**Consider the following reaction:**\[ 2 \text{NO}_2(g) + \text{O}_3(g) \rightarrow \text{N}_2\text{O}_5(g) + \text{O}_2(g) \]---**(a) The rate law for this reaction is first order in \(\text{NO}_2(g)\) and first order in \(\text{O}_3(g)\). What is the rate law for this reaction?**- [ ] Rate = k \([\text{NO}_2(g)] [\text{O}_3(g)]\)- [ ] Rate = k \([\text{NO}_2(g)]^2 [\text{O}_3(g)]\)- [ ] Rate = k \([\text{NO}_2(g)] [\text{O}_3(g)]^2\)- [ ] Rate = k \([\text{NO}_2(g)]^2 [\text{O}_3(g)]^2\)- [ ] Rate = k \([\text{NO}_2(g)] [\text{O}_3(g)]^3\)- [ ] Rate = k \([\text{NO}_2(g)]^4 [\text{O}_3(g)]\)---**(b) If the rate constant for this reaction at a certain temperature is 97900, what is the reaction rate when \([\text{NO}_2(g)] = 0.587 \, M\) and \([\text{O}_3(g)] = 1.40 \, M\)?**Rate = \(\_\_\_\_\_\) M/s.---**(c) What is the reaction rate when the concentration of \(\text{NO}_2(g)\) is doubled, to 1.17 M, while the concentration of \(\text{O}_3(g)\) is 1.40 M?**Rate = \(\_\_\_\_\_\) M/s.

According to the rate law ; rate of reaction is directly proportional to the active masses of the…

Consider the following reaction: (a) The rate law for this reaction is first order in NO₂(g) and first order in O3(g). What is the rate law for this reaction? Rate = k [NO₂(g)] [03(g)] Rate = k [NO₂(g)]² [03(g)] Rate = k [NO₂(g)] [03(g)]² O Rate = k [NO₂(g)]² [03(g)]² Rate = k [NO₂(g)] [03(g)]³ Rate = k [NO₂(g)]4 [03(g)] (b) If the rate constant for this reaction at a certain temperature is 97900, what is the reaction rate when [NO₂(g)] = 0.5 M and [03(9)] = 1.40 M? Rate = 2 NO₂(g) + 03(9) → N₂O5(9) + O₂(g) M/s. Rate = (c) What is the reaction rate when the concentration of NO₂(g) is doubled, to 1.17 M while the concentration of O3(g) is 1.40 M? M/s

Consider the following reaction: (a) The rate law for this reaction is first order in NO₂(g) and first order in O3(g). What is the rate law for this reaction? Rate = k [NO₂(g)] [03(g)] Rate = k [NO₂(g)]² [03(g)] Rate = k [NO₂(g)] [03(g)]² O Rate = k [NO₂(g)]² [03(g)]² Rate = k [NO₂(g)] [03(g)]³ Rate = k [NO₂(g)]4 [03(g)] (b) If the rate constant for this reaction at a certain temperature is 97900, what is the reaction rate when [NO₂(g)] = 0.5 M and [03(9)] = 1.40 M? Rate = 2 NO₂(g) + 03(9) → N₂O5(9) + O₂(g) M/s. Rate = (c) What is the reaction rate when the concentration of NO₂(g) is doubled, to 1.17 M while the concentration of O3(g) is 1.40 M? M/s

