I think the correct answer from the choices listed above is the first option. When the the pressure is increased, the equilibrium of the reaction would favor <span>formation of reactants. One indication would be the gas that is present in the product side. Increasing the pressure would allow the products to react and form the reactants. Hope this helps.</span>
According to Le Chatelier's principle, if an equilibrium reaction is subjected to a change, the reaction adjusts itself in a way to undo the change imposed.
The effect of pressure affects the equilibrium only when the reactants or products are in gaseous phase.
As none of the reactants or products is in gaseous state, there is no effect of pressure on equilibrium.
They are so small that they barely make up any of the mass of the atom, and they are so miniscule that during Rutherford 's Gold foil experiment ,they didn't even react with the alpha particles. They circle the nucleus on a ring. shown through Rutherford Atomic Model
hen the number of neutrons is known and the atomic number of an element is known, it becomes easier to determine the approximate mass number by adding the two.