Question 1

The value of K for a given reaction is a constant and does not have units.

Accepted Answer

A) True 
 B)False

Question 2

Consider the reaction 4NH3(g)+ 3O2(g) →2N2(g)+ 6H2O(g),K = 1080 at a certain temperature.
Initially,all reactants and products have concentrations equal to 12 M.At equilibrium,the approximate concentration of ammonia is

Accepted Answer

A) 6 M. 
B) 3 M. 
C) 12 M. 
D) 18 M. 
E) 0 M. 
A) 6 M. 
B) 3 M. 
C) 12 M. 
D) 18 M. 
E) 0 M.

Question 3

Consider the reaction
N2(g)3H2(g) →2NH3(g)
If the initial concentrations of nitrogen and hydrogen are each 1.0 M,and X is the equilibrium concentration of ammonia,what is the correct equilibrium expression?

Accepted Answer

K<sub>c</sub> = (X/2

Question 4

What is the relationship between K and Kc for the reaction below? NH4(NH2CO2)(s) →2NH3(g)+ CO2(g)

Accepted Answer

A) Kc = (RT)2K 
B) K = RTKc  
C) K = (RT)2Kc  
D) K = (RT)3Kc  
E) Kc = (RT)3K 
A) Kc = (RT)2K 
B) K = RTKc  
C) K = (RT)2Kc  
D) K = (RT)3Kc  
E) Kc = (RT)3K

Question 5

If a reaction mixture that is not at equilibrium contains more products than reactants,$\Delta$G > 0 for the forward reaction.

Accepted Answer

A) True 
 B)False

Question 6

Consider the reaction Ni(s)+ 4CO(g) →Ni(CO)4(g)
At 30S1U1P1$\circ$S1S1P0C and PCO = 1 atm,Ni reacts with CO(g)to form Ni(CO)4(g).At 200S1U1P1$\circ$S1S1P0C,Ni(CO)4(g)decomposes to Ni(s)and CO(g).This means

Accepted Answer

A) adding an inert gas like argon favors the forward reaction. 
B) the activation energy for the forward reaction is greater than for the reverse reaction. 
C) the forward reaction is endothermic. 
D) K at 30S1U1P1$\circ$S1S1P0C is greater than K at 200S1U1P1$\circ$S1S1P0C. 
E) a decrease in pressure favors the forward reaction. 
A) adding an inert gas like argon favors the forward reaction. 
B) the activation energy for the forward reaction is greater than for the reverse reaction. 
C) the forward reaction is endothermic. 
D) K at 30S1U1P1$\circ$S1S1P0C is greater than K at 200S1U1P1$\circ$S1S1P0C. 
E) a decrease in pressure favors the forward reaction.

Question 7

For any reaction at equilibrium,$\Delta$G < 0.

Accepted Answer

A) True 
 B)False

Question 8

Consider the reaction
Na+(g)+ Cl-(g) → NaCl(s)
If the temperature is lowered,the products/reactants are favored.

Accepted Answer

The answer of Consider the reaction
Na+(g)+ Cl-(g) → NaCl(s)
If the...

Question 9

The reaction free energy $\Delta$Gr = $\Delta$G°r - RTln(K).

Accepted Answer

A) True 
 B)False

Question 10

For the reaction Br2(g) →2Br(g),$\Delta$Gro = +161.69 kJ·mol-1 at 25S1U1P1$\circ$S1S1P0C.Calculate the value of Kc for this reaction.

Accepted Answer

A) 0.0378 
B) 1.12 * 10-27 
C) 1.83 * 10-30 
D) 4.54 * 10-29 
A) 0.0378 
B) 1.12 * 10-27 
C) 1.83 * 10-30 
D) 4.54 * 10-29

Question 11

Given: C(s)+ CO2(g) → 2CO(g) At equilibrium at a certain temperature,the partial pressures of CO(g)and CO2(g)are 1.44 atm and 0.820 atm,respectively.Calculate the value of K for this reaction.

Accepted Answer

A) 2.53 
B) 10.1 
C) 1.76 
D) 3.08 
E) 3.51 
A) 2.53 
B) 10.1 
C) 1.76 
D) 3.08 
E) 3.51

Question 12

Given: C(s)+ CO2(g) → 2CO(g) At equilibrium at a certain temperature,the partial pressures of CO(g)and CO2(g)are 1.22 atm and 0.780 atm,respectively.Calculate the value of K for this reaction.

