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Exam 16: Principles of Reactivity: Chemical Equilibria

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Question 1

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The following reaction occurred when a 1.0-liter reaction vessel was initially charged with 2.0 moles of N₂(g) and 4.0 moles of H₂(g) : Once equilibrium was established,the concentration of NH₃(g) was determined to be 0.59 M at 700.°C.The value for K_c at 700.°C for the formation of ammonia is:

A) 3.5 $\times$ 10^-1
B) 6.8 $\times$ 10^-3
C) 1.1 $\times$ 10^-1
D) 6.6 $\times$ 10^-2
E) none of these

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B

Question 2

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Nitrogen and oxygen gases may react to form nitrogen monoxide. At 1500 ^$\circ$ C,K_c equals 1.0 $\times$ 10^-5.N₂(g) + O₂(g) 2 NO(g) If 0.030 mol N₂ and 0.030 mol O₂ are sealed in a 1.0 L flask at 1500 ^$\circ$ C,what is the concentration of NO(g) when equilibrium is established?

A) 3.0 $\times$ 10^-7 M
B) 4.7 $\times$ 10^-5 M
C) 9.5 $\times$ 10^-5 M
D) 3.0 $\times$ 10^-2 M
E) 9.1 $\times$ 10¹ M

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Question 3

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An aqueous mixture of phenol and ammonia has initial concentrations of 0.200 M C₆H₅OH(aq) and 0.120 M NH₃(aq) .At equilibrium,the C₆H₅O^-(aq) concentration is 0.050 M.Calculate K for the reaction. C₆H₅OH(aq) + NH₃(aq) C₆H₅O^- + NH₄⁺(aq)

At 700 K,K_p for the following equilibrium is 5.6 $\times$ 10^-3.2HgO(s) 2Hg(l) + O₂(g) Suppose 51.2 g of mercury(II) oxide is placed in a sealed 3.00-L vessel at 700 K.What is the partial pressure of oxygen gas at equilibrium? (R = 0.0821 L · atm/(K · mol) )

In which of the following reactions does a decrease in the volume of the reaction vessel at constant temperature favor formation of the products?

The equilibrium constant at 25 ^$\circ$ C for the dissolution of silver iodide is 8.5 $\times$ 10^-17.AgI(s) Ag⁺(aq) + I^-(aq) If an excess quantity of AgI(s) is added to water and allowed to equilibrate,what is the equilibrium concentration of I^-?

A 2.5 L flask is filled with 0.25 mol SO₃,0.20 mol SO₂,and 0.40 mol O₂,and allowed to reach equilibrium.Assume the temperature of the mixture is chosen so that K_c = 0.12.Predict the effect on the concentration of SO₃ as equilibrium is achieved by using Q,the reaction quotient. 2 SO₃(g) 2 SO₂(g) + O₂(g)

What balanced equation is the following equilibrium expression derived from?

Write a balanced chemical equation which corresponds to the following equilibrium constant expression.

For which of the following equilibria does K_c = K_p?

For the reaction N₂O₄(g) 2NO₂(g) ,K_p = 0.148 at a temperature of 298 K.What is K_p for the following reaction? 14NO₂(g) 7N₂O₄(g)

Consider the following equilibrium: PCl₅(g) PCl₃(g) + Cl₂(g) ; $~~~~~~~~$ $\Delta$ H = 92 kJ The concentration of PCl₃ at equilibrium may be increased by

A 10.0-g sample of solid NH₄Cl is heated in a 5.00-L container to 900.°C.At equilibrium the pressure of NH₃(g) is 1.47 atm. NH₄Cl(s) NH₃(g) + HCl(g) The equilibrium constant,K_p,for the reaction is:

At a high temperature,equal concentrations of 0.160 mol/L of H₂(g) and I₂(g) are initially present in a flask.The H₂ and I₂ react according to the balanced equation below. When equilibrium is reached,the concentration of H₂(g) has decreased to 0.036 mol/L.What is the equilibrium constant,K_c,for the reaction?

When 1.0 mole of acetic acid is diluted with water to a volume of 1.0 L at 25 ^$\circ$ C,0.42% of the acetic acid ionizes to form acetate ion and hydronium ion.CH₃CO₂H(aq)+ H₂O( ) CH₃CO₂^-(aq)+ H₃O⁺(aq) What percentage of the acid ionizes when 0.75 mole of acetic acid is diluted with water to 1.0 L at 25 ^$\circ$ C?

Given the following chemical equilibria, N₂(g) + O₂(g) 2 NO(g) $~~~~~~~~$ $~~~~~~~~$ K₁ N₂(g) + 3 H₂(g) 2 NH₃(g) $~~~~~~~~$ $~~ ~~~$ K₂ H₂(g) + 1/2 O₂(g) H₂O(g) $~~~~~~~~$ $~~~~ ~$ K₃ Determine the method used to calculate the equilibrium constant for the reaction below. 4 NH₃(g) + 5 O₂(g) 4 NO(g) + 6 H₂O(g) $~~~~~~~~$ K _c

What is the K_c equilibrium-constant expression for the following equilibrium?

Given the following equilibria, PbBr₂(s) Pb²⁺(aq) + 2 Br^-(aq) $~~~~~~~~$ $~~~~~~~~~~~~$ K₁ = 6.6 $\times$ 0 10^-6 Pb(OH) ₂(s) Pb²⁺(aq) + 2 OH^-(aq) $~~~~~~~~$ $~~~~~~~~$ K₂ = 1.4 $\times$ 10^-15 Determine the equilibrium constant,K_c,for the following reaction. PbBr₂(s) + 2 OH^-(aq) Pb(OH) ₂(s) + 2 Br^-(aq)

When 0.20 mole HF is dissolved in water to a volume of 1.00 L,5.8% of the HF dissociates to form F^-(aq) .What is the equilibrium constant for the reaction?

Nitrogen trifluoride decomposes at to form nitrogen and fluorine gases according to the following equation: 6.00-L reaction vessel is initially charged with 1.96 mol of NF₃ and allowed to come to equilibrium at 800 K.Once equilibrium is established,the reaction vessel is found to contain 0.0380 mol of N₂.What is the value of K_p at this temperature? (R = 0.0821 L.atm.mol.K)