In the reaction N2(g) + O(g)
↔ 2NO(g) produced i an increase in the total pressure will?
cause less nitrogen to be produced in the equilibrium mixture
cause less nitric oxide to be produced in the equilibrium mixture
cause more nitric oxide to be produced in the equilibrium mixture
cause more oxygen to be produced in the equilibrium mixture
have no effect
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Discussions (14)
Under the topic chemical equilibrium, we study that pressure will have effect on equilibrium position if all reactants and products are gaseous and if the sum total of moles of gaseous reactants and moles of gaseous products differ.
Note: pressure is inversely proportional to volume.
To determine volume, the number of moles is used.
Hence, If the reactants have a lesser number of moles than the number of moles of products and pressure is applied, the pressure applied favors the reactant side. In other words, the equilibrium position would shift to the left.
The same principle applies vice versa.
the answer is E no effect on the product since the mole are 2 and 2 so they are no effect of change on the product.
Increase in pressure should favour the side with lesser amount of moles. Therefore the correct answer is C
The equation is not balanced, its 02 not just 0, that is where confusion is comming from
myschool please amend your answer the answer should be B, because the reactants and product are all gases, and an increase in pressure should favour the one with lesser amount of moles.
