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 Kc 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 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 B

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) decreasing the temperature. B) adding Cl2 to the system. C) adding PCl5 to the system. D) increasing the pressure. E) adding a catalyst. A) decreasing the temperature. B) adding Cl2 to the system. C) adding PCl5 to the system. D) increasing the pressure. E) adding a catalyst.

When 1.0 mole of acetic acid is diluted with water to a volume of 1.0 L at 25 S1U1P1$\circ$S1S1P0C,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 S1U1P1$\circ$S1S1P0C?

The answer of When 1.0 mole of acetic acid is...

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 Kp at this temperature? (R = 0.0821 L.atm.mol.K)

A) 1.53 $\times$ 10-5 B) 1.91 $\times$ 10-3 C) 1.76 $\times$ 10-3 D) 1.59 $\times$ 10-5 E) 4.43 $\times$ 10-7 A) 1.53 $\times$ 10-5 B) 1.91 $\times$ 10-3 C) 1.76 $\times$ 10-3 D) 1.59 $\times$ 10-5 E) 4.43 $\times$ 10-7

Nitrogen and oxygen gases may react to form nitrogen monoxide. At 1500 S1U1P1$\circ$S1S1P0C,Kc equals 1.0 $\times$10-5.N2(g)+ O2(g) 2 NO(g) If 0.030 mol N2 and 0.030 mol O2 are sealed in a 1.0 L flask at 1500 S1U1P1$\circ$S1S1P0C,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 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

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,Kp,for the reaction is:

A) 2.16 B) 7.78 C) 1.47 D) 2.94 E) none of these A) 2.16 B) 7.78 C) 1.47 D) 2.94 E) none of these

The equilibrium constant at 25 S1U1P1$\circ$S1S1P0C 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) 7.2 $\times$ 10-33 M B) 4.3 $\times$ 10-17 M C) 8.5 $\times$ 10-17 M D) 6.5 $\times$ 10-9 M E) 9.2 $\times$ 10-9 M A) 7.2 $\times$ 10-33 M B) 4.3 $\times$ 10-17 M C) 8.5 $\times$ 10-17 M D) 6.5 $\times$ 10-9 M E) 9.2 $\times$ 10-9 M

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,Kc,for the following reaction. PbBr2(s)+ 2 OH-(aq) Pb(OH)2(s)+ 2 Br-(aq)

A) 9.2 $\times$ 10-21 B) 2.1 $\times$ 10-10 C) 6.6 $\times$ 10-6 D) 4.7 $\times$ 109 E) 1.1 $\times$ 1020 A) 9.2 $\times$ 10-21 B) 2.1 $\times$ 10-10 C) 6.6 $\times$ 10-6 D) 4.7 $\times$ 109 E) 1.1 $\times$ 1020

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)

A) 0.10 B) 0.24 C) 2.1 D) 4.2 E) 4.8 A) 0.10 B) 0.24 C) 2.1 D) 4.2 E) 4.8

Exam 16: Principles of Reactivity: Chemical Equilibria

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:

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Question 1

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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?

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Question 2

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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)

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Question 3

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

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Question 4

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

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Question 5

For which of the following equilibria does K_c = K_p?

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Question 6

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?

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Question 7

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

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Question 8

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)

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Question 9

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)

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Question 10

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

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Question 11

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

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Question 12

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

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Question 13

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

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Question 14

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:

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Question 15

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

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Question 16

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

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Question 17

What balanced equation is the following equilibrium expression derived from?

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Question 18

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

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Question 19

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)

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Question 20

Showing 1 - 20 of 82

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:

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

For which of the following equilibria does K_c = K_p?

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?

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)

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

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:

What balanced equation is the following equilibrium expression derived from?

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

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)

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Exam 16: Principles of Reactivity: Chemical Equilibria

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 Kc at 700.°C for the formation of ammonia is:

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

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

For which of the following equilibria does Kc = Kp?

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?

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

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

Nitrogen and oxygen gases may react to form nitrogen monoxide. At 1500 ∘\circ∘ C,Kc 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?

At 700 K,Kp 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))

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,Kp,for the reaction is:

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-?

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,Kc,for the following reaction. PbBr2(s)+ 2 OH-(aq) Pb(OH)2(s)+ 2 Br-(aq)

What balanced equation is the following equilibrium expression derived from?

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

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)

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Mathlets Review: The Tools of Quantitative Chemistry

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Stoichiometry: Quantitative Information About Chemical Reactions

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The Structure of Atoms and Periodic Trends

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Bonding and Molecular Structure: Orbital Hybridization and Molecular Orbitals

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For which of the following equilibria does K_c = K_p?

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?

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)

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:

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

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)