It is the ratio of the concentrations of products to the concentrations of reactants.
It depends on the stoichiometry of the balanced reaction. For instance, if you have a reaction that is
A ---> B
then the rate of disappearance of A is exactly equal to the rate of appearance of B.
However, if the balanced reaction was
2A ---> B
then the rate of disappearance of A would be exactly double the rate of appearance of B, because 2 A's have to be consumed to make 1 B.
Said in general terms, for a reaction:
aA + bB ---> cC + dD
rate = 1/a * -d[A]/dt = 1/b * -d[B]/dt = 1/c * d[C]/dt = 1/d * d[D]/dt
where lower-case letters are the coefficients of the balanced reactions, upper-case letters are the species involved in the reaction, and square brackets means the concentration of whichever chemical is inside.
...don't quote me but i would assume they would be "the same".
Added:Yes, this is a very fine definition of what an equilibriumactually is: dynamic, going both sides (forward and backward), at the same time, at the same rate.The effect is that all concentrations (Products and Reactants) are constant, remain the same.
when concentration is increased to reactants - the forward reaction increases and backward reaction decreases.
when concentration of product is increased - forward reaction decrease and backward reaction increases
At equilibrium, the rate of production of the reactants compared with the rate of production of the products is the same.
At equilibrium the concentration of products and reactants is constant.
the same
Perhaps you are referring to a first order reaction.
This substance is called "reactant" or "initial product".
It should represent a true chemical change. It should be balance it should be molecular all the reactant and product must be written in term of there respective chemical formula.
Kp = (P-product)(P-product) --------------------------- (P-reactant)(P-reactant) its always products over reactants, you can always re-arrange the formula to find the pressure of one of the products or reactants.
The initial rate refers to the rate at which a chemical reaction occurs at the beginning, when the reactants are first mixed together. It is determined by measuring the change in concentration of a reactant or product over a short period of time immediately after the reaction has started.
molecular concentration
This is the law of mass conservation.
Fire is Combustion, in which your reactant is reacted with oxygen and heat to form carbon dioxide and water, so you turn your reactant into a product this is a chemical change.
Perhaps you are referring to a first order reaction.
This substance is called "reactant" or "initial product".
it depends if it is on the reactant side or product side. BUTTT in this case, I am assuming HCL is a solid.which whether or not it is on the reactant or product side, there would be NO CHANGE.
When reactants are converted into products some amount of reactant actually do not get converted into product. This is the case in any process. Total conversion of reactant species into product species is never possible.
Le Chetalier's Principle states "If to a system in equilibrium, a change is applied, the system will react to tend to negate that change" - or the substance of that statement. So if you add product, the system will tend to go to the reverse reaction and produce more reactant. Vice Versa. If more reactant is added, the system reacts to make more product to restore equilibrium.
These are: reaction, chemical formula, reactant, product, chemical equation.
The effect of concentration of reactants on rate of reaction depends on the ORDER of the reaction. For many reactions, as the concentration of reactants increases, the rate of reaction increases. There are exceptions however, for example a zero order reaction where the rate of reaction does not change with a change in the concentration of a reactant.
concentration
It doesn't - the reaction rate will not change regardless of how much of that reactant is added. That's the definition of zero-order.