Gen Chem 3 Values and Their Meanings Flashcards
K is 25. What does that tell you about the reaction?
The reaction FAVORS PRODUCTS.
If it was at equilibrium, there would be more products than reactants.
K is 8.27 x 10^12. What does that tell you about the reaction?
The reaction FAVORS PRODUCTS.
If it was at equilibrium, there would be more products than reactants.
K is 0.491 What does that tell you about the reaction?
The reaction FAVORS REACTANTS
If it was at equilibrium, there would be more reactants than products
K is 2.69 x 10 ^ -5 What does that tell you about the reaction?
The reaction FAVORS REACTANTS
If it was at equilibrium, there would be more reactants than products
You calculate that K is -58.4 What does that tell you about the reaction?
Trick question. It tells you that you don’t understand chemistry, because K cannot be negative!
K is a ratio of product amounts over reactant amounts, and you can’t have a negative amount of a chemical!
Q is 300 What does that tell you about the reaction?
Not much. All it says is that you have a lot more products present now than reactants.
But you can’t figure out which way the reaction will shift b/c you don’t know K.
Q is 0.1111 What does that tell you about the reaction?
Not much. All it says is that you have more reactants than products present right now.
But you can’t figure out which way the reaction will shift b/c you don’t know K
Q = 750 and K = 200 What can you say about the reaction?
Because K is bigger than 1, the reaction generally FAVORS PRODUCTS.
But because Q is bigger than K, it must SHIFT TO FORM REACTANTS in order to reach equilibrium.
Q = 5267 and K = 9000 What can you say about the reaction?
Because K is bigger than 1, the reaction generally FAVORS PRODUCTS.
Because Q is smaller than K, it must SHIFT TO FORM PRODUCTS in order to reach equilibrium.
Q = 0.00543 and K = 0.0654 What can you say about the reaction?
Because K is less than 1, the reaction generally FAVORS REACTANTS
But because Q is smaller than K, it must SHIFT TO FORM PRODUCTS in order to reach equilibrium.
Q = 650 and K = 8.33 x 10^ -5 What can you say about the reaction?
Because K is less than 1, the reaction generally FAVORS REACTANTS
Because Q is bigger than K, it must SHIFT TO FORM REACTANTS in order to reach equilibrium.
Q = 27.6 and K = 27.6 What can you say about the reaction?
Because K is bigger than 1, the reaction generally FAVORS PRODUCTS.
Because Q = K, the reaction is currently AT EQUILIBRIUM
ΔG = 85.0 kJ/mol What can you say about the reaction?
Because ΔG is positive, given the current conditions, the reaction must SHIFT to form REACTANTS in order to reach equilibrium.
ΔG = 0.250 kJ/mol What can you say about the reaction?
Because ΔG is positive, given the current conditions, the reaction must SHIFT to form REACTANTS in order to reach equilibrium.
ΔG-standard = 155 kJ/mol. What can you say about the reaction?
Because ΔG-standard is positive, the reaction generally FAVORS REACTANTS. If it ever reaches equilibrium, there will be more reactants present than products.
ΔG-standard = 0.617 kJ/mol What can you say about the reaction?
Because ΔG-standard is positive, the reaction generally FAVORS REACTANTS. If it ever reaches equilibrium, there will be more reactants present than products.
ΔG = - 376 kJ/mol What can you say about the reaction?
Because ΔG is negative, given the current conditions, the reaction must SHIFT to form PRODUCTS in order to reach equilibrium.
ΔG = - 0.444 kJ/mol What can you say about the reaction?
Because ΔG is negative, given the current conditions, the reaction must SHIFT to form PRODUCTS in order to reach equilibrium.
ΔG-standard = -500 kJ/mol. What can you say about the reaction?
Because ΔG-standard is negative, the reaction generally FAVORS PRODUCTS. If it ever reaches equilibrium, there will be more reactants present than products.
ΔG-standard = -0.246 kJ/mol What can you say about the reaction?
Because ΔG-standard is negative, the reaction generally FAVORS PRODUCTS. If it ever reaches equilibrium, there will be more reactants present than products.
ΔG = 0 kJ/mol What can you say about the reaction?
It is at equilibrium.
ΔG-standard = 0 kJ/mol. What can you say about the reaction?
If it ever reached equilibrium, it would have equal amounts of reactants and products. It does not FAVOR either one.
E = 5.25 V What can you say about the reaction?
Because E is positive, given the current conditions, the reaction will SHIFT to form PRODUCTS.
E = 0.355 V What can you say about the reaction?
Because E is positive, given the current conditions, the reaction will SHIFT to form PRODUCTS.
E = -1.77 V What can you say about the reaction?
Because E is negative, given the current conditions, the reaction will SHIFT to form REACTANTS.
E = -3.18 V What can you say about the reaction?
Because E is negative, given the current conditions, the reaction will SHIFT to form REACTANTS.
E-standard = 4.81 V What can you say about the reaction?
Because E-Standard is positive, the reaction generally FAVORS PRODUCTS.
E-standard = 0.813 V What can you say about the reaction?
Because E-Standard is positive, the reaction generally FAVORS PRODUCTS.
E-standard = -2.81 V. What can you say about the reaction?
Because E-Standard is negative, the reaction generally FAVORS REACTANTS.
E-standard = -0.194 V What can you say about the reaction?
Because E-Standard is negative, the reaction generally FAVORS REACTANTS.
E = 0 V. What can you say about the reaction?
The reaction is at equilibrium.
E-standard = 0 V What can you say about the reacftion?
If the reaction ever reached equilibrium, it would have equal amounts of reactants and products. Neither one is FAVORED.
What sort of values can K be?
Any positive number.
What sort of values can Q be?
Zero or any positive number.
What sort of values can ΔG be?
ΔG can be any real number.
( Just so you have a reference for “does my answer make sense”, I typically write problems where it is between -2500 kJ/mol and 2500 kJ/mol, but there’s no real limit in either direction. )
What sort of values can ΔG-standard be?
ΔG-standard can be any real number.
( Just so you have a reference for “does my answer make sense”, I typically write problems where it is between -2500 kJ/mol and 2500 kJ/mol, but there’s no real limit in either direction. )
What sort of voltages can E be?
E can be ANY real number.
(To get large magnitudes of E, you need to connect together multiple electrochemical cells, but they ARE certainly possible. In the questions I write, E is typically between -4.00 V and 4.00 V but those are not real cutoffs. )
What sort of voltages can E-standard be?
E-standard can be ANY real number.
(To get large magnitudes of E-standard, you need to connect together multiple electrochemical cells, but they ARE certainly possible. In the questions I write, E is typically between -4.00 V and 4.00 V but those are not real cutoffs. )
What thing(s) should you compare K to?
K should be compared to 1 to figure out what is FAVORED
K should be compared to Q to figure out which way it will SHIFT
What thing(s) should you compare Q to?
You should compare Q to K to figure out which way the reaction SHIFTS
What thing(s) should you compare ΔG to?
You should compare ΔG to zero to figure out which way the reaction will SHIFT.
What thing(s) should you compare ΔG-standard to?
You should compare ΔG-standard to zero to figure out what the reaction FAVORS.
What thing(s) should you compare E to?
You should compare E to zero to figure out which way the reaction will SHIFT.
What thing(s) should you compare E-standard to?
You should compare E-standard to zero to figure out what the reaction FAVORS.
What values can pH be?
pH can be any number. It’s USUALLY between -1 and 15, but those aren’t hard cutoffs.
What values can pOH be?
pOH can be any number. It’s USUALLY between -1 and 15, but those aren’t hard cutoffs.
