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.

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 parti

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:

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