Accepted Answer

A) 3.13 
B) 2.00 
C) 1.91 
D) 1.56 
E) 0.640 
A) 3.13 
B) 2.00 
C) 1.91 
D) 1.56 
E) 0.640

Question 13

Calculate $\Delta$G at 298 K for the reaction C2H5OH(l)$\rightarrow$C2H5OH(g,0.0263 bar)
Given $\Delta$GS1U1P1$\circ$S1S1P0 = 6.2 kJ at 298 K.

Accepted Answer

A) 6.2 kJ 
B) 15 kJ 
C) 2.8 kJ 
D) -2.8 kJ 
E) -15 kJ 
A) 6.2 kJ 
B) 15 kJ 
C) 2.8 kJ 
D) -2.8 kJ 
E) -15 kJ

Question 14

For the decomposition of ammonia to nitrogen and hydrogen,the equilibrium constant is 1.47 * 10-6 at 298 K.Calculate the temperature at which K = 1.00.For this reaction,$\Delta$HS1U1P1$\circ$S1S1P0 = 92.38 kJ.mol-1.

Accepted Answer

A) 193 K 
B) 353 K 
C) 466 K 
D) 492 K 
E) 219 K 
A) 193 K 
B) 353 K 
C) 466 K 
D) 492 K 
E) 219 K

The value of K for a given reaction is a constant and does not have units.

Consider the reaction 4NH₃(g)+ 3O₂(g) →2N₂(g)+ 6H₂O(g),K = 10⁸⁰ at a certain temperature. Initially,all reactants and products have concentrations equal to 12 M.At equilibrium,the approximate concentration of ammonia is

Consider the reaction N₂(g)3H₂(g) →2NH₃(g) If the initial concentrations of nitrogen and hydrogen are each 1.0 M,and X is the equilibrium concentration of ammonia,what is the correct equilibrium expression?

What is the relationship between K and K_c for the reaction below? NH₄(NH₂CO₂)(s) →2NH₃(g)+ CO₂(g)

If a reaction mixture that is not at equilibrium contains more products than reactants, $\Delta$ G > 0 for the forward reaction.

Consider the reaction Ni(s)+ 4CO(g) →Ni(CO)₄(g) At 30^$\circ$C and P_CO = 1 atm,Ni reacts with CO(g)to form Ni(CO)₄(g).At 200^$\circ$C,Ni(CO)₄(g)decomposes to Ni(s)and CO(g).This means

For any reaction at equilibrium, $\Delta$ G < 0.

Consider the reaction Na⁺(g)+ Cl^-(g) → NaCl(s) If the temperature is lowered,the products/reactants are favored.

The reaction free energy $\Delta$ G_r = $\Delta$ G°_r - RTln(K).

For the reaction Br₂(g) →2Br(g), $\Delta$ G_r^o = +161.69 kJ·mol^-1 at 25^$\circ$C.Calculate the value of K_c for this reaction.

Given: C(s)+ CO₂(g) → 2CO(g) At equilibrium at a certain temperature,the partial pressures of CO(g)and CO₂(g)are 1.44 atm and 0.820 atm,respectively.Calculate the value of K for this reaction.

Given: C(s)+ CO₂(g) → 2CO(g) At equilibrium at a certain temperature,the partial pressures of CO(g)and CO₂(g)are 1.22 atm and 0.780 atm,respectively.Calculate the value of K for this reaction.

Calculate $\Delta$ G at 298 K for the reaction C₂H₅OH(l) $\rightarrow$ C₂H₅OH(g,0.0263 bar) Given $\Delta$ G^$\circ$ = 6.2 kJ at 298 K.

For the decomposition of ammonia to nitrogen and hydrogen,the equilibrium constant is 1.47 * 10^-6 at 298 K.Calculate the temperature at which K = 1.00.For this reaction, $\Delta$ H^$\circ$ = 92.38 kJ.mol^-1.

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Exam 11: Chemical Equilibria

The value of K for a given reaction is a constant and does not have units.

Consider the reaction 4NH3(g)+ 3O2(g) →2N2(g)+ 6H2O(g),K = 1080 at a certain temperature. Initially,all reactants and products have concentrations equal to 12 M.At equilibrium,the approximate concentration of ammonia is

Consider the reaction N2(g)3H2(g) →2NH3(g) If the initial concentrations of nitrogen and hydrogen are each 1.0 M,and X is the equilibrium concentration of ammonia,what is the correct equilibrium expression?

What is the relationship between K and Kc for the reaction below? NH4(NH2CO2)(s) →2NH3(g)+ CO2(g)

If a reaction mixture that is not at equilibrium contains more products than reactants, Δ\DeltaΔ G > 0 for the forward reaction.

