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If a reaction of 5.0 g of hydrogen with 5.0 g of carbon monoxide produced 4.5 g of methanol, what was the percent yield?

If a reaction of 5.0 g of hydrogen with 5.0 g of carbon monoxide produced 4.5 g of methanol, what was the percent yield?

Asked by: Guest | Views: 35
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Guest [Entry]

"Answer:

The percent yield is 78.75%.

Explanation:

The balanced chemical reaction for this problem is

H₂ + CO → CH₃OH

2H₂ + CO → CH₃OH

Using the given data in the problem, we solve for the limiting reactant.

Solving the limiting reactant:

5.0 g H₂ = 2.5 mol H₂
5.0 g CO = 0.17857 mol CO

Looking in the balanced equation, we can see that the theoretical moles of H₂ is 2 moles while the theoretical moles of CO is 1 mole.

Comparing the computed moles of H₂ and CO from the experimental amount to the moles in the balanced equation, the excess reactant is H₂ (because 2.5 is greater than 2) and limiting reactant is CO (because 0.17857 is lesser that 1)

Solving for the theoretical mass of H₂ and CO:

(2.5 mol H₂) = 40 grams methanol
(0.17857 mol CO) = 5.71424 grams methanol

Solving percent yield:

% yield =
% yield =
% yield = 78.75%

Learn more about percent yield here:

brainly.ph/question/2620069

Know more about chemical equation here: brainly.ph/question/2133024

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