The rate of a reaction is dependent on the concentration of one or more reactants and this dependence is evident from the rate equation of that reaction. the concentration of the reactants appears in the rate equation raised to some power which are the individual orders of reaction with respect to that reactant. Overall order is the sum total of the individual orders.
For the given reaction
Rate = k [BrO3-] [Br-] [H+]2
Order with respect to BrO3- = 1 (this means rate of reaction will double if we double the concentration of BrO3-)
Order with respect to Br- = 1 (this means rate of reaction will double if we double the concentration of Br-)
Order with respect to H+= 2 (this means rate of reaction will quadruple if we double the concentration of H+)
Overall order = 1 + 1+ 2 = 4
Give the individual reaction orders for all of the following substances and the overall reaction order...
Give the individual reaction orders for all substances and the overall reaction order from the following rate law: Rate = k([O3]2 /[O2])By what factor does the rate change if each of the following changes occurs: (a) [O3] is doubled; (b)[O2] is doubled; (c) [O2]is halved?
What is the reaction order of Br- for a reaction with the following rate law? Rate = k[BrO3-][Br-][H+]2
What is the overall order of the following reaction , given the rate law ? NO(g) + O3-> No2(g)+O2(g) Rate = K (NO) (O3) 1st order 2nd order 3 order 1 1/2 order 0 order
what is the overall order of the following reaction, given the rate law? 2X + 3Y > 2Z. Rate = k[X] 1 [Y] 2
For each of the rate laws below, what is the order of the reaction with respect to the hypothetical substances X, Y, and Z? What is the overall order? (For each answer, enter an exact number as an integer or decimal.) rate = k [X]"m[2]2 Overall Overall [zi* rate = k Overall
What is the overall order of the following reaction, given the rate law? X + 2Y = 42 Rate = K[X][Y] 1st 3rd 5th 2 nd Next → F5 F6 F FBI
Use the following data to determine the individual and overall reaction orders. NO(g)+ CO2(g) rate kINO,1"[coj NO2u)+ COE) Experiment Initial Rate(M/S) Initial INO,L(M Initial ICOL (M) 0.0050 0.080 0.0050 0.10 0.40 0.10 0.10 0.10 0.20
2. (13 pts) Determine the rate constant and reaction orders for the following reaction using the data provided: 2 NO (g) + 02 (g) > 2 NO2 (g) Rate (M/s 0.028 0.057 0.114 0.227 Experiment NO 0.020 0.020 0.020 0.040 0.010 0.010 0.020 0.040 0.020 0.020 3 4 a.) For the rate law, determine all reaction orders Rate -k [NO]m[O2]' Reaction order m (CIRCLE ONE) 1½ Reaction order n (CIRCLE ONE) 1½
The reduction of bromate ions, BrO^-_3, by bromide ions in acidic solution has a rate law R = k [BrO^-_3][Br^-][H^+ ]^2. What are the orders with respect to the reactants? What is the overall order?
A)What is the overall order of reaction for a reaction that obeys the rate law rate k[A]²[B]³b) c)