DATA: CALCULATIONS: Because the potassium nitrate is a strong electrolyte, its solution reaction will be: KNO3(s) + H2O →K+ (aq) + NOз - (aq) The reaction is at equilibrium when the solid is in contact with a saturated solution, the condition we have when crystallization begins. The solubility, s, of the salt in moles per liter may be calculated from the amount of salt weighed out and the volume of the solution. The equilibrium constant, K, for the reaction will be: Ksp = [K][NO3] = (s)(s) = s² (1) The equilibrium constant Ksp may be used to calculate the AG for the reaction at each temperature using the thermodynamic relationship: AG = -RT In K (2) where T is the Kelvin temperature and R is the gas constant (8.314 J/mol-K). AGAHTAS (3) These two variables, AH and TAS, can be substituted for AG into Equation 3. With some rearrangement the mathematical relationship between Ksp, AH, and AS as a function of T is given in a useful form for graphing in Equation 5 below. The equation is written in In Ksp--AH/R*(1/T) + AS/R y = mx + b the form of a straight line, y = mx + b as shown above. The form of a straight line, y = mx + b as shown above. We may assume that AH and AS are constant over these small temperature ranges. The last equation relates the overall change in Gibbs free energy, AG, to the changes in Ksp as given in Equation 3. It also allows for the other two thermodynamic variables to be estimated. In this experiment you will obtain the thermodynamic values AG, AH, and AS, associated with the solubility of KNO3 One final note: Adding moderately large amounts of solids to moderately small amounts of water has a large effect on the final volume of the solution. When saturated solutions are prepared the volume of the resulting solution must be determined experimentally. Use The Excel Worksheet to do the calculations. 1. Using equation 1, calculate the K for each temperature, and 2. Using equation 2, calculate AG for each temperature. The variation of K with temperature is such that if a plot of In K (on the y axis) vs. 1/T is made, the result is a straight line with the slope -AH/R. 3. Using Excel construct a graph of In K vs 1/T and measure the slope of the line, and determine the value of AH for the reaction. At this point, K and AG for each temperature 2 Thermodynamics Mass of KNO3 20 g Moles of KNO3 0.1978 moles Total Volume Temperature Temperature (mL) °C K Molarity (Molarity)2 Trial 1 25.0 69.9 343.0 7.9 62.6 Trial 2 29.0 58.4 331.6 6.8 46.5 Trial 3 33.0 49.1 322.2 6.0 35.9 Trial 4 38.0 40.6 313.8 5.2 27.1 Trial 5 43.0 33.5 306.6 4.6 21.2 In Ksp 1/K AG Trial 1 4.1 0.00292 -12 Trial 2 3.8 0.00302 -11 Trial 3 3.6 0.00310 -10 Trial 4 3.3 0.00319 -9 Trial 5 3.1 0.00326 -8 Slope -14380 In Ksp vs 1/T AH (kJ/mole) 119.6 kJ/mole 4.5 4.0 y=-14380x + 48.044 R² = 0.9334 Intercept 48.0 3.5 AS (J/K Mole) 399 J/K mole 3.0 2.5 2.0 1.5. 1.0 0.5 0.0 0.00285 0.00290 0.00295 0.00300 0.00305 0.00310 0.00315 0.00320 0.00325 0.00330
DATA: CALCULATIONS: Because the potassium nitrate is a strong electrolyte, its solution reaction will be: KNO3(s) + H2O →K+ (aq) + NOз - (aq) The reaction is at equilibrium when the solid is in contact with a saturated solution, the condition we have when crystallization begins. The solubility, s, of the salt in moles per liter may be calculated from the amount of salt weighed out and the volume of the solution. The equilibrium constant, K, for the reaction will be: Ksp = [K][NO3] = (s)(s) = s² (1) The equilibrium constant Ksp may be used to calculate the AG for the reaction at each temperature using the thermodynamic relationship: AG = -RT In K (2) where T is the Kelvin temperature and R is the gas constant (8.314 J/mol-K). AGAHTAS (3) These two variables, AH and TAS, can be substituted for AG into Equation 3. With some rearrangement the mathematical relationship between Ksp, AH, and AS as a function of T is given in a useful form for graphing in Equation 5 below. The equation is written in In Ksp--AH/R*(1/T) + AS/R y = mx + b the form of a straight line, y = mx + b as shown above. The form of a straight line, y = mx + b as shown above. We may assume that AH and AS are constant over these small temperature ranges. The last equation relates the overall change in Gibbs free energy, AG, to the changes in Ksp as given in Equation 3. It also allows for the other two thermodynamic variables to be estimated. In this experiment you will obtain the thermodynamic values AG, AH, and AS, associated with the solubility of KNO3 One final note: Adding moderately large amounts of solids to moderately small amounts of water has a large effect on the final volume of the solution. When saturated solutions are prepared the volume of the resulting solution must be determined experimentally. Use The Excel Worksheet to do the calculations. 1. Using equation 1, calculate the K for each temperature, and 2. Using equation 2, calculate AG for each temperature. The variation of K with temperature is such that if a plot of In K (on the y axis) vs. 1/T is made, the result is a straight line with the slope -AH/R. 3. Using Excel construct a graph of In K vs 1/T and measure the slope of the line, and determine the value of AH for the reaction. At this point, K and AG for each temperature 2 Thermodynamics Mass of KNO3 20 g Moles of KNO3 0.1978 moles Total Volume Temperature Temperature (mL) °C K Molarity (Molarity)2 Trial 1 25.0 69.9 343.0 7.9 62.6 Trial 2 29.0 58.4 331.6 6.8 46.5 Trial 3 33.0 49.1 322.2 6.0 35.9 Trial 4 38.0 40.6 313.8 5.2 27.1 Trial 5 43.0 33.5 306.6 4.6 21.2 In Ksp 1/K AG Trial 1 4.1 0.00292 -12 Trial 2 3.8 0.00302 -11 Trial 3 3.6 0.00310 -10 Trial 4 3.3 0.00319 -9 Trial 5 3.1 0.00326 -8 Slope -14380 In Ksp vs 1/T AH (kJ/mole) 119.6 kJ/mole 4.5 4.0 y=-14380x + 48.044 R² = 0.9334 Intercept 48.0 3.5 AS (J/K Mole) 399 J/K mole 3.0 2.5 2.0 1.5. 1.0 0.5 0.0 0.00285 0.00290 0.00295 0.00300 0.00305 0.00310 0.00315 0.00320 0.00325 0.00330
