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A 4.72-g sample of methanol (CH3OH) was placed in an otherwise empty 1.00-L flask and
Chapter 13, Problem 13.127(choose chapter or problem)
A \(4.72-g\) sample of methanol (\(CH_{3}OH\)) was placed in an otherwise empty \(1.00-L\) flask and heated to \(250.^{\circ}\)C to vaporize the methanol. Over time the methanol vapor decomposed by the following reaction:
\(\mathrm{CH}_{3} \mathrm{OH}(\mathrm{g}) \rightleftharpoons \mathrm{CO}(\mathrm{g})+2 \mathrm{H}_{2}(\mathrm{~g})\)
After the system has reached equilibrium, a tiny hole is drilled in the side of the flask allowing gaseous compounds to effuse out of the flask. Measurements of the effusing gas show that it contains \(33.0\) times as much \(H_{2}(g)\) as \(CH_{3}OH(g)\). Calculate \(K\) for this reaction at \(250.^{\circ}\)C.
Questions & Answers
QUESTION:
A \(4.72-g\) sample of methanol (\(CH_{3}OH\)) was placed in an otherwise empty \(1.00-L\) flask and heated to \(250.^{\circ}\)C to vaporize the methanol. Over time the methanol vapor decomposed by the following reaction:
\(\mathrm{CH}_{3} \mathrm{OH}(\mathrm{g}) \rightleftharpoons \mathrm{CO}(\mathrm{g})+2 \mathrm{H}_{2}(\mathrm{~g})\)
After the system has reached equilibrium, a tiny hole is drilled in the side of the flask allowing gaseous compounds to effuse out of the flask. Measurements of the effusing gas show that it contains \(33.0\) times as much \(H_{2}(g)\) as \(CH_{3}OH(g)\). Calculate \(K\) for this reaction at \(250.^{\circ}\)C.
ANSWER:Step 1 of 5
The balanced equation for the decomposition of methanol is:
\(\mathrm{CH}_{3} \mathrm{OH}(\mathrm{g}) \rightarrow \mathrm{CO}(\mathrm{g})+2 \mathrm{H}_{2}(\mathrm{~g})\)
Let's first calculate the number of moles of \(\mathrm{CH}_{3} \mathrm{OH}\) that were vaporized. \(\mathrm{CH}_{3} \mathrm{OH}\)’s molar mass is 32.04 g/mol.