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.

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:
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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.

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