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...
Related questions
Question
HELP!
Lab
1.Using equation 1, calculate the K for each temperature, and
2. Using equation 2, calculate AG for each temperature. The variation of K with temperature
is such that if a plot of In K (on the y axis) vs. 1/T is made, the result is a straight line with
the slope -AH/R.
3. Using Excel construct a graph of In K vs 1/T and measure the slope of the line, and
determine the value of AH for the reaction. At this point, K and AG for each temperature
![DATA: CALCULATIONS: Because the potassium nitrate is a strong electrolyte, its solution
reaction will be:
KNO3(s) + H2O →K+ (aq) + NOз - (aq)
The reaction is at equilibrium when the solid is in contact with a saturated solution, the condition
we have when crystallization begins. The solubility, s, of the salt in moles per liter may be
calculated from the amount of salt weighed out and the volume of the solution. The equilibrium
constant, K, for the reaction will be:
Ksp = [K][NO3] = (s)(s) = s²
(1)
The equilibrium constant Ksp may be used to calculate the AG for the reaction at each
temperature using the thermodynamic relationship:
AG = -RT In K
(2)
where T is the Kelvin temperature and R is the gas constant (8.314 J/mol-K).
AGAHTAS
(3)
These two variables, AH and TAS, can be substituted for AG into Equation 3. With some
rearrangement the mathematical relationship between Ksp, AH, and AS as a function of T is
given in a useful form for graphing in Equation 5 below. The equation is written in
In Ksp--AH/R*(1/T) + AS/R
y
= mx
+
b
the form of a straight line, y = mx + b as shown above. The form of a straight line, y = mx + b as
shown above. We may assume that AH and AS are constant over these small temperature
ranges. The last equation relates the overall change in Gibbs free energy, AG, to the changes
in Ksp as given in Equation 3. It also allows for the other two thermodynamic variables to be
estimated. In this experiment you will obtain the thermodynamic values AG, AH, and AS,
associated with the solubility of KNO3
One final note: Adding moderately large amounts of solids to moderately small amounts of water
has a large effect on the final volume of the solution. When saturated solutions are prepared the
volume of the resulting solution must be determined experimentally. Use The Excel Worksheet
to do the calculations.
1. Using equation 1, calculate the K for each temperature, and
2. Using equation 2, calculate AG for each temperature. The variation of K with temperature
is such that if a plot of In K (on the y axis) vs. 1/T is made, the result is a straight line with
the slope -AH/R.
3. Using Excel construct a graph of In K vs 1/T and measure the slope of the line, and
determine the value of AH for the reaction. At this point, K and AG for each temperature
2](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F765b863c-0883-4071-8f0f-832646f981bf%2F7a6345ea-d9e7-483f-a306-9883c2ae3e6a%2Fi3j15rl_processed.jpeg&w=3840&q=75)
Transcribed Image Text:DATA: CALCULATIONS: Because the potassium nitrate is a strong electrolyte, its solution
reaction will be:
KNO3(s) + H2O →K+ (aq) + NOз - (aq)
The reaction is at equilibrium when the solid is in contact with a saturated solution, the condition
we have when crystallization begins. The solubility, s, of the salt in moles per liter may be
calculated from the amount of salt weighed out and the volume of the solution. The equilibrium
constant, K, for the reaction will be:
Ksp = [K][NO3] = (s)(s) = s²
(1)
The equilibrium constant Ksp may be used to calculate the AG for the reaction at each
temperature using the thermodynamic relationship:
AG = -RT In K
(2)
where T is the Kelvin temperature and R is the gas constant (8.314 J/mol-K).
AGAHTAS
(3)
These two variables, AH and TAS, can be substituted for AG into Equation 3. With some
rearrangement the mathematical relationship between Ksp, AH, and AS as a function of T is
given in a useful form for graphing in Equation 5 below. The equation is written in
In Ksp--AH/R*(1/T) + AS/R
y
= mx
+
b
the form of a straight line, y = mx + b as shown above. The form of a straight line, y = mx + b as
shown above. We may assume that AH and AS are constant over these small temperature
ranges. The last equation relates the overall change in Gibbs free energy, AG, to the changes
in Ksp as given in Equation 3. It also allows for the other two thermodynamic variables to be
estimated. In this experiment you will obtain the thermodynamic values AG, AH, and AS,
associated with the solubility of KNO3
One final note: Adding moderately large amounts of solids to moderately small amounts of water
has a large effect on the final volume of the solution. When saturated solutions are prepared the
volume of the resulting solution must be determined experimentally. Use The Excel Worksheet
to do the calculations.
1. Using equation 1, calculate the K for each temperature, and
2. Using equation 2, calculate AG for each temperature. The variation of K with temperature
is such that if a plot of In K (on the y axis) vs. 1/T is made, the result is a straight line with
the slope -AH/R.
3. Using Excel construct a graph of In K vs 1/T and measure the slope of the line, and
determine the value of AH for the reaction. At this point, K and AG for each temperature
2

