Part A
What is the overall reaction?
Part B
Which species is a reaction intermediate?
Part C
What is the rate law for step 1 of this reaction?
Part D
What is the rate law for step 2 of this reaction
2X→Y+Z2X→Y+Z Y+2L→M+ZY+2L→M+Z Part A What is the overall reaction? Part B Which species is a reaction...
To understand how elementary steps make up a mechanism and how the rate law for an elementary step can be determined. Very often, a reaction does not tell us the whole story. For instance, the reaction NO2(g)+CO(g)→NO(g)+CO2(g)NO2(g)+CO(g)→NO(g)+CO2(g) does not involve a collision between an NO2NO2 molecule and a COCO molecule. Based on experimental data at moderate temperatures, this reaction is thought to occur in the following two steps: NO2(g)+NO2(g)→NO3(g)+NO(g)NO2(g)+NO2(g)→NO3(g)+NO(g) NO3(g)+CO(g)→CO2(g)+NO2(g)NO3(g)+CO(g)→CO2(g)+NO2(g) Each individual step is called an elementary step. Together, these...
what is the overall order of the following reaction, given the rate law? 2X + 3Y > 2Z. Rate = k[X] 1 [Y] 2
For the overall reaction below, which of the following is the correctly written rate law? Overall reaction: O3(g)+2NO2(g)→N2O5(g)+O2(g) Step 1: O3(g)+NO2(g)→NO3(g)+O2(g) slow Step 2: NO3(g)+NO2(g)→N2O5(g) fast View Available Hint(s) For the overall reaction below, which of the following is the correctly written rate law? Overall reaction: Step 1: slow Step 2: fast A.] Rate=k[O3][NO2]2 B.] Rate=k[O3][NO2] C.] Rate=k[NO3][NO2] D.] Rate=k[O3][NO2]2[N2O5][O2]
Consider the hypothetical reaction: 2 X + Y → Z and its general rate law Rate = k[X]m[Y]n The following data was obtained when the reaction studied at –10°C: [X], M [Y], M Rate, M/min 0.10 0.10 0.18 0.10 0.20 0.36 0.20 0.20 1.45 (a) What is the order of reaction with respect to X? (2 points) (b) What is the order of reaction with respect to Y? (2 points) (c) What is the overall order of reaction?...
For a hypothetical chemical reaction that has the stoichiometry 2X + Y -----Z the following initial data were obtained X (Mol/L Y(Mol/L) rate of formation of Z (Mol/L s .4 .2 1.4 x 10^-3 .4 .4 2.8 x 10^-3 .2 .1 7.0 x 10^-4 .6 .6 4.2 x 10^-3 Give rate Law for this reaction Callculate rate constant and specify units How long must reaction proceed to produce concentration of Z =to .2 molar if initial concentrations of x=.8M and...
Consider the reaction X Y +Z Which of the following is a possible rate law? a) Rate = k[X] b) Rate = K[Y] c) Rate = k[Y][Z] Rate = k[X][Y] Rate = k[Z] e) Rate 3. What are the units for the rate constant for an overall third order reaction? a) L/mol:s b) LP/mol.s mol/L'S e) L2 For which order reaction is the half-life of the reaction inversely proportional to k, the rate constant? a) zero order b) first order...
Consider the overall reaction and proposed mechanism. What step is rate determining (slow) if the rate law of overall reaction is Rate = k[A][BC] step 1: A + BC --> AB + C step 2: AB + D --> AD + B step 3: B + C --> BC overall reaction: A + D --> AD
A mechanism for the gas phase reaction of fluorine with chlorine dioxide that is consistent with the observed rate law is: step slow: F2+CIO, FCIO, + F step 2 fast: F+CIO, FCIO, (1) What is the equation for the overall reaction? Use the smallest integer coefficients possible. If a box is not needed, leave it blank. (2) Which species acts as a catalyst? Enter formula. If none, leave box blank (3) Which species acts as a reaction intermediate? Enter formula....
Consider the elementary reaction equations shown. A(g) + B(g) --> C(g) + D(g) 2X(g) --> Y(g) + Z(g) Write the rate law for reaction A. Write the rate law for reaction B.
A chemist determined that a reaction was composed of the following steps: Step Reaction Rate i) 3B + 2 A = D + 2E 65.3 M-3min-1 ii) 2E + 3 F = 2 A + 2 C 248 M-4min-1 (a) Write the equation that describes the net reaction: (b) Write the rate law of the reaction that the chemist will most likely observe for this reaction. (c) Which of the following species (A, B, C, D, E, F) is the catalyst? (d) Which of the following species (A,...