section: CQB) CHEM 102B/C Fall 2019 (Student Messages Courses Help Logout Lorcan James McGrath Main Menu Contents Grades Course Contents » ... » Homework 11 » Homework 11-4 Timer Consider the following reaction for which K = 1.60 x 10-7 at some temperature: 2 NOCI (g) 2 NO (g) + Cl2(g) In a given experiment, 0.845 moles of NOCI (g) were placed in an otherwise empty 1.51 L vessel. Complete the following table by entering numerical values in the Initial row and values containing the variable "x" in the Change and Equilibrium rows. Define 2x as the amount (mol/L) of NOCI that reacts to reach equilibrium. Include signs in the Change column to indicate a gain or loss of concentration (Omit units, use 3 sig.fig. and write concentrations less than 1 as 0.###, not as .# ##. If nothing is present initially, enter 0 for the molarity.) [Cl2] (M) [NOCI] (M) [NO] (M) Initial Change Equilibrium Incorrect. Tries 3/99 Previous Tries Submit Answer Since K is very small, K = 1.60 x 10-7, very little product will be present at equilibrium, which tells us that very little NOCI will react to reach equilibrium. Because of this, the equilibrium concentration of NOCI will remain, essentially, at its initial concentration. Making this assumption, calculate the equilibrium concentration of NO. Note: use the ICE table from the previous problem to help you solve this problem. (Scientific notation can be entered using the following convention: 1.93 x 10-3 = 1.93E-3.) [NOleq= Tries 0/99 Submit Answer Post Discussion Send Feedback
section: CQB) CHEM 102B/C Fall 2019 (Student Messages Courses Help Logout Lorcan James McGrath Main Menu Contents Grades Course Contents » ... » Homework 11 » Homework 11-4 Timer Consider the following reaction for which K = 1.60 x 10-7 at some temperature: 2 NOCI (g) 2 NO (g) + Cl2(g) In a given experiment, 0.845 moles of NOCI (g) were placed in an otherwise empty 1.51 L vessel. Complete the following table by entering numerical values in the Initial row and values containing the variable "x" in the Change and Equilibrium rows. Define 2x as the amount (mol/L) of NOCI that reacts to reach equilibrium. Include signs in the Change column to indicate a gain or loss of concentration (Omit units, use 3 sig.fig. and write concentrations less than 1 as 0.###, not as .# ##. If nothing is present initially, enter 0 for the molarity.) [Cl2] (M) [NOCI] (M) [NO] (M) Initial Change Equilibrium Incorrect. Tries 3/99 Previous Tries Submit Answer Since K is very small, K = 1.60 x 10-7, very little product will be present at equilibrium, which tells us that very little NOCI will react to reach equilibrium. Because of this, the equilibrium concentration of NOCI will remain, essentially, at its initial concentration. Making this assumption, calculate the equilibrium concentration of NO. Note: use the ICE table from the previous problem to help you solve this problem. (Scientific notation can be entered using the following convention: 1.93 x 10-3 = 1.93E-3.) [NOleq= Tries 0/99 Submit Answer Post Discussion Send Feedback
Chemistry
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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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![section: CQB)
CHEM 102B/C Fall 2019
(Student
Messages Courses Help Logout
Lorcan James McGrath
Main Menu
Contents
Grades
Course Contents » ... » Homework 11 » Homework 11-4
Timer
Consider the following reaction for which K = 1.60 x 10-7 at some temperature:
2 NOCI (g)
2 NO (g) + Cl2(g)
In a given experiment, 0.845 moles of NOCI (g) were placed in an otherwise empty 1.51 L vessel. Complete the following table by entering numerical values in the Initial row and values containing the
variable "x" in the Change and Equilibrium rows. Define 2x as the amount (mol/L) of NOCI that reacts to reach equilibrium. Include signs in the Change column to indicate a gain or loss of concentration
(Omit units, use 3 sig.fig. and write concentrations less than 1 as 0.###, not as .# ##. If nothing is present initially, enter 0 for the molarity.)
[Cl2] (M)
[NOCI] (M)
[NO] (M)
Initial
Change
Equilibrium
Incorrect. Tries 3/99 Previous Tries
Submit Answer
Since K is very small, K = 1.60 x 10-7, very little product will be present at equilibrium, which tells us that very little NOCI will react to reach equilibrium. Because of this, the equilibrium concentration of
NOCI will remain, essentially, at its initial concentration. Making this assumption, calculate the equilibrium concentration of NO. Note: use the ICE table from the previous problem to help you solve
this problem. (Scientific notation can be entered using the following convention: 1.93 x 10-3 = 1.93E-3.)
[NOleq=
Tries 0/99
Submit Answer
Post Discussion
Send Feedback](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F0afecb3b-1c57-41b2-8bdb-98be9b732678%2F477e84b5-7bb3-4bf6-9fea-4897bebdbed8%2Fm61zai9.png&w=3840&q=75)
Transcribed Image Text:section: CQB)
CHEM 102B/C Fall 2019
(Student
Messages Courses Help Logout
Lorcan James McGrath
Main Menu
Contents
Grades
Course Contents » ... » Homework 11 » Homework 11-4
Timer
Consider the following reaction for which K = 1.60 x 10-7 at some temperature:
2 NOCI (g)
2 NO (g) + Cl2(g)
In a given experiment, 0.845 moles of NOCI (g) were placed in an otherwise empty 1.51 L vessel. Complete the following table by entering numerical values in the Initial row and values containing the
variable "x" in the Change and Equilibrium rows. Define 2x as the amount (mol/L) of NOCI that reacts to reach equilibrium. Include signs in the Change column to indicate a gain or loss of concentration
(Omit units, use 3 sig.fig. and write concentrations less than 1 as 0.###, not as .# ##. If nothing is present initially, enter 0 for the molarity.)
[Cl2] (M)
[NOCI] (M)
[NO] (M)
Initial
Change
Equilibrium
Incorrect. Tries 3/99 Previous Tries
Submit Answer
Since K is very small, K = 1.60 x 10-7, very little product will be present at equilibrium, which tells us that very little NOCI will react to reach equilibrium. Because of this, the equilibrium concentration of
NOCI will remain, essentially, at its initial concentration. Making this assumption, calculate the equilibrium concentration of NO. Note: use the ICE table from the previous problem to help you solve
this problem. (Scientific notation can be entered using the following convention: 1.93 x 10-3 = 1.93E-3.)
[NOleq=
Tries 0/99
Submit Answer
Post Discussion
Send Feedback
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