Transcribed Image Text:Thermodynamics
Mass of KNO3
20
g
Moles of KNO3
0.1978 moles
Total Volume Temperature Temperature
(mL)
°C
K
Molarity (Molarity)2
Trial 1
25.0
69.9
343.0
7.9
62.6
Trial 2
29.0
58.4
331.6
6.8
46.5
Trial 3
33.0
49.1
322.2
6.0
35.9
Trial 4
38.0
40.6
313.8
5.2
27.1
Trial 5
43.0
33.5
306.6
4.6
21.2
In Ksp
1/K
AG
Trial 1
4.1
0.00292
-12
Trial 2
3.8
0.00302
-11
Trial 3
3.6
0.00310
-10
Trial 4
3.3
0.00319
-9
Trial 5
3.1
0.00326
-8
Slope
-14380
In Ksp vs 1/T
AH (kJ/mole)
119.6
kJ/mole
4.5
4.0
y=-14380x + 48.044
R² = 0.9334
Intercept
48.0
3.5
AS (J/K Mole)
399
J/K mole
3.0
2.5
2.0
1.5.
1.0
0.5
0.0
0.00285 0.00290 0.00295 0.00300 0.00305 0.00310
0.00315
0.00320 0.00325 0.00330
Expert Solution

This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
This is a popular solution!
Trending now
This is a popular solution!
Step by step
Solved in 2 steps

Recommended textbooks for you

Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning

Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education

Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning

Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning

Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education

Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning

Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education

Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning

Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY