Unless the reaction is not using up all of the reactants, adding more of just one cannot increase the amount of the products.
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 molecules will rearrange, giving off or absorbing energy. The atoms will be by and large unaffected (they might gain or loose an electron or two)
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.
Factors which can increase the rate of a chemical reaction:- temperature- pressure- concentration of reactants- stirring- if solids are involved the dimension of particles is important- the type of reaction- the order of reaction- presence of catalysts- influence of external factorsetc.
endothermic and exothermic reactions
in order for reactants to be changed into products, there needs to be a chemical change.
The total numbers of atoms of reactants do not change in products.
The concentrations of reactants and products are modified.
In a chemical reaction that proceeds to completion, there will be reactants and products at any time during the reaction. Reactants are the substances that react to produce products. This occurs through collisions that happen on the microscopic level. Two reactant particles cannot react unless they collide with the correct orientation and sufficient energy to form an activated complex, which is the intermediate molecule between reactants and products.
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 mass of reactants must be equal to the mass of products.
what will happen to the rate if you decrease the enzyme concentration
it will increase.
Glucose and oxygen become carbon dioxide and water. The products have a lower energy content than the reactants.
The concentration of products would increase. apex
Increasing the concentration of reactants will shift the equilibrium towards the products. The equilibrium will always shift to reduce the change you caused. If you add more products, it shifts toward reactants. This is known as the Le Chatelier Principle.See the Web Links to the left of this answer for more about this.
Increase