Concentration of products would increase in order to attain equilibrium in the system again.
For example:
H2CO3 --> H+ + HCO3-
K= ([H+][žHCO3-])/([H2CO3])
K is constant for this process, so if you increase the concentration of reactants (H2CO3), in order for K to stay the same, concentration of products (H+, HCO3-) would also have to increase.
It's part of Le Chatelier's principle: "If a chemical system at equilibrium experiences a change in concentration, temperature, volume, or partial pressure, then the equilibrium shifts to counteract the imposed change and a new equilibrium is established."
So, in your case, adding more reactant would cause equilibrium to shift to the right (toward products), and therefore, their concentration would increase so that new equilibrium could be established.
The reaction would shift to balance the change
The concentration of products would increase. apex
Concentration of products would increase in order to attain equilibrium in the system again.
For example:
H2CO3 --> H+ + HCO3-
K= ([H+][žHCO3-])/([H2CO3])
K is constant for this process, so if you increase the concentration of reactants (H2CO3), in order for K to stay the same, concentration of products (H+, HCO3-) would also have to increase.
It's part of Le Chatelier's principle: "If a chemical system at equilibrium experiences a change in concentration, temperature, volume, or partial pressure, then the equilibrium shifts to counteract the imposed change and a new equilibrium is established."
So, in your case, adding more reactant would cause equilibrium to shift to the right (toward products), and therefore, their concentration would increase so that new equilibrium could be established.
The concentration of REACTANTS would increase. APEX
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The concentration of products would increase APEX
The concentration of products would increase.
The concentration of reactants would increase.
The concentrations of reactants and products are modified.
more reactants will form
If the added substance is a reactant, the equilibrium shifts toward products. If it is a product, it moves towards reactants.
In a reversible reaction, the reactants and products become to a dynamic equilibrium after some time. after gaining this equilibrium, when more reactants are added the equilibrium breaks. So according to the Le Chetelier principle, the reaction will proceed until the equilibrium is gained.
More No will be produced
The concentrations of reactants and products are modified.
The concentration of products would increase. apex
more reactants will form
If the added substance is a reactant, the equilibrium shifts toward products. If it is a product, it moves towards reactants.
If the added substance is a reactant, the equilibrium shifts toward products. If it is a product, it moves towards reactants.
To the right because it would move the opposite way of the reactants.
the equilibrium will be shifted backward so that the dissociation of NaHSO4 will decrease (less H+)
more reactants will form
In a reversible reaction, the reactants and products become to a dynamic equilibrium after some time. after gaining this equilibrium, when more reactants are added the equilibrium breaks. So according to the Le Chetelier principle, the reaction will proceed until the equilibrium is gained.
Le Chetalier's principle predicts a system at equilibrium will change to adapt. If more products are added, the system will react to tend to negate that change, so more reactants would form.
More Reactants will form!!
Adding NO to the system at equilibrium would increase the concentration of the NO product. According to Le Chatelier's principle, the system will counteract this change by producing more of the reactants, N2 and O2.