Problem: Given the reaction H₂ (g) + N₂ (g) → NH3 (g) (a) write the corresponding expressions for the reaction rate in terms of each reactant and product (hint: you may need to balance the equation first) (b) if oxygen gas is consumed at a rate of 4.96×10-5 M/s, what is the corresponding reaction rate and what is the rate of consumption of H₂ (g) and the rate of formation of NH3(g)?

Problem: Given the reaction H₂ (g) + N₂ (g) → NH3 (g) (a) write the corresponding expressions for the reaction rate in terms of each reactant and product (hint: you may need to balance the equation first) (b) if oxygen gas is consumed at a rate of 4.96×10-5 M/s, what is the corresponding reaction rate and what is the rate of consumption of H₂ (g) and the rate of formation of NH3(g)?

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...

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Account for the relationship between the rate of a reaction and its activation energy, and the relationship between the rate of the reaction and the reaction temperature. Group of answer choices The rate of reaction will increase as the activation energy decreases; the rate of reaction will increase as the reaction temperature increases. The rate of reaction will increase as the activation energy decreases; the rate of reaction will remain the same as the reaction temperature increases. The rate of reaction will increase as the activation energy increases; the rate of reaction will increase as the reaction temperature increases. The rate of reaction will remain the same as the activation energy decreases; the rate of reaction will increase as the reaction temperature increases. The rate of reaction will increase as the activation energy decreases; the rate of reaction will decrease as the reaction temperature increases.
The mechanism for the reaction of CH3OH andHBr is believed to involve two steps. The overallreaction is exothermic.Step 1: Fast, endothermicCH3OH + H+ uv CH3OH2+Step 2: SlowCH3OH2+ + Br− n CH3Br + H2O(a) Write an equation for the overall reaction.(b) Draw a reaction coordinate diagram for thisreaction.(c) Show that the rate law for this reaction isRate = k[CH3OH][H+][Br−].
Problem: Given the reaction NO₂ (g) + CO (g) 2 (a) Determine the order with respect to 0₂ (b) Determine the order with respect to NO (c) Write the complete rate law (d) Determine the value of the rate constant k Experiment 1 2 3 Initial Rate (M/s) 0.00501 0.0803 0.00502 NO (g) + CO₂ (g) and initial rate data below: Initial [NO₂] (M) 0.100 0.400 0.100 Initial [CO] (M) 0.100 0.100 0.200
Problem: The rate law for the reaction 2 H₂ (g) + 2 NO (g)→ N₂ (g) + 2 H₂O (g) is observed to be rate = k[NO]²[H₂]. Three possible mechanisms have been proposed; which can be ruled out? Proposed Mechanism I: NO (g) + H₂(g) →→→ H₂O (g) + N (g) [slow] N (g) + NO (g) → N₂ (g) + 0 (g) [fast] H₂O (g) [fast] 2 O(g) + H₂(g) → Proposed Mechanism II: 2 NO(g) + H₂(g) → N₂0 (g) + H₂O (g) [slow] N₂O(g) + H₂(g) → N₂ (g) + H₂O (g) [fast] Proposed Mechanism III: 2 NO (g) = N₂O₂ (g) [fast equilibrium] N₂O₂(g) + H₂(g) → N₂0 (g) + H₂O (g) [fast] N₂O(g) + H₂(g) → N₂ (g) + H₂O (g) [fast]
Indicate whether it is true or false: ( ) Electromotive force is defined as a potential difference and can be accurately measured using a potentiometer. ( ) When the rate of product formation is independent of the reactant concentration, it is called a zero-order reaction. ( ) In a chemical reaction profile graph, the activation energy can be determined by the difference between the energy of the products and the reactants. ( ) The equilibrium constant of a chemical reaction at a given temperature is independent of concentrations or pressures. ( ) The compounds NaCl, KBr, KOH and H2O are considered strong electrolytes. ( ) Weak electrolytes do not ionize completely and are usually covalent compounds. ( ) The equilibrium constant depends on the temperature. ( ) In chemical equilibrium, the standard free energy of the reaction is equal to the equilibrium constant.
1. Which of the following statements is incorrect? (A) The reaction in which the rate equation corresponds to a stoichiometric equation is called an elementary reaction. (B) Molecularity of a reaction may not be equal to the order of reaction. (C) With increase in temperature, the rate constant obeying Arrhenius equation decreases. (D) Rate of a chemical reaction is independent of the concentration of the reactants for a zero order reaction. 2. The rate of a gas phase reaction is given by, kCACB. If the volume of the reaction vessel is reduced to l/3rd of its initial volume, then the reaction rate compared to the original rate will be _____ times. (A) 3 (C) 6 (B) 9 (D) 12 3. A given number of molecules (i.e., moles) of a particular chemical species have reacted or disappeared when any of the following occurs except (A) Combination (C) Isomerization (B) Decomposition (D) Isolation Please Answer all!
(a) A certain first-order reaction has an activation energy of 53 kJ mol-!. It is run twice, first at 298 K and then at 308 K (10°C higher). All other conditions are iden- tical. Show that, in the second run, the reaction occurs at double its rate in the first run. (b) The same reaction is run twice more at 398 K and 408 K. Show that the reaction goes 1.5 times as fast at 408 K as it does at 398 K.
36. The gas-phase reaction H+ D2 → HD + D is the exchange of isotopes of hydrogen of atomic mass 1 (H) and 2 (D, deuterium). The following data were obtained for the rate constant k of this reaction: Temperature (K) k (L mol-1 s-1) 299 1.56 x 104 327 3.77 x 104 346 7.6 x 104 440 106 549 1.07 × 105 745 8.7 x 107
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(а) (b) (c) (d) all react at same rate
what is the mechanism if this reaction?
1. (a) Show that decomposition of the organic compound 1,3-pentadiene is a second-order reaction and determine the rate constant. The concentration of 1,3-pentadiene was measured as a function of time. The data are as follows: (b) What is the value of the rate constant for the decomposition of 1,3-pentadiene.(c) What is the initial concentration for the reaction? Report to 3 significant figures.(d) What is the concentration of 1,3-pentadiene after 3.750 x10^3 s? Time(s) [1,3-pentadiene] (M) 0 .480 1000 .179 2000 .110 3000 .0795 4000 .0622 5000 .0510