according to the reaction's stoichiometry.

Excess Reactant

The excess reactant is the substance that remains unconsumed after the reaction has finished. Its initial amount is more than necessary to react completely with the limiting reactant. Determining the excess reactant and the remaining amount after the reaction are important for yield calculations and optimizing reaction conditions.

Gas Laws and Volume Relationships

When dealing with gaseous reactants and products in chemical reactions under constant temperature and pressure, Avogadro's law applies. This law states that equal volumes of gases contain equal numbers of molecules, allowing the use of direct volume ratios in place of mole ratios. This simplifies the stoichiometric calculations by linking the volumes of gas directly to the coefficients in the balanced chemical equation.

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