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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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For this we can use the combined gas law:

\frac{P_{1}V_{1} }{T_{1}} = \frac{P_{2}V_{2} }{T_{2}}

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\frac{P_{1} }{T_{1}} = \frac{P_{2} }{T_{2}}

P₁ = 2 atm

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Plug these values in:

\frac{2atm}{27C} = \frac{2.2atm}{T_{2}}

Solve for T₂.

2atm = \frac{2.2atm}{T_{2}}*27C

2atm * T_{2}={2.2atm}*27C

T_{2}={2.2atm}\div2atm*27C

T_{2}=1.1*27C

T_{2}=29.7C

Convert this to kelvin and get 302.85 K, which is closest to B. 330 K.

Hope this helps!

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