Identify the molecularity and the rate law for each of the following elementary reactions.
(a) I2(g)→2I(g)I2(g)→2I(g)
(b) 2NO(g)+Br2(g)→2NOBr(g)2NO(g)+Br2(g)→2NOBr(g)
(c) N2O5(g)→NO2(g)+NO3(g)N2O5(g)→NO2(g)+NO3(g)
Match the items in the left column to the appropriate blanks in the sentences on the right.
Reaction (a) is , Rate =
Reaction (b) is , Rate =
reaction (c) is , rate = .Identify the molecularity and the rate law for each of the following elementary reactions. (a) I2(g)→2I(g)I2(g)→2I(g)...
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...
The rate law for the reaction 2NO2 + O3 → N2O5 + O2 is rate = k[NO2][O3]. Which one of the following mechanisms is consistent with this rate law? A) NO2 + NO2 → N2O4 (fast) N2O4 + O3 → N2O5 + O2 (slow) B) NO2 + O3 → NO5 (fast) NO5 + NO5 → N2O5 + 5/2O2 (slow) C) NO2 + O3 → NO3 + O2 (slow) NO3 + NO2 → N2O5 (fast) D) NO2 + NO2 → N2O2...
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 following mechanism for the reaction of hydrogen and iodine monochloride: Step1.H2(g)+ICl(g)?HI(g)+HCl(g)Step2.HI(g)+ICl(g)?I2(g)+HCl(g) Part A Write the equation for the overall reaction. Write the equation for the overall reaction. H2(g)+2ICl(g)?I2(g)+2HCl(g) H2(g)+ICl(g)?I2(g)+HCl(g) H2(g)+2ICl(g)?I2(g)+HCl(g) H2(g)+ICl(g)?I2(g)+2HCl(g) SubmitMy AnswersGive Up Part B Identify any reaction intermediates. Identify any reaction intermediates. HCl HI ICl H2 SubmitMy AnswersGive Up Part C What is the molecularity of the first elementary step? What is the molecularity of the first elementary step? unimolecular bimolecular termolecular SubmitMy AnswersGive Up Part...
8. Which of the following reactions cannot proceed through a single elementary step in view of the experimental rate law given? (a) NO(g) + O3(g) ⟶ NO2(g) + O2(g) rate = k[NO][O3] (b) 2HI(g) ⟶ H2(g) + I2(g) rate = k[HI]2 (c) C4H8(g) ⟶ 2C2H4(g) rate = k[C4H8] (d) 2NO(g) + H2(g) ⟶ N2(g) + H2O(g) rate = k[NO][H2] (e) 2NO(g) + Cl2(g) ⟶ 2NOCl(g) rate = k[NO]2[Cl2] The worksheet says that the answer is D, but I don’t get...
6. The rate law for the following reaction is rate=k[NO2] (F2]: 2NO2(g) + F2(g) → 2NO2F(g) The mechanism proposed for this reaction is as follows: (i) NO2(g) + F2(g) → NO2F(g) + F(g) (ii) NO2(g) + F(g) → NO2F(g) Which elementary step is the rate-determining step in this reaction? Explain your answer in 1-2 sentences.
The following reaction is first order in N2O5N2O5: N2O5(g)→NO3(g)+NO2(g)N2O5(g)→NO3(g)+NO2(g) The rate constant for the reaction at a certain temperature is 0.053/s/s. Part A Calculate the rate of the reaction when [N2O5]=[N2O5]= 5.1×10−2 MM. Express your answer using two significant figures. rate= ______ M/s Part B What would the rate of the reaction be at the same concentration as in Part A if the reaction were second order? (Assume the same numerical value for the rate constant with the appropriate units.)...
If you mix equal concentrations of reactants and products, will the reaction proceed to the right or the left? HF (aq) + NO3- (aq) - HNO3(aq) +F- (aq) Match the items in the left column to the appropriate blanks in the sentences on the right Reset Help base .and is a stronger acid than Because proton transfer occurs from the stronger the reaction proceeds to the is a stronger base than to the stronger HNO, acid left right HF NO
predict the sign of the entropy change for each of the following processes: a) I2(s)---->2I(g) cannot predict negative positive b) 2Zn(s) + O2 (g) ---> 2ZnO(S) cannot predict positive negative c) N2 (g) + O2(g) ---> 2NO(g) negative postive cannot predict
Part A Would decreasing the volume of the container for each of the following reactions cause the equilibrium to shift in the direction of the products, the reactants, or not change? Drag the appropriate items to their respective bins. Reset Help 302(g) = 203(g) 4NH3(g) +502(g) = 4NO(g) + 6H2O(g) 2NOBr() = 2NO(g) + Br2(g) Shift in the direction of the products Shift in the direction of the reactants Equilibrium does not change