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cricket20 [7]
3 years ago
8

The reaction takes place in water. What happens to the equilibrium when the pressure is increased? a)It favors formation of prod

ucts. b)It is conserved. c)It favors formation of reactants. d)It does not change
Chemistry
1 answer:
OLga [1]3 years ago
6 0

Answer:

I don't really get the options but it favoures the reactant side.

Explanation:

Increasing pressure favours the side with fewer moles of gas while decreasing pressure favours the side with the more moles of gas. E.g

If there is 0 moles of gas particles in the reactant side and 1 mole of gas particle in the product side, increasing pressure favours the reactants while decreasing pressure favours the product side.

With the explanations I have made, I hope the question is now clear to you.

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<h3>Balancing chemical equations</h3>

The equation of the reaction can be represented by the following chemical equation:

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Thus, the coefficient of ammonia will be 4, that of oxygen will be 5, that of nitrogen monoxide will be 4, and that of water will be 6.

More on balancing chemical equations can be found here: brainly.com/question/15052184

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