Homework Help is Here – Start Your Trial Now!
Science
Chemistry
Consider the reaction: NH2COONH4 (s) = 2 NH3 (g) + CO2 (g) At high temperatures such as 250.°C, the equilibrium constant for the reaction is 1.58 x 10-8. A research student ran the experiment by first placing 39.1 g of the reactant compound in a 750. mL evacuated closed container. (R = 0.08206 L.atm/K.mol; K = °C + 273; pay attention to sig figs) a) Write the equilibrium expression, Kc, for this reaction. kc=l.58 x 10 COONH kc [NH3]? [COz] b) What is the concentration of each of the products at equilibrium? NH2COONH4 (s) = 2 NH3 (g) + CO2 (g) NHz COON H4: 39.1g 78.070 gimol 50 mol NH2 COON Hy = Z NH3 CO2 Tnitial -50 gimo1 W 999. + 2 X t ズ ミGGG N •150L E : 666-X answer: ENHS] = 2(-89x104) :1.78x10-4 M C COz] = -89x 10 4 M kc CNH3]?CCO1] →1.58* 10°8-(2x) Cx) 2x2.1.58x 1 X: 1.58x108 c) What is the pressure in atm exerted by each of the products at equilibrium? on 79x 10 こ、 kp= kc x (RT) X= .89x104 R=. 08206 kp:1.58x10-8 x(.08206x523)? :1,58 x 108x (42.91738)? : 2.9|x 10-5 n (3-1) = 2 入 T 523 k -5 [NH3]=2(,0302) = . O605 altm X= .0302 COL): 10302 atm d) Use these pressures to calculate the Kp for the reaction at this temperature. d) Use these pressures to calculate the K, for the reaction at this temperature. e) What is the total pressure in the container at equilibrium. f) If the reaction was initially set up with 95.5 g of the reactant instead of the 39.1 g, and all other conditions were the same , what are the concentrations of each of the products at equilibrium?

Consider the reaction: NH2COONH4 (s) = 2 NH3 (g) + CO2 (g) At high temperatures such as 250.°C, the equilibrium constant for the reaction is 1.58 x 10-8. A research student ran the experiment by first placing 39.1 g of the reactant compound in a 750. mL evacuated closed container. (R = 0.08206 L.atm/K.mol; K = °C + 273; pay attention to sig figs) a) Write the equilibrium expression, Kc, for this reaction. kc=l.58 x 10 COONH kc [NH3]? [COz] b) What is the concentration of each of the products at equilibrium? NH2COONH4 (s) = 2 NH3 (g) + CO2 (g) NHz COON H4: 39.1g 78.070 gimol 50 mol NH2 COON Hy = Z NH3 CO2 Tnitial -50 gimo1 W 999. + 2 X t ズ ミGGG N •150L E : 666-X answer: ENHS] = 2(-89x104) :1.78x10-4 M C COz] = -89x 10 4 M kc CNH3]?CCO1] →1.58* 10°8-(2x) Cx) 2x2.1.58x 1 X: 1.58x108 c) What is the pressure in atm exerted by each of the products at equilibrium? on 79x 10 こ、 kp= kc x (RT) X= .89x104 R=. 08206 kp:1.58x10-8 x(.08206x523)? :1,58 x 108x (42.91738)? : 2.9|x 10-5 n (3-1) = 2 入 T 523 k -5 [NH3]=2(,0302) = . O605 altm X= .0302 COL): 10302 atm d) Use these pressures to calculate the Kp for the reaction at this temperature. d) Use these pressures to calculate the K, for the reaction at this temperature. e) What is the total pressure in the container at equilibrium. f) If the reaction was initially set up with 95.5 g of the reactant instead of the 39.1 g, and all other conditions were the same , what are the concentrations of each of the products at equilibrium?

Chemistry: The Molecular Science
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter12: Chemical Equilibrium
Section: Chapter Questions
Problem 61QRT
See similar textbooks
icon
Related questions
Question

I need help with parts d, e, and f, please

 

 

