First order; the rate is directly proportional to the concentration of reactant.
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.
Mainly with respect to energy.
Sodium fizzes in water because it is undergoing a chemical reaction with water to form sodium hydroxide. The result is more stable than either of the original chemicals. When sodium chloride is added to water both of these substances are stable with respect to each other and no reaction occurs that results in a new chemical product.
There are three types of phase in Bowen reaction series. 1.continuous 2.Discontiuous 3.Residual phase Discontinuous series depends upon one mineral plagioclase feldspar while exchange of sodium to calcium to sodium takes place with respect to temperature while continuous series depends upon different minerals changes with temperature.
misogynist or sexist
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.
That depends on the order of the reaction. If the reaction is zero order with respect to a reactant, then changing the concentration will have no effect on rate. If it is first order, then doubling the concentration will double the rate. If it is second order, then doubling the concentration will quadruple the rate.
Rates of reaction can be expressed depending upon their order.For example say you have a reaction between two chemicals and the initial rate for that reaction is known :-when:-The concentration of one of the reactants is doubled and the other reactants concentration remains the same and the overall rate of reaction does not change - reaction is zero orderwith respect to chemical which was doubled.The concentration of one of the reactants is doubled and other reactants concentration remains the same and the overall rate of reaction doubles - reaction is first order with respect to chemical which was doubled.The concentration of one of the reactants is doubled and other reactants concentration remains the same and the overall rate of reaction quadruples - reaction is second order with respect to chemical which was doubled.Zero Orderrate = kFirst Orderrate = k [A] (reaction is 1st order with respect to [A] and 1st order overall)Second Orderrate = k [A][B] (reaction is first order with respect to [A] and first order with respect to[B], reaction is second order overall)rate = k [A]2 (reaction is second order with respect to [A] and second order overall)Orders are simply added together in order to determine the overall order of reaction :-rate = k [A][B][C] would be third order overall and first order with respect to each of the reactantsThere are other orders of reaction, for example 2 and 3 quarter orders and third order reactions, but these are a little more complex.
You can measure it by how QUICKLY THE REACTANT IS " APPEARING OR DISAPPEARING"BY:jehad mohammad
Let assume a simple synthesis chemical reaction in solution (the solute is inert for the considered phenomenon). We can write A + B -> C and image to start with a concentration CA and CB of the components A and B and with no molecule of C. At the beginning A and B combine to form C at high speed, since no C is yet present. While the reaction goes on, C start to be present in a certain concentration CC and also the inverse reaction starts to happen, that is C decomposes in A+B. In an instant t, the rates of variation of the concentration of the three substances, that is the quantity of substance produced (or consumed if the rate is negative) in a very small time interval (let us call them RA, RB and RC) follows the so called chemical kinetics laws RA = ki CC - kd CA CB RB=RA RC=kd CA CB - ki CC where the parameters kd and ki are called direct and inverse reaction rates. Their values depends on the microscopic characteristics of the involved molecules, like collision section so on. This is a very simple situation in which the synthesis happens directly by uniting an A molecule with a B molecule. There are much more complicated reactions, where the reaction happens in a set of subsequent states and stoichiometric coefficients different from one are present. For example oxidation of carbon oxide to carbonn dioxide NO2 + CO -> NO + CO2 is a two step reaction, that happens as 1) NO2 + NO2 -> NO3 + NO 2) NO3 + CO -> NO2 + CO2 When a multiple step reaction is present, the rates can always be written, by their dependence from the concentration of the reaction elements is not linear, but depends on some power of the concentrations (that generally has no relation with the original reaction stoichiometry). Also in this case however, the coefficients of such nonlinear dependence are called reaction rates.
In general (but not always), the reaction rate will increase with increasing concentrations. If the reaction is zero order with respect to that substance, then the rate will not change.
it may be , the limiting reactant is that which is totally consumed during the reaction but its amount must be less than required amount with respect to excess reactant for example, H2SO4 + 2NaOH = Na2SO4 + 2H2O in this reaction suppose acid is 95 g and base is 85 g but acid with higher amount is the limiting reactant and base is in excess. Essentially, it's possible whenever the molecular weight of the limiting reagent is higher than the molecular weights of the other reagents.
increasing the concentration of reactants
The speed of the reaction
Since the reaction is first order with respect to H2, if the concentration of H2 were halved, the rate of the reaction would be halved. This can be seen by entering one for each value in the rate equation, then changing the value of [H2] to 1/2 while keeping the other values the same: The rate changes from 1 to 1/2.
a list of 100 words
The equation is called the rate law equation. For the reaction aA+bB =>cC+dD the rate law would be rate = k[A]^m[B]^n where k is the rate constant and m and n are the "order" with respect to each reactant. m and n must be determined experimentally and may or may not be the same as the coefficients a and b.