Yield and atom economy of chemical reactions (chemistry only)

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Question 12
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This question is about reversible reactions and chemical equilibrium.

Methanol (CH3OH\text{CH}_3\text{OH}CH3​OH) is an important liquid fuel and chemical feedstock. It can be produced industrially by the catalytic hydrogenation of carbon dioxide (CO2\text{CO}_2CO2​).

The equation for the reaction is:

CO2(g)+3H2(g)⇌CH3OH(g)+H2O(g)\text{CO}_2(\text{g}) + 3\text{H}_2(\text{g}) \rightleftharpoons \text{CH}_3\text{OH}(\text{g}) + \text{H}_2\text{O}(\text{g})CO2​(g)+3H2​(g)⇌CH3​OH(g)+H2​O(g)

a.

Calculate the atom economy for the formation of methanol (CH3OH\text{CH}_3\text{OH}CH3​OH) in this reaction.

Relative atomic masses (ArA_{\text{r}}Ar​): H=1\text{H} = 1H=1, C=12\text{C} = 12C=12, O=16\text{O} = 16O=16

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b.

Explain the effect of increasing the pressure on the equilibrium yield of methanol. Give your answer in terms of equilibrium.

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Yield and atom economy of chemical reactions (chemistry only) Questions

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  2. /Chemistry
  3. /Yield and atom economy of chemical reactions (chemistry only)