Consider the reaction: NH2COONH4 (s) = 2 NH3 (g) + CO2 (g) At high temperatures such as 250.°C, the equilibrium constant for the reaction is 1.58 x 10-8. A research student ran the experiment by first placing 39.1 g of the reactant compound in a 750. mL evacuated closed container. (R = 0.08206 L.atm/K.mol; K = °C + 273; pay attention to sig figs) a) Write the equilibrium expression, Kc, for this reaction. kc=l.58 x 10 COONH kc [NH3]? [COz] b) What is the concentration of each of the products at equilibrium? NH2COONH4 (s) = 2 NH3 (g) + CO2 (g) NHz COON H4: 39.1g 78.070 gimol 50 mol NH2 COON Hy = Z NH3 CO2 Tnitial -50 gimo1 W 999. + 2 X t ズ ミGGG N •150L E : 666-X answer: ENHS] = 2(-89x104) :1.78x10-4 M C COz] = -89x 10 4 M kc CNH3]?CCO1] →1.58* 10°8-(2x) Cx) 2x2.1.58x 1 X: 1.58x108 c) What is the pressure in atm exerted by each of the products at equilibrium? on 79x 10 こ、 kp= kc x (RT) X= .89x104 R=. 08206 kp:1.58x10-8 x(.08206x523)? :1,58 x 108x (42.91738)? : 2.9|x 10-5 n (3-1) = 2 入 T 523 k -5 [NH3]=2(,0302) = . O605 altm X= .0302 COL): 10302 atm d) Use these pressures to calculate the Kp for the reaction at this temperature.
Transcribed Image Text:Consider the reaction: NH2COONH4 (s) = 2 NH3 (g) + CO2 (g) At high temperatures such as 250.°C, the equilibrium constant for the reaction is 1.58 x 10-8. A research student ran the experiment by first placing 39.1 g of the reactant compound in a 750. mL evacuated closed container. (R = 0.08206 L.atm/K.mol; K = °C + 273; pay attention to sig figs) a) Write the equilibrium expression, Kc, for this reaction. kc=l.58 x 10 COONH kc [NH3]? [COz] b) What is the concentration of each of the products at equilibrium? NH2COONH4 (s) = 2 NH3 (g) + CO2 (g) NHz COON H4: 39.1g 78.070 gimol 50 mol NH2 COON Hy = Z NH3 CO2 Tnitial -50 gimo1 W 999. + 2 X t ズ ミGGG N •150L E : 666-X answer: ENHS] = 2(-89x104) :1.78x10-4 M C COz] = -89x 10 4 M kc CNH3]?CCO1] →1.58* 10°8-(2x) Cx) 2x2.1.58x 1 X: 1.58x108 c) What is the pressure in atm exerted by each of the products at equilibrium? on 79x 10 こ、 kp= kc x (RT) X= .89x104 R=. 08206 kp:1.58x10-8 x(.08206x523)? :1,58 x 108x (42.91738)? : 2.9|x 10-5 n (3-1) = 2 入 T 523 k -5 [NH3]=2(,0302) = . O605 altm X= .0302 COL): 10302 atm d) Use these pressures to calculate the Kp for the reaction at this temperature.
d) Use these pressures to calculate the K, for the reaction at this temperature. e) What is the total pressure in the container at equilibrium. f) If the reaction was initially set up with 95.5 g of the reactant instead of the 39.1 g, and all other conditions were the same , what are the concentrations of each of the products at equilibrium?
Transcribed Image Text:d) Use these pressures to calculate the K, for the reaction at this temperature. e) What is the total pressure in the container at equilibrium. f) If the reaction was initially set up with 95.5 g of the reactant instead of the 39.1 g, and all other conditions were the same , what are the concentrations of each of the products at equilibrium?
Expert Solution
trending now

Trending now

This is a popular solution!

steps

Step by step

Solved in 6 steps

SEE SOLUTIONCheck out a sample Q&A here
Blurred answer
Knowledge Booster
Tools in Analytical Chemistry
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.
Similar questions
Recommended textbooks for you
Chemistry: The Molecular Science
Chemistry: The Molecular Science
Chemistry
ISBN:
9781285199047
Author:
John W. Moore, Conrad L. Stanitski
Publisher:
Cengage Learning
Chemistry
Chemistry
Chemistry
ISBN:
9781133611097
Author:
Steven S. Zumdahl
Publisher:
Cengage Learning
Chemistry
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry: An Atoms First Approach
Chemistry: An Atoms First Approach
Chemistry
ISBN:
9781305079243
Author:
Steven S. Zumdahl, Susan A. Zumdahl
Publisher:
Cengage Learning
Chemistry for Engineering Students
Chemistry for Engineering Students
Chemistry
ISBN:
9781337398909
Author:
Lawrence S. Brown, Tom Holme
Publisher:
Cengage Learning
Introductory Chemistry: A Foundation
Introductory Chemistry: A Foundation
Chemistry
ISBN:
9781285199030
Author:
Steven S. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
SEE MORE TEXTBOOKS