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timurjin [86]
3 years ago
5

The reaction to prepare methanol from carbon monoxide and hydrogen ‍ is exothermic. If you wanted to use this reaction to produc

e methanol commercially, would high or low temperatures favor a maximum yield? Explain.
Chemistry
1 answer:
Alex_Xolod [135]3 years ago
8 0

Answer:

The reaction in low temperature will favor maximum yield.

Explanation:

Methanol is mainly produced by hydrogenation of carbon monoxide.It is the simplest alcohol which contain methyl group that is linked with hydroxyl group.Methanol is volatile,colorless,flammable liquid.

Ethanol is less toxic than methanol.Methanol is the precursor of acetic acid,methyl tertiary butyl ether.

During formation of commercial methanol,carbon dioxide and water acts as poisons to alkali metal methoxide catalyst in low temperature in methanol synthesis reaction.

More over,high temperature evaporates methanol.

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Your question is incomplete. However, I found a similar problem fromanother website as shown in the attached picture.

To solve this problem, you must know that at STP, the volume for any gas is 22.4 L/mol. So,

Moles O₂: 156.8 mL * 1 L/1000 mL* 1 mol/22.4 L = 0.007 moles
Mass calcium: 0.007 mol O₂ * 2 mol Ca/1 mol O₂ * 40 g/mol Ca =<em> 0.56 g Ca</em>

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Answer:

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