🤓 Based on our data, we think this question is relevant for Professor Teets' class at UH.

Solution: Carbon monoxide gas reacts with hydrogen gas to form methanol via the following reaction:CO(g) + 2 H2(g) → CH3OH(g)A 1.55 L reaction vessel, initially at 305 K, contains carbon monoxide gas at a partial pressure of 232 mmHg and hydrogen gas at a partial pressure of 376 mmHg .Identify the limiting reactant and determine the theoretical yield of methanol in grams.

Problem

Carbon monoxide gas reacts with hydrogen gas to form methanol via the following reaction:

CO(g) + 2 H₂(g) → CH₃OH(g)

A 1.55 L reaction vessel, initially at 305 K, contains carbon monoxide gas at a partial pressure of 232 mmHg and hydrogen gas at a partial pressure of 376 mmHg .

Identify the limiting reactant and determine the theoretical yield of methanol in grams.

Solution

• Calculate for the moles of each reactant gas and use stoichiometry to determine the moles and eventually mass of CH₃OH
• Moles of reactant will be calculated using the conditions via the ideal gas equation
• Ideal gas equation will appear as:

• Calculating the moles of reactant gases:

View Complete Written Solution