(a)
Interpretation:
The order with respect to each reactant and the overall order of the reaction have to be determined.
Concept Introduction:
The rate of the reaction is referred to the change in the molar concentration in the distinct interval of time. According to the rate law, the rate of the reaction is directly proportional to the initial concentration of the reactant of the reaction.
(b)
Interpretation:
The expression for the rate law has to be determined.
Concept Introduction:
Same as part (a).
(c)
Interpretation:
The rate constant for the given reaction has to be determined.
Concept Introduction:
Same as part (a).
(d)
Interpretation:
The
Concept Introduction:
Same as part (a).
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ACHIEVE/CHEMICAL PRINCIPLES ACCESS 1TERM
- The decomposition of XY is second order in XY and has a rate constant of 7.41 × 10−3 L·mol−1·s−1 at a certain temperature, the half-life for this reaction at an initial concentration of 0.101 mol·L−1 1336. A) If the initial concentration of XY is 0.225 mol·L−1, how long will it take for the concentration to decrease to 6.95 × 10−2 mol·L−1 ?, B) If the initial concentration of XY is 0.080 mol·L−1, what is the concentration of XY after 75 s ?arrow_forwardConsider the following reaction: 1. 2 N,O5 (g) → 4 NO, (g) + O, (g) The initial concentration of N2O5 was 0.48 mol/L, and 25 minutes after initiating the reaction, all of the N,Os has been consumed. (a) Calculate the average rate of the reaction over this 25-minute time interval. (b) Is it correct to assume that the rate law is Rate = k[N,O5]² based on the balanced chemical equation? Briefly explain your answer.arrow_forwardThe reaction O₂(g) + 2 NO(g) → 2 NO₂(g) was studied at a certain temperature with the following results: (a) What is the rate law for this reaction? O Ratek [0₂(9)] [NO(g)] O Ratek [0₂(9)]² [NO(g)] O Rate = k [0₂(9)] [NO(g)]² O Ratek [0₂(9)]² [NO(g)]² O Ratek [0₂(9)] [NO(g)]³ O Rate = k [O₂(g)]* [NO(g)] (b) What is the value of the rate constant? Experiment [0₂(9)] (M) 0.0235 0.0235 0.0470 0.0470 [NO(g)] (M) 0.0235 0.0470 0.0235 0.0470 Rate (M/S) 0.158 0.633 0.317 1.27 (c) What is the reaction rate when the concentration of O₂(g) is 0.0318 M and that of NO(g) is 0.0649 M if the temperature is the same as that used to obtain the data shown above?arrow_forward
- The reaction 2 NO(g) + Cl2(g) → 2 NOCl has the following rate law: Rate = k[NO]2 [Cl2]. The initial speed of the reaction was found to be 5.72×10‒6 M/s when the reaction was carried out at 25 °C with initial concentrations of 0.500 M NO and 0.250 M Cl2. What is the value of k?(a) 1.83×10‒4(b) 1.09×104(c) 9.15×10‒5(d) 5.72×10‒6arrow_forwardAssume that the formation of nitrogen dioxide, 2 NO(g) + 02(g) – 2 NO2(g) is an elementary reaction. (a) Write the rate law for this reaction. (Rate expressions take the general form: rate = k. [A]ª . [B]b.) chemPad О Help Greek - rate=k•[NO]2.[02] rate=k*[NO]^2*[O_2] Correct. (b) A sample of air at a certain temperature is contaminated with 1.9 ppm of NO by volume. Under these conditions, can the rate law be simplified? If so, write the simplified rate law. If not, repeat your answer from above. (Rate expressions take the general form: rate = k . [A]ª . [B]b. Use k' for the new rate constant as needed.) chemPad O Help Greek - rate=k':[NO]2 rate=k*[NO]^2 Correct. (c) Under the conditions described in (b), the half-life of the reaction has been estimated to be 6.7x103 min. What would the half-life be if the initial concentration of NO were 12.4 ppm? 4.0 |1030192 X min Supporting Materials Periodic Table Constants and E Supplemental Dataarrow_forwardThe reaction