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 $1.50-$ Lreaction vessel, initially at 305 $\mathrm{K}$ , contains carbon monoxide gas at a partial pressure of 232 $\mathrm{mm} \mathrm{Hg}$ and hydrogen gas at a partial pressure of 397 $\mathrm{mm} \mathrm{g}$ . 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 $1.50-$ Lreaction vessel, initially at 305 $\mathrm{K}$ , contains carbon monoxide gas at a partial pressure of 232 $\mathrm{mm} \mathrm{Hg}$ and hydrogen gas at a partial pressure of 397 $\mathrm{mm} \mathrm{g}$ . Identify the limiting reactant and determine the theoretical yield of methanol in grams.

Key Concepts

Stoichiometry

Stoichiometry involves using the quantitative relationships between reactants and products in a balanced chemical equation. It allows one to determine how much product can form from given amounts of reactants by comparing mole ratios derived from the balanced chemical reaction.

Limiting Reactant

The limiting reactant is the substance that is completely consumed first in a chemical reaction, thus determining the maximum amount of product that can be formed. Identifying the limiting reactant is crucial because it limits the overall reaction yield, even if other reactants are in excess.

Ideal Gas Law

The ideal gas law (PV = nRT) relates the pressure, volume, temperature, and number of moles of a gas. It is used for converting the given partial pressures of gaseous reactants into moles, which is essential for applying stoichiometric calculations in gas phase reactions.

Partial Pressures in Gas Mixtures

Partial pressures refer to the pressures exerted by individual gases in a mixture. In reactions involving gases, these partial pressures can be used to calculate the amount (in moles) of each gas present by applying the ideal gas law, aiding in the determination of the limiting reactant.

Molar Mass and Theoretical Yield

Once the number of moles of the product is determined through stoichiometric calculation, the molar mass is used to convert from moles to grams, yielding the theoretical mass of product formed. Theoretical yield is the maximum amount of product predicted by the stoichiometry of the reaction, assuming complete conversion of the limiting reactant.

Transcript

00:01 Hey guys i'm here to solve question 80 so the reaction is this carbon monoxide gas plus hydrogen gas and to give metano c830h metanath so from the question we have 1 .5 the volume of the gas is 1 .5 later the temperature is 305 and the partial pressure pressure of the gas the carbon monoxide pressure pressure is 232 limiter mercury and partial pressure for hydrogen gas is 397 so i need to calculate the mold of this gas if this gas the two gas are mixed together in a container so the most the whole of each of the gas is proportional to the partial pressure of that gas.

01:31 Let me calculate the total pressure which is going to be p .t is 232 plus 397 and that gives 629mm mercury.

01:50 I can confer this to atmosphere straight away.

01:55 I like walking in an atmosphere.

01:58 Equals 760 millimeter accrued and i gave 0 .8 to 763 atmosphere.

02:14 Okay now i have my volume so i want to calculate i want to use this idea the gas of pv cost nrt so yeah and then n will be pv over rt.

02:31 Here i'm using p total so i want to calculate the mold of the gas mold of all the the both carbon dioxide and hydrogen the mold of the gas together okay it's going to be 0 .8276 atmosphere multiplied by volume is 1 .5 liter and my gas constant is 0 .082 atmosphere per kevin per mole and my temperature is 305 kelvin and with this my end will be my n is 0 .0 .049638 mole that is the mold of the two gas together so now i want to find mole of mole of each of the gas mold of carbon dioxide it would be the partial pressure of carbon dioxide which is going to be carbon dioxide is two thirty two to five by the total pressure three ninety seven tons more so this will give me the more of carbon monoxide and that is zero point 0183 more so let me calculate more of hydrogen with partial pressure of hydrogen 397 multiplied by total pressure so to be partial pressure of hydrogen is yes 399 so this is this is wrong this would be 232 divided by 629 okay that works right now.

05:20 So this one is 397 divided by 629 times 0 .049, 638...

Please give Ace some feedback