● Definition of equilibrium Keq: law of mass action Le Chatelier's Principle ● ● Topics: • Properties of acids & bases • Brønstead-Lowry Acids & Base: Kw & calculating [H3O+], [OH-], 1. If the reaction below is initially at equilibrium, and then each of the following changes are n which direction the reaction rate will be fastest until equilibrium is once again established: reverse, or no change. H2(g) + Cl2(g) 2 HCl(g) a. the concentration of H₂ is increased forward b. the concentration of HCI is decreased forward c. the concentration of Cl₂ is decreased reverse 2. If the reaction below is initially at equilibrium, and then more NH4 is added, predict which
● Definition of equilibrium Keq: law of mass action Le Chatelier's Principle ● ● Topics: • Properties of acids & bases • Brønstead-Lowry Acids & Base: Kw & calculating [H3O+], [OH-], 1. If the reaction below is initially at equilibrium, and then each of the following changes are n which direction the reaction rate will be fastest until equilibrium is once again established: reverse, or no change. H2(g) + Cl2(g) 2 HCl(g) a. the concentration of H₂ is increased forward b. the concentration of HCI is decreased forward c. the concentration of Cl₂ is decreased reverse 2. If the reaction below is initially at equilibrium, and then more NH4 is added, predict which
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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
Can you explain step by step with number 4 part A, number 4 part B, and number 4 part C? Can you explain it to me?
![● Definition of equilibrium
• Keq: law of mass action
●
Le Chatelier's Principle
Topics:
●
●
●
Properties of acids & bases
Brønstead-Lowry Acids & Bases definition
Kw & calculating [H3O+], [OH-], pH
1. If the reaction below is initially at equilibrium, and then each of the following changes are made, predict
which direction the reaction rate will be fastest until equilibrium is once again established: forward,
reverse, or no change.
H2(g) + Cl2(g) 2 HCl(g)
a. the concentration of H₂ is increased forward
b. the concentration of HCl is decreased forward
c. the concentration of Cl₂ is decreased versc
2. If the reaction below is initially at equilibrium, and then more NH4* is added, predict which direction the
reaction rate will be fastest until equilibrium is once again established: forward, reverse, or no
change. Forward
If more Hu is added
If more wHyt addel, forwa rol NH4* (aq) + H₂O (1) NH3 (aq) +
Hut reactant
reaction fast until equilibrium
reestablished
-1
[30+ (aq)
3. Define (a) reversible reaction and (b) equilibrium.
A) Reversible reaction is
produce original reactant,
one where the products of the reaction can themselves react to
B.) Equilibrium: Amount of reactant reach a balance istay there,
4. For the reaction below: reverse reaction take place exactly same rate in both direction
Reaction takes place in both direction but over all effect forward's
2 NO2 (g) + O2 (g) 2 NO3 (g)
a. Write the law of mass action (the equilibrium expression for Keq)
Keq = [03]
кед
[c]c[d] Products
Aja (B]b reactants
[0₂] [NO₂]²
b. If gas concentrations are as follows, 2.10 M NO2, 1.75 M O2, and 1.00 M NO3, calculate Keq
1.00m]
0.130x102
(1.00m)
0.1295
Keq=
(2.10m) ³x (675m) 0.130m²
(4.41m x1.75m) 0.130
c. Based on the Keq value that you calculated in part b, are the reactants or products predominant
(predominant means that there is a greater amount present)?
Keq is a less than 1, then equilibrium will shift to
reverse direction.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fb60ce3d5-7de7-48ff-b6dc-19fe3a1e14b8%2F3a1cc6f6-910e-438c-a12c-516ae17f74d6%2F9v83uhc_processed.jpeg&w=3840&q=75)
Transcribed Image Text:● Definition of equilibrium
• Keq: law of mass action
●
Le Chatelier's Principle
Topics:
●
●
●
Properties of acids & bases
Brønstead-Lowry Acids & Bases definition
Kw & calculating [H3O+], [OH-], pH
1. If the reaction below is initially at equilibrium, and then each of the following changes are made, predict
which direction the reaction rate will be fastest until equilibrium is once again established: forward,
reverse, or no change.
H2(g) + Cl2(g) 2 HCl(g)
a. the concentration of H₂ is increased forward
b. the concentration of HCl is decreased forward
c. the concentration of Cl₂ is decreased versc
2. If the reaction below is initially at equilibrium, and then more NH4* is added, predict which direction the
reaction rate will be fastest until equilibrium is once again established: forward, reverse, or no
change. Forward
If more Hu is added
If more wHyt addel, forwa rol NH4* (aq) + H₂O (1) NH3 (aq) +
Hut reactant
reaction fast until equilibrium
reestablished
-1
[30+ (aq)
3. Define (a) reversible reaction and (b) equilibrium.
A) Reversible reaction is
produce original reactant,
one where the products of the reaction can themselves react to
B.) Equilibrium: Amount of reactant reach a balance istay there,
4. For the reaction below: reverse reaction take place exactly same rate in both direction
Reaction takes place in both direction but over all effect forward's
2 NO2 (g) + O2 (g) 2 NO3 (g)
a. Write the law of mass action (the equilibrium expression for Keq)
Keq = [03]
кед
[c]c[d] Products
Aja (B]b reactants
[0₂] [NO₂]²
b. If gas concentrations are as follows, 2.10 M NO2, 1.75 M O2, and 1.00 M NO3, calculate Keq
1.00m]
0.130x102
(1.00m)
0.1295
Keq=
(2.10m) ³x (675m) 0.130m²
(4.41m x1.75m) 0.130
c. Based on the Keq value that you calculated in part b, are the reactants or products predominant
(predominant means that there is a greater amount present)?
Keq is a less than 1, then equilibrium will shift to
reverse direction.
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