O₂(g) + 2 NO(g) → 2 NO₂(g) was studied at a certain temperature with the following results: (a) What is the rate law for this reaction? O Rate = k [0₂(g)] [NO(g)] O Rate = k [0₂(g)]² [NO(g)] O Rate = k [0₂(g)] [NO(g)]² O Rate = k [O₂(g)]² [NO(g)]²2 O Rate = k [O₂(g)] [NO(g)]³ O Rate = k [0₂(g)]4 [NO(g)] (b) What is the value of the rate constant? Experiment M/s 1 2 3 4 [0₂(g)] (M) 0.0231 0.0231 0.0462 0.0462 [NO(g)] (M) 0.0231 0.0462 0.0231 0.0462 Rate (M/s) 0.112 0.448 0.224 0.896 (c) What is the reaction rate when the concentration of O₂(g) is 0.0437 M and that of NO(g) is 0.0567 M if the temperature is the same as that used to obtain the data shown above?arrow_forward
- Lanthanum(III) phosphate crystallizes as a hemihydrate, LAPO4 · H20. When it is heated, it loses water to give anhydrous lanthanum(III) phosphate: 2(LAPO4 · H2O(s)) → 2 LaPO4 (s) + H20(g) This reaction is first order in the chemical amount of LAPO, · H2O. The rate constant varies with tempera- ture as follows: Temperature (°C) k (s-1) 205 2.3 x 10-4 219 3.69 x 10-4 246 7.75 x 10-4 260 12.3 x 10-4 Compute the activation energy of this reaction.arrow_forward(9) The reaction 2A → B+C (molecular weight of A = 150.0 amu; B = 75.0 amu) has a rate constant of 0.112 s¹. (a) If the initial concentration of A is 0.200 M, what is the mass (in grams) of A that are left after 2.00 s when the reaction is run in a 2.00 L flask? (b) What is the mass (in grams) of B that are produced in the reaction?arrow_forward5*) a) The reaction A B has been experimentally determined to be second order. The initial rate is 0.0100 M/s at an initial concentration of [A] of 0.100 M. What is the initial rate at [A]o = 0.500 M? b) The reaction below was experimentally determined to be first order with respect to O2 and second order with respect to NO. O2(g) + 2 NO(g) → 2 NO2(g) The diagrams provided represent reaction mixtures in which the number of each type of molecule represents its relative initial concentration. Which mixture has the fastest initial rate? Explain. KEY: = 02 = NO (i) (ii) (iii)arrow_forward
- The reaction 2 NO₂(g) + O₂(g) → N₂O5(g) + O₂(g) was studied at a certain temperature with the following results: (a) What is the rate law for this reaction? Rate = k [NO₂(g)] [03(g)] O Rate = k [NO₂(g)]² [03(g)] O Rate = k [NO₂(g)] [03(g)]² O Rate = k [NO₂(g)]² [03(g)]² O Rate = k [NO₂(g)] [03(g)]³ O Rate = k [NO₂(g)]* [03(g)] (b) What is the value of the rate constant? 137268 Experiment M/S AWNPE 1 2 3 4 [NO₂(g)] (M) 0.718 0.718 1.44 1.44 [03(g)] (M) 0.718 1.44 0.718 1.44 Rate (M/s) (c) What is the reaction rate when the concentration of NO₂(g) is 1.26 M and that of O3(g) is 2.10 M if the temperature is the same as that used to obtain the data shown above? 26600 53400 53400 1.07e+05arrow_forwardIn a study of the formation of HI from its elements, H2(g) + 12(g) == 2HI(g) equal amounts of H2 and 12 were placed in a container, which was then sealed and heated. (a) On one set of axes, sketch concentration vs. time curves for H and HI, and explain how Q changes as a function of time. (b) Is the value of Q different if [12] is plotted instead of [H2]?arrow_forward1) A reagent used in organic synthesis, decomposes in acidic solution by following a first-order kinetic, producing B and CO2(g). A(aq) → B(aq) + CO2(g) If the half-life of this decomposition reaction is 143.5 min, (a) What is the time required for the 65% decomposition of A(aq)? (b) How many liters of CO2(g), measured at 24.5 °C and 747 mmHg, are produced when 10.0 g sample decomposes for 575 min? (A = 102.09 g/mol; R= 0.082 L atm/mol K).arrow_forward
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