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For the reaction, choose the CORRECT equilibrium constant, K_c.

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From the reaction, choose the CORRECT equilibrium constant, K_p.

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At elevated temperatures ammonium carbonate, NH₂COONH₄, is in equilibrium with NH₃ and CO₂ according to the equation;

NH₂COONH₄(s) ↔ 2 NH₃(g) + CO₂(g)

What is the equilibrium expression for this reaction?

• K = 2 [NH₃][CO₂]

  [NH₂COONH₄]

• K = [NH₃]²[CO₂]

  [NH₂COONH₄]

• K = 2 [NH₃][CO₂]

• K = [NH₃]²[CO₂]

What is the Kc expression for the reaction below:
SOCl2(g)  +  H2O(g)   ⇌    SO2(g)  +  2HCl(g)

What are [A] and [B]?

• concentration of reactants
• concentration of products
• energy of reactants
• energy of products

Which of the following is soluble in water?

• AgNO₃

• Ca₃(PO₄)₂

• Mg(OH)₂

• PbCl₂

The concentration of OH– in a saturated solution of Mg(OH)₂ is 3.6 x 10^–4 M. The Ksp of Mg(OH)₂ is

• 1.3 x 10^–7

• 4.7 x 10^–11

• 3.6 x 10^–4

• 2.3 x 10^–11

Sodium chloride is added slowly to a solution that is 0.010 M in Cu+, Ag+, and Au+. The Ksp values for the chloride salts are 1.9 x 10^-7, 1,6 x 10^-10, and 2.0 x 10^-13, respectively. Which compound will precipitate first?

• CuCl(s)

• AgCl(s)

• AuCl(s)

• All will precipitate at the same time.

How many moles of Ca(NO₃)₂ must be added to 1.0 L of a 0.100 M HF solution to begin precipitation of CaF₂ (s)? For CaF₂, Ksp = 4.0 x 10^–11.

• 5.8 x 10^–7

• 1.6 x 10^–9

• 7.0 x 10^–11

• 4.0 x 10^–9

If 30 mL of 5.0 x 10^-4 M Ca(NO₃)₂ are added to 70 mL of 2.0 x 10^-4 M NaF, will a precipitate occur? (Ksp of CaF₂ = 4.0 x 10^–11)

• No, because the ion product (Qsp) is greater than Ksp.

• Yes, because the ion product (Qsp) is less than Ksp.

• No, because the ion product (Qsp) is less than Ksp

• Yes, because the ion product is (Qsp) greater than Ksp.