Consider the chemical equation in equilibrium.

Chemistry

2 answers:

RSB [31]3 years ago

8 0

Answer:

The correct answer is :'The equilibrium will shift to the right to favor the forward reaction'.

Explanation:

$CH_4(g) + H_2O(g) \rightleftharpoons CO(g) + 3H2(g)$

According to Le-Chatlier's principle,When the pressure is increased the equilibrium shifts in the direction where number of moles of gas molecules are greater .

The equilibrium will shift towards the product side because there are more number of moles of gas re greater on product side. So, the equilibrium will shift in the right direction favoring the forward reaction.

Andrew [12]3 years ago

5 0

When pressure in a chemical reaction increases, the equilibrium will shift towards the side of the reaction with fewer moles of gas. When there is a decrease in pressure, the equilibrium will shift towards the side of the reaction with more moles of gas.Therefore; in this case; increased the Equilibrium will shift to the left and favor the reverse reaction. This is because the side of products has more moles compared to the side of reactants, thus increased in pressure will aid conversion of products to reactants.

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8.7 Two products are formed in the following reaction in a 50:50 mixture. Would the resulting solution be optically active

k0ka [10]

Answer:

Yes. The solution would be optically active.

Explanation:

Diastereomer are defined as the image that is non mirror and non -identical. It is made up of two stereoisomers. They are formed when the two stereoisomers or more than two stereoisomers of the compound have the same configuration at the equivalent stereocenters.

In the given context, as the product given is a diastereomeric mixture, the product would have an optical activity in total.

So the answer is Yes.