AP CHEM Unit 2 Day 4

For a reaction at equilibrium, which of the following is the best way to think about it? 

• The concentration of reactants and products are not related. 
• concentration of reactants = concentration of products 
• forward rate = reverse rate
  
• The concentration of reactants becomes negligible. 

Pure liquids or solids do NOT appear in the equilibrium constant expression. 

• True
• False
• Don't choose me. 
• Don't choose me. 

Consider the chemical equation shown. 
What would Keq be for this reaction? 

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What is the equilibrium expression for the following equation?  Assume that all species here are gases. 

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Consider the reaction shown.  What is the form of the equilibrium constant, Kc, for the reaction? 

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What is the form of the equilibrium constant for the process shown? 

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Tags

NGSS.HS-PS1-7

Write the reaction quotient for

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Which of the following is TRUE? 

• A small value of K means that the equilibrium concentrations of the reactants are small compared to the equilibrium concentrations of the products.
• When the value of Q is large, the equilibrium lies on the product side of the equilibrium reaction
• A large value of K means that the equilibrium concentrations of products are large compared to the equilibrium concentrations of the reactants. 
• When the value of K is large, the equilibrium lies on the reactant side of the equilibrium reaction.

Consider the reaction shown:
If K is 10⁸⁰ which of the following is a good estimate of equilibrium concentrations of H₂, O₂ and H₂O, respectively?

• 10 M, 5 M and 10 M, respectively
• 5 M, 0 M and 10 M, respectively
• 0 M, 0 M and 5 M, respectively
• 10 M, 5 M and 0 M, respectively

Tags

NGSS.HS-PS1-7

The equilibrium constant for the reaction shown is 4.3 × 10⁻⁴ at 25^◦ C. Will nitrous acid spontaneously dissociate (will the forward reaction occur) when

[HNO₂(aq)] = 0.10 M

[NO₂⁻ (aq)] = [H₃O⁺(aq)] = 1.0 × 10⁻² M?

• No

• Yes

• Cannot be determined

• #chemISlyfe

Tags

NGSS.HS-PS1-5

NGSS.HS-PS1-7