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

An experiment was performed and the concentration of A and B was 1.300 M and 1.708 M, respectively. The rate of this reaction was 17.181 M/s. The rate law for this reaction was determined to be Rate = k(A)3(B)3. Calculate the rate constant, k.
Dinitrogen Pentoxide, N2O5, decomposes when heated to give in carbon tetrachloride solvent. N2O5(g) → 2 NO2(g) + 1/2 O2(g) The reaction is first order in N2O5. If the rate constant for the decomposition is (8.20x10^0)x10-4/min, how long, in minutes, would it take for the concentration of N2O5 to decrease to 6.25% of its initial value? Express your answer to three significant figures.
In a reversible reaction between A and B, k1 is the rate constant for the formation of B from A, and k–1 is the rate constant for the formation of A from B. What is the rate equation if both reactions are first order with respect to the reactant? Rate of disappearance of A = k1 [A] – k–1 [B] Rate of disappearance of A = k1 [A] + k–1 [B] Rate of disappearance of A = k–1 [A] + k1 [B] Rate of disappearance of A = (k–1/k1) [A][B] Rate of disappearance of A = k–1 [A] – k1 [B]
3. (a) The following data were collected for the reaction between hydrogen and nitric oxide at 700 degrees Celsius: (i) Determine the order of the reaction. (ii) Calculate the rate constant. (b) Consider the reaction ( ) 3 ( ) 2 ( ) N2 g  H2 g  NH3 g Suppose that at a particular moment during the reaction molecular hydrogen is reacting at the rate of 0.074 M/s. (i) At what rate is ammonia being formed? (ii) At what rate is molecular nitrogen reacting?
The rate of a certain reaction is given by the following rate law: rate = k[NO]²[0₂] Use this information to answer the questions below. What is the reaction order in NO? What is the reaction order in O₂? What is overall reaction order? At a certain concentration of NO and O2, the initial rate of reaction is 6.0 x 105 M/s. What would the initial rate of the reaction be if the concentration of NO were doubled? Round your answer to 2 significant digits. The rate of the reaction is measured to be 6.0 M/s when [NO] = 1.3 M and [0₂] = 1.2 M. Calculate the value of the rate constant. Round your answer to 2 significant digits. 0 1 k = M 04/1 S -2 -1 - м - OM ²²-5-¹ S
Consider this balanced chemical equation:H2O2(aq) + 3 I - (aq) + 2 H+ (aq)------> I3 - (aq) + 2 H2O(l )In the first 10.0 seconds of the reaction, the concentration of I - drops from 1.000 M to 0.868 M.(a) Calculate the average rate of this reaction in this time interval.(b) Determine the rate of change in the concentration of H+ (that is, Δ[H+]>Δt) during this time interval.
The initial rate of the reaction is determined for different initial conditions, with the results listed in the table. (a) What is the overall reaction order? (b) What is the value of the rate constant, k
Under certain conditions the rate of this reaction is zero order in dinitrogen monoxide with a rate constant of 0.0066 M·s : 2 N20(g) → 2 N2(8)+O2(g) Suppose a 250. mL flask is charged under these conditions with 150. mmol of dinitrogen monoxide. How much is left 20. s later? You may assume no other reaction is important. Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits. x10
How do I answer 30?
The rate of a certain reaction is given by the following rate law: = k[N₂]²[H₂]² Use this information to answer the questions below. rate= What is the reaction order in N₂? What is the reaction order in H₂? What is overall reaction order? At a certain concentration of N₂ and H₂, the initial rate of reaction is 6.0 x 105 M/s. What would the initial rate of the reaction be if the concentration of N₂ were doubled? Round your answer to 2 significant digits. The rate of the reaction is measured to be 97.0 M/s when [N₂] = 1.2 M and [H₂] = 0.36 M. Calculate the value of the rate constant. Round your answer to 2 significant digits. k = -3 DM 11 0 0 0 M. -1
Consider the following reaction: A + B --> products. The rate law was found to be rate = k[A][B]^2. If the concentration of B is doubled while the concentration of A is halved, how will this affect the rate of the equation? How will this affect the time required for the reaction to reach completion?
Chlorine oxide (CIO), which plays an important role in the depletion of ozone, decays rapidly according to the equation 2CIO(g) →→→ Cl₂(g) + O₂(g) - From the following data, determine the reaction order and calculate the rate constant of the reaction. Time (s) [CIO] (M) 2.91 x 103 8.11 × 10-6 3.64 x 10-3 5.77 × 10-6 4.37x103 4.48 x 10-6 5.10 x 10 3 3.66 x 10-6 5.83 x 10-3 3.09 x 10-6 Reaction order: O O 1 2 Rate constant: k = x 10 Ms (Enter your answer in scientific notation.)