Consider the reaction Ni(s)+ 4CO(g) →Ni(CO)4(g) At 30 ∘\circ∘ C and PCO = 1 atm,Ni reacts with CO(g)to form Ni(CO)4(g).At 200 ∘\circ∘ C,Ni(CO)4(g)decomposes to Ni(s)and CO(g).This means

For any reaction at equilibrium, Δ\DeltaΔ G < 0.

Consider the reaction Na+(g)+ Cl-(g) → NaCl(s) If the temperature is lowered,the products/reactants are favored.

The reaction free energy Δ\DeltaΔ Gr = Δ\DeltaΔ G°r - RTln(K).

For the reaction Br2(g) →2Br(g), Δ\DeltaΔ Gro = +161.69 kJ·mol-1 at 25 ∘\circ∘ C.Calculate the value of Kc for this reaction.

Given: C(s)+ CO2(g) → 2CO(g) At equilibrium at a certain temperature,the partial pressures of CO(g)and CO2(g)are 1.44 atm and 0.820 atm,respectively.Calculate the value of K for this reaction.

Given: C(s)+ CO2(g) → 2CO(g) At equilibrium at a certain temperature,the partial pressures of CO(g)and CO2(g)are 1.22 atm and 0.780 atm,respectively.Calculate the value of K for this reaction.

Calculate Δ\DeltaΔ G at 298 K for the reaction C2H5OH(l) →\rightarrow→ C2H5OH(g,0.0263 bar) Given Δ\DeltaΔ G ∘\circ∘ = 6.2 kJ at 298 K.

For the decomposition of ammonia to nitrogen and hydrogen,the equilibrium constant is 1.47 * 10-6 at 298 K.Calculate the temperature at which K = 1.00.For this reaction, Δ\DeltaΔ H ∘\circ∘ = 92.38 kJ.mol-1.

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Quantum Mechanics in Action: Atoms

Chemical Bonds

Molecular Shape and Structure

The Properties of Gases

Liquids and Solids

Inorganic Materials

Thermodynamics: The First Law

Thermodynamics: The Second and Third Laws

Physical Equilibria

Acids and Bases

Aqueous Equilibria

Electrochemistry

Chemical Kinetics

The Elements: the Main Group Elements

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Consider the reaction 4NH₃(g)+ 3O₂(g) →2N₂(g)+ 6H₂O(g),K = 10⁸⁰ at a certain temperature. Initially,all reactants and products have concentrations equal to 12 M.At equilibrium,the approximate concentration of ammonia is

Consider the reaction N₂(g)3H₂(g) →2NH₃(g) If the initial concentrations of nitrogen and hydrogen are each 1.0 M,and X is the equilibrium concentration of ammonia,what is the correct equilibrium expression?

What is the relationship between K and K_c for the reaction below? NH₄(NH₂CO₂)(s) →2NH₃(g)+ CO₂(g)

If a reaction mixture that is not at equilibrium contains more products than reactants, $\Delta$ G > 0 for the forward reaction.

Consider the reaction Ni(s)+ 4CO(g) →Ni(CO)₄(g) At 30^$\circ$C and P_CO = 1 atm,Ni reacts with CO(g)to form Ni(CO)₄(g).At 200^$\circ$C,Ni(CO)₄(g)decomposes to Ni(s)and CO(g).This means

For any reaction at equilibrium, $\Delta$ G < 0.

Consider the reaction Na⁺(g)+ Cl^-(g) → NaCl(s) If the temperature is lowered,the products/reactants are favored.

The reaction free energy $\Delta$ G_r = $\Delta$ G°_r - RTln(K).

For the reaction Br₂(g) →2Br(g), $\Delta$ G_r^o = +161.69 kJ·mol^-1 at 25^$\circ$C.Calculate the value of K_c for this reaction.

Given: C(s)+ CO₂(g) → 2CO(g) At equilibrium at a certain temperature,the partial pressures of CO(g)and CO₂(g)are 1.44 atm and 0.820 atm,respectively.Calculate the value of K for this reaction.

Given: C(s)+ CO₂(g) → 2CO(g) At equilibrium at a certain temperature,the partial pressures of CO(g)and CO₂(g)are 1.22 atm and 0.780 atm,respectively.Calculate the value of K for this reaction.

Calculate $\Delta$ G at 298 K for the reaction C₂H₅OH(l) $\rightarrow$ C₂H₅OH(g,0.0263 bar) Given $\Delta$ G^$\circ$ = 6.2 kJ at 298 K.

For the decomposition of ammonia to nitrogen and hydrogen,the equilibrium constant is 1.47 * 10^-6 at 298 K.Calculate the temperature at which K = 1.00.For this reaction, $\Delta$ H^$\circ$ = 92.38 kJ.mol^-1.