Question 5 The equilibrium constant (K) of the reaction is 9.10: If at equilibrium, [H₂] = 0.300 M and [NH₂] = 0.200 M, what is the concentration of N, at equilibrium? M N₂(g) + 3H₂(g) = 2 NH3(g) M Type numbers in the boxes. Part 1: 10 points Part 2: 10 points 20 points At a different temperature for this same reaction the equilibrium constant (K) is determined to be 4.47. At this new temperature, at equilibrium [H₂] = 0.200 and [N₂] = 0.200. What is the [NH,] at equilibrium for this reaction? Question 1 Which of the following statements for a chemical reaction at equilibrium is true? A. O The rate of the forward reaction becomes zero. B. The concentration(s) of the reactant(s) equals the concentration(s) of the product(s). C. The rates of the forward and reverse reactions are equal. D. O The concentration(s) of the reactant(s) becomes zero. Question 2 What is the expression for the equilibrium constant (K) for the general reaction? mA + nB = xC + yD A. B.O C.O D. O Kp Kp Kp Kp (Pc)(PD") (PA") (PB") (PA") (PB") (Pc)(PD") (Pc)(Pb) (PA) (PB) (PA)(PB) (Pc)(Pb) Select one answer. 5 points Question 3 Indicate whether the following statements are true or false concerning the reaction quotient (Q) and the equilibrium constant (K). When the value of Q is less than the value of K, the equilibrium shifts to the right. [true When the value of Q equals to the value of K, the equilibrium is reached. true When the value of Q is larger than the value of K, the equilibrium shifts to the left. [true The value of Q cannot be equal to the value of K. [true Select one answer. 5 points Fill in the blanks by selecting one option from each menu. Part 1:2 points Part 2:2 points Part 3:2 points *Part 4:2 points 8 points
Question 5 The equilibrium constant (K) of the reaction is 9.10: If at equilibrium, [H₂] = 0.300 M and [NH₂] = 0.200 M, what is the concentration of N, at equilibrium? M N₂(g) + 3H₂(g) = 2 NH3(g) M Type numbers in the boxes. Part 1: 10 points Part 2: 10 points 20 points At a different temperature for this same reaction the equilibrium constant (K) is determined to be 4.47. At this new temperature, at equilibrium [H₂] = 0.200 and [N₂] = 0.200. What is the [NH,] at equilibrium for this reaction? Question 1 Which of the following statements for a chemical reaction at equilibrium is true? A. O The rate of the forward reaction becomes zero. B. The concentration(s) of the reactant(s) equals the concentration(s) of the product(s). C. The rates of the forward and reverse reactions are equal. D. O The concentration(s) of the reactant(s) becomes zero. Question 2 What is the expression for the equilibrium constant (K) for the general reaction? mA + nB = xC + yD A. B.O C.O D. O Kp Kp Kp Kp (Pc)(PD") (PA") (PB") (PA") (PB") (Pc)(PD") (Pc)(Pb) (PA) (PB) (PA)(PB) (Pc)(Pb) Select one answer. 5 points Question 3 Indicate whether the following statements are true or false concerning the reaction quotient (Q) and the equilibrium constant (K). When the value of Q is less than the value of K, the equilibrium shifts to the right. [true When the value of Q equals to the value of K, the equilibrium is reached. true When the value of Q is larger than the value of K, the equilibrium shifts to the left. [true The value of Q cannot be equal to the value of K. [true Select one answer. 5 points Fill in the blanks by selecting one option from each menu. Part 1:2 points Part 2:2 points Part 3:2 points *Part 4:2 points 8 points
Chemistry & Chemical Reactivity
10th Edition
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter15: Principles Of Chemical Reactivity: Equilibria
Section: Chapter Questions
Problem 38GQ: At 2300 K the equilibrium constant for the formation of NO(g) is 1.7 103. N2(g) + O2(g) 2 NO(g)...
Related questions
Question
![Question 5
The equilibrium constant (K) of the reaction is 9.10:
If at equilibrium, [H₂] = 0.300 M and [NH₂] = 0.200 M, what is the concentration of N, at
equilibrium?
M
N₂(g) + 3H₂(g) = 2 NH3(g)
M
Type numbers in the boxes.
Part 1: 10 points
Part 2: 10 points
20 points
At a different temperature for this same reaction the equilibrium constant (K) is determined to be 4.47.
At this new temperature, at equilibrium [H₂] = 0.200 and [N₂] = 0.200. What is the [NH,] at equilibrium for this
reaction?](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F5d8f76dc-6c73-4d70-9f36-edd8bf23a157%2F636f5433-c648-4c42-ad1d-84632b860d31%2Fmphl6ol_processed.png&w=3840&q=75)
Transcribed Image Text:Question 5
The equilibrium constant (K) of the reaction is 9.10:
If at equilibrium, [H₂] = 0.300 M and [NH₂] = 0.200 M, what is the concentration of N, at
equilibrium?
M
N₂(g) + 3H₂(g) = 2 NH3(g)
M
Type numbers in the boxes.
Part 1: 10 points
Part 2: 10 points
20 points
At a different temperature for this same reaction the equilibrium constant (K) is determined to be 4.47.
At this new temperature, at equilibrium [H₂] = 0.200 and [N₂] = 0.200. What is the [NH,] at equilibrium for this
reaction?
Transcribed Image Text:Question 1
Which of the following statements for a chemical reaction at equilibrium is true?
A. O The rate of the forward reaction becomes zero.
B. The concentration(s) of the reactant(s) equals the concentration(s) of the product(s).
C. The rates of the forward and reverse reactions are equal.
D. O The concentration(s) of the reactant(s) becomes zero.
Question 2
What is the expression for the equilibrium constant (K) for the general reaction?
mA + nB = xC + yD
A.
B.O
C.O
D. O
Kp
Kp
Kp
Kp
(Pc)(PD")
(PA") (PB")
(PA") (PB")
(Pc)(PD")
(Pc)(Pb)
(PA) (PB)
(PA)(PB)
(Pc)(Pb)
Select one answer.
5 points
Question 3
Indicate whether the following statements are true or false concerning the reaction quotient
(Q) and the equilibrium constant (K).
When the value of Q is less than the value of K, the equilibrium shifts to the right. [true
When the value of Q equals to the value of K, the equilibrium is reached. true
When the value of Q is larger than the value of K, the equilibrium shifts to the left. [true
The value of Q cannot be equal to the value of K. [true
Select one answer.
5 points
Fill in the blanks by selecting
one option from each menu.
Part 1:2 points
Part 2:2 points
Part 3:2 points
*Part 4:2 points
8 points
Expert Solution
This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
Step by step
Solved in 1 steps with 3 images
Recommended textbooks for you
Chemistry & Chemical Reactivity
Chemistry
ISBN:
9781337399074
Author:
John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:
Cengage Learning
Chemistry & Chemical Reactivity
Chemistry
ISBN:
9781133949640
Author:
John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry & Chemical Reactivity
Chemistry
ISBN:
9781337399074
Author:
John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:
Cengage Learning
Chemistry & Chemical Reactivity
Chemistry
ISBN:
9781133949640
Author:
John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry: An Atoms First Approach
Chemistry
ISBN:
9781305079243
Author:
Steven S. Zumdahl, Susan A. Zumdahl
Publisher:
Cengage Learning
Chemistry by OpenStax (2015-05-04)
Chemistry
ISBN:
9781938168390
Author:
Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:
OpenStax