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.
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FREE Expert 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:
Problem Details
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.
Frequently Asked Questions
What scientific concept do you need to know in order to solve this problem?
Our tutors have indicated that to solve this problem you will need to apply the Gas Stoichiometry concept. If you need more Gas Stoichiometry practice, you can also practice Gas Stoichiometry practice problems.
What professor is this problem relevant for?
Based on our data, we think this problem is relevant for Professor Teets' class at UH.