Questions 5 & 6 both use the chemical reaction below: Cr3+ (aq) + SCN (aq) CrSCN²+ (aq) Solutions of Cr(NO3)3 and KSCN are mixed so that the initial [Cr³+] in the solution is 0.899 M. At equilibrium, the [CrSCN2+] is found to be 0.138 M. What is the [Cr³+] at equilibrium? Enter your answer as a number without units. Your Answer: Answer Question 12 In a separate reaction under certain conditions, the following concentrations are found at equilibrium: [Cr³+] = 0.0167 M, [CrSCN2+] = 0.681 M, and [SCN'] = 0.0824 M. Calculate the value of K for the reaction at this temperature. Enter your answer as a number without units.
Questions 5 & 6 both use the chemical reaction below: Cr3+ (aq) + SCN (aq) CrSCN²+ (aq) Solutions of Cr(NO3)3 and KSCN are mixed so that the initial [Cr³+] in the solution is 0.899 M. At equilibrium, the [CrSCN2+] is found to be 0.138 M. What is the [Cr³+] at equilibrium? Enter your answer as a number without units. Your Answer: Answer Question 12 In a separate reaction under certain conditions, the following concentrations are found at equilibrium: [Cr³+] = 0.0167 M, [CrSCN2+] = 0.681 M, and [SCN'] = 0.0824 M. Calculate the value of K for the reaction at this temperature. Enter your answer as a number without units.
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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Question 12
![Questions 5 & 6 both use the chemical reaction below:
Cr³+ (aq) + SCN (aq)
CrSCN²+ (aq)
Solutions of Cr(NO3)3 and KSCN are mixed so that the initial [Cr³+] in the solution is
0.899 M. At equilibrium, the [CrSCN2+] is found to be 0.138 M. What is the [Cr³+] at
equilibrium? Enter your answer as a number without units.
Your Answer:
Answer
Question 12
In a separate reaction under certain conditions, the following concentrations are
found at equilibrium: [Cr3+] = 0.0167 M. [CrSCN2+] = 0.681 M, and [SCN] = 0.0824
M. Calculate the value of K for the reaction at this temperature. Enter your answer as
a number without units.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F707cabdc-1809-4680-b100-3c0d66ee6663%2F0b4335ea-560f-4f29-b76f-ddff19744692%2Fk1y1wy8_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Questions 5 & 6 both use the chemical reaction below:
Cr³+ (aq) + SCN (aq)
CrSCN²+ (aq)
Solutions of Cr(NO3)3 and KSCN are mixed so that the initial [Cr³+] in the solution is
0.899 M. At equilibrium, the [CrSCN2+] is found to be 0.138 M. What is the [Cr³+] at
equilibrium? Enter your answer as a number without units.
Your Answer:
Answer
Question 12
In a separate reaction under certain conditions, the following concentrations are
found at equilibrium: [Cr3+] = 0.0167 M. [CrSCN2+] = 0.681 M, and [SCN] = 0.0824
M. Calculate the value of K for the reaction at this temperature. Enter your answer as
a number without units.
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