1. For an irreversible reaction A products, the graph of 1/[A] as a function of time is linear. What is the reaction order in A? a. Zeroth-order b. First-order c. Second-order d. The order in A cannot be determined based on the information given. 2. A proposed mechanism for the reduction of nitrogen as NO by hydrogen is: Step 1: H₂ (g) + 2 NO (g) → N₂O (g) + H₂O (g) - Step 2: N₂O (g) + H₂ (g) → N2 (g) + H₂O (g) What is the molecularity of Step 2? a. unimolecular b. bimolecular c. termolecular d. zero molecular (spontaneous) e. More information is needed to answer this question. 3. Which one of the following will change the value of an equilibrium constant? a. changing temperature b. adding other substances that do not react with any of the species involved in the equilibrium c. varying the initial concentrations of reactants d. varying the initial concentrations of products e. changing the volume of the reaction vessel

1. For an irreversible reaction A products, the graph of 1/[A] as a function of time is linear. What is the reaction order in A? a. Zeroth-order b. First-order c. Second-order d. The order in A cannot be determined based on the information given. 2. A proposed mechanism for the reduction of nitrogen as NO by hydrogen is: Step 1: H₂ (g) + 2 NO (g) → N₂O (g) + H₂O (g) - Step 2: N₂O (g) + H₂ (g) → N2 (g) + H₂O (g) What is the molecularity of Step 2? a. unimolecular b. bimolecular c. termolecular d. zero molecular (spontaneous) e. More information is needed to answer this question. 3. Which one of the following will change the value of an equilibrium constant? a. changing temperature b. adding other substances that do not react with any of the species involved in the equilibrium c. varying the initial concentrations of reactants d. varying the initial concentrations of products e. changing the volume of the reaction vessel

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

8. Smelling salt decomposes spontaneously at room temperature by the equation below. A student places a 10.00-g sample into a 1-liter sealed rigid vessel. What measurements should the student make to determine the rate of this reaction?(NH4)2CO3(s)→2NH3(g)+H2O(g)+CO2(g) a. change in mass and temperature b. temperature and time c. change in mass and time d. change in pressure and time
The half-life (t1/2) of a first-order reaction is 1.00 s. What is the value of the rate constant? A. 6.93 s–1 B. 0.144 s–1 C. 0.0693 s–1 D. 0.693 s–1 E. 3.01 s–1
The reaction NO3 (g) + NO(g) → 2 NO2 has a rate of rate=k[NO3]3. What is the order with respect to NO? A. First order B. Second order C. Third order D. Zero order
For the reaction:A(g) + B(g) →AB(g) the rate is 0.30 mol/L.s, when [A]0 = [B]0 = 1.0 mol/L. If the reaction is first order in B and second order in A, what is the rate when [A]0 = 1.9 mol/L and [B]0 = 4.3 mol/L?
22. Be sure to answer all parts.The reaction2A + 3B → C is first order with respect to A and B. When the initial concentrations are [A] = 1.70 × 10−2 M and [B] = 2.27 × 10−3 M, the rate is 4.33 × 10−4 M/s. Calculate the rate constant of the reaction.Enter your answer in scientific notation.
36 The reaction C2H5Cl →C2H4 + HCl is first order in C2H5Cl. The rate constant is 1.60 x 10-6/s. In an investigation of the decomposition of C2H5Cl an initial concentration of 0.165 mol/L was used. What will the concentration of C2H5Cl be after 125 hours? Select one: a. 0.0803 M b. 0.0703 M c. 0.0603 M d. 0.0503M
The rate for the overall reaction NO2 (g) + CO (g) → NO (g) + CO2 (g) is Rate = k[NO2]2 a. Consider this mechanism: i. 2NO2 (g) → N2 (g) + 2O2 (g) [slow] ii. 2CO (g) + O2 (g) → 2CO2 (g) [fast] iii. N2 (g) + O2 (g) →2NO (g) [fast] d. Draw a reaction energy diagram for this mechanism, given that the overall reaction’s ΔH°rxn = -226 kJ/mol.
The reaction between hydrogen and chlorine is as follows: Cl2(g) + H2(g) → 2HCl(g) Experiments show that this reaction is first order with respect to H2 and one-half order with respect to Cl2. What is the rate law? a. Rate = k [H2]1/2 [Cl2] b. Rate = k [Cl2] [H2]2 c. Rate = k [Cl2]1/2 [H2] d. Rate = k [Cl2]2 [H2]
Hydrogen peroxide, H₂O₂ (aq), decomposes to H₂O₂(l) and Q₂ (g) in a reaction that is first-order in H₂O₂ and has a rate constant k = 1.06 × 10-³ min-¹ at a given temperature. a. How long will it take for 10.% of a sample of H₂O₂ to decompose? min b. How long will it take for 86% of the sample to decompose? min
Molecular iodine, I2 (g), dissociates into iodine atoms at 652 K, with a first order rate constant of 0.452 s-1. I2(g) -----> 2I a. What is the half life for this reaction? b. If you start with 0.35 M I2 at this temperature, how long will it take for the concentration of I2 to reach 0.12 M?