(a)
Interpretation:
The rate law has to be written for the given elementary reaction.
Concept Introduction:
For elementary reactions, rate law can be written using stoichiometry. The order of unimolecular reaction is one and bimolecular reaction is two. In a bimolecular reaction if the reactants are different then order with respect to each reactant will be one in order to make the overall order two.
(b)
Interpretation:
The rate law has to be written for the given elementary reaction.
Concept Introduction:
Refer to part (a).
(c)
Interpretation:
The rate law has to be written for the given elementary reaction.
Concept Introduction:
Refer to part (a).
(d)
Interpretation:
The rate law has to be written for the given elementary reaction.
Concept Introduction:
Refer to part (a).
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Chapter 11 Solutions
OWLV2 FOR MOORE/STANITSKI'S CHEMISTRY:
- Distinguish between the differential rate law and the integrated rate law. Which of these is often called just the rate law? What is k in a rate law, and what are orders in a rate law? Explain.arrow_forwardThe Raschig reaction produces the industrially important reducing agent hydrazine, N2H4, from ammonia, NH3, and hypochlorite ion, OCl−, in basic aqueous solution. A proposed mechanism is Step 1: Step 2: Step 3: What is the overall stoichiometric equation? Which step is rate-limiting? What reaction intermediates are involved? What rate law is predicted by this mechanism?arrow_forward. find the rate law predicted for a particular reaction mechanism.arrow_forward
- The isomerization of cyclopropane, C3H6, to propylene, CH2=CHCH3, is first order in cyclopropane and first order overall. At 1000oC, the rate constant is 9.2/s. (a) What is the half-life of cyclopropane at 1000oC? (b) How long would it take for the concentration of cyclopropane to decrease to 50% of its initial value? (c) To 25% of its initial value?arrow_forwardIn a study of nitrosyl halides, a chemist proposes the fol-lowing mechanism for the synthesis of nitrosyl bromide:(1)NO(g)+Br₂(g)→NOBr₂(g)[fast] (2)NOBr₂(g)+NO(g)→ 2NOBr(g)[slow].If the rate law is rate k[NO]²[Br₂], is the proposed mechanismvalid? If so, show that it satisfies the three criteria for validity.arrow_forwardThe reaction 2NO(g) + O₂(g) → 2NO₂(g) is second order in NO and first order in O₂. When [NO] = 0.2 M and [0₂] = 3 M, the observed rate of the reaction is 0.00001116 M/s. (a) What is the value of the rate constant? (b) What are the units of the rate constant? Mºs-1 The rate constant has no unit. O S-¹ O M¹s-¹ M-2S-1 O M-¹5-² O M-¹ M-³5-1 O M³s O M-¹5-1 (c) What would happen to the rate if the concentration of NO were increased by a factor of 2.4? O The rate of the reaction would decrease O The rate of the reaction would increase By what factor would the rate of reaction increase? (d) What is the rate of reaction when [NO] = 0.1 M and [0₂] = 0.85 M? M/sarrow_forward
- [4] Consider the following mechanism for the reaction of nitric oxide and hydrogen: kı 2NO(g)+ H2(g) → N;O(g) + H¿O(g) slow k2 N,0(g) + H2(g) → N2(g) + H2O(g) fast (a) Write an equation for the overall reaction. (b) Write the theoretical rate law for the above mechanism. (c) Is a catalyst involved in the above mechanism? If so, what is it? (d) Are there any reaction intermediates? If so, list them.arrow_forwardGiven the following reactions and the corresponding rate laws, in which of the reactions might the elementary reaction and the overall reaction be the same? Cl2 + CO – Cl2CO (a) rate = k[C12V2 [COj PC13 + Cl2 PC15 - (b) rate = k[PC!3]Cl} 2NO +H2 (c) rate = k[NO][H2] → N2 + H2O 2NO +02 (d) rate = k[NO]?(0,l 2NO2 NO +03 (е) rate = k[NO][O3} NO2 +02arrow_forwardThe reaction 2 NO(g) + O₂(g) -> 2 NO₂(g) proceeds through the following mechanism: (a) The second step of this mechanism is rate-determining (slow). What is the rate law for this reaction? Ratek [NO] (O₂) Rate-k [NO] [0₂] Ratek [NO] [O₂)² Ratek [NO]1/2 [0₂] Ratek [NO] [0₂]1/2 O Rate-k [NO] 2 NO(g)--> N₂O₂(9) N₂O₂(g) + O₂(9) --> 2 NO₂(9) Ratek [NO]2 [0₂11/2arrow_forward
- Consider the following reaction: Q:4-1 2 NO(g) + 2 H;(g) → N;(8) + 2 H,0(g) (a) The rate law for this reaction is first order in H, and second order in NO. Write the rate law. (b) If the rate constant for this reaction at 1000 K is 6.0 × 10ª M-²s¯!, what is the re- action rate when [NO] = 0.035 M and [H,] = 0.015 M? (c) What is the reaction rate at 1000 K when the concentration of NO is increased to 0.10 M, while the concentration of H, is 0.010 M? (d) What is the reaction rate at 1000 K if [NO] is decreased to 0.010 M and [H,] is increased to 0.030 M? %3Darrow_forwardConsider the following hypothetical reaction: 2P + Q→ 2 R + S. The following mechanism is proposed for this reaction: P + P = T (fast) Q + T → R+ U (slow) U-R + S (fast) Substances T and U are unstable intermediates. What rate law is predicted by this mechanism? (a) Rate = k[P]? (b) Rate = k[P][Q] (c) Rate = k[P]°[QI (d) Rate = k[P][Q? (e) Rate = k[U]arrow_forwardConsider the following reaction: 4 HBr(g) + O2(g) 2 H2O(g) + 2 Br2(g) (a) The rate law for this reaction is first order in HBr(g) and first-order in O2(g). What is the rate law for this reaction? Rate = k [HBr(g)] [O2(g)]Rate = k [HBr(g)]2 [O2(g)] Rate = k [HBr(g)] [O2(g)]2Rate = k [HBr(g)]2 [O2(g)]2Rate = k [HBr(g)] [O2(g)]3Rate = k [HBr(g)]4 [O2(g)] (b) If the rate constant for this reaction at a certain temperature is 9920, what is the reaction rate when [HBr(g)] = 0.00467 M and [O2(g)] = 0.00876 M?Rate = M/s.(c) What is the reaction rate when the concentration of HBr(g) is doubled, to 0.00934 M while the concentration of O2(g) is 0.00876 M?Rate = M/sarrow_forward
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