Time Consider the reaction represented by the equation 2X + 22 - X,Z,. During a reaction in which a large excess of reactant X was present, the concentration of reactant Z was monitored over time. A plot of the natural logarithm of the concentration of Z versus time is shown in the figure above. The order of the reaction with respect to reactant Z is Izl uI
Time Consider the reaction represented by the equation 2X + 22 - X,Z,. During a reaction in which a large excess of reactant X was present, the concentration of reactant Z was monitored over time. A plot of the natural logarithm of the concentration of Z versus time is shown in the figure above. The order of the reaction with respect to reactant Z is Izl uI
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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![Time
Consider the reaction represented by the equation
2 X + 2Z X,Z2. During a reaction in which
a large excess of reactant X was present, the
concentration of reactant Z was monitored over
time. A plot of the natural logarithm of the
concentration of Z versus time is shown in the
figure above. The order of the reaction with
respect to reactant Z is
(A) zero order
(B) first order
(C) second order
(D) third order](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Ff5623a21-96a6-4e52-bd12-f1a647763b36%2F2a1dca3c-af9f-4902-ab92-c9584f90db1d%2F6865gd_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Time
Consider the reaction represented by the equation
2 X + 2Z X,Z2. During a reaction in which
a large excess of reactant X was present, the
concentration of reactant Z was monitored over
time. A plot of the natural logarithm of the
concentration of Z versus time is shown in the
figure above. The order of the reaction with
respect to reactant Z is
(A) zero order
(B) first order
(C) second order
(D) third order
![N2(8) + 3 H,(g) 2 2 NH,(8)
AH398 =-92 kJ/mol,i AG298 =-33 kJ/mol,
Consider the reaction represented above at 298 K.
When equal volumes of N,(g) and H,(g), each at
1 atm, are mixed in a closed container at 298 K,
no formation of NH,(g) is observed. Which of the
following best explains the observation?
(A) The N2(g) and the H,(g) must be mixed in a
1:3 ratio for a reaction to occur.
(B) A high activation energy makes the forward
reaction extremely slow at 298 K.
(C) The reaction has an extremely small
equilibrium constant, thus almost no
product will form.
(D) The reverse reaction has a lower activation
energy than the forward reaction, so the
forward reaction does not occur.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Ff5623a21-96a6-4e52-bd12-f1a647763b36%2F2a1dca3c-af9f-4902-ab92-c9584f90db1d%2F6a1qf5i_processed.jpeg&w=3840&q=75)
Transcribed Image Text:N2(8) + 3 H,(g) 2 2 NH,(8)
AH398 =-92 kJ/mol,i AG298 =-33 kJ/mol,
Consider the reaction represented above at 298 K.
When equal volumes of N,(g) and H,(g), each at
1 atm, are mixed in a closed container at 298 K,
no formation of NH,(g) is observed. Which of the
following best explains the observation?
(A) The N2(g) and the H,(g) must be mixed in a
1:3 ratio for a reaction to occur.
(B) A high activation energy makes the forward
reaction extremely slow at 298 K.
(C) The reaction has an extremely small
equilibrium constant, thus almost no
product will form.
(D) The reverse reaction has a lower activation
energy than the forward reaction, so the
forward reaction does not occur.
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