Yield and atom economy of chemical reactions (chemistry only)

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Question 18
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This question is about reversible reactions and chemical equilibrium.

Acetylene (C2H2\text{C}_2\text{H}_2C2​H2​) is an important industrial chemical used in welding. It can be produced by the thermal cracking of methane (CH4\text{CH}_4CH4​).

The equation for the reaction is:

2CH4(g)⇌C2H2(g)+3H2(g)2\text{CH}_4(\text{g}) \rightleftharpoons \text{C}_2\text{H}_2(\text{g}) + 3\text{H}_2(\text{g})2CH4​(g)⇌C2​H2​(g)+3H2​(g)

a.

Calculate the atom economy for the formation of acetylene (C2H2\text{C}_2\text{H}_2C2​H2​) in this reaction.

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

[3]
b.

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

[3]

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

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