Question 1

The _____ is an economical process for making nitric acid in which nitric oxide is prepared by the oxidation of ammonia.

Accepted Answer

A) ​Hall-Héroult process 
B) ​Ostwald process 
C) ​Frasch process 
D) ​Bessemer process 
E) ​Castner process 
A) ​Hall-Héroult process 
B) ​Ostwald process 
C) ​Frasch process 
D) ​Bessemer process 
E) ​Castner process

Question 2

For the equilibrium PCl5(g)   PCl3(g)+ Cl2(g),Kc = 2.0 × 101 at 240°C.If pure PCl5 is placed in a 1.00-L container and allowed to come to equilibrium,and the equilibrium concentration of PCl3(g)is 0.27 M,what is the equilibrium concentration of PCl5(g)?

Accepted Answer

A) 0.54 M 
B) 0.13 M 
C) 0.013 M 
D) 0.0036 M 
E) 8.6 M 
A) 0.54 M 
B) 0.13 M 
C) 0.013 M 
D) 0.0036 M 
E) 8.6 M

Question 3

When cobalt chloride is added to pure water,the Co2+ ions hydrate.The hydrated form then reacts with the Cl- ions to set up the equilibrium shown here:
Co(H2O)62+ + 4Cl-  
CoCl42- + 6H2O
(pink)
(blue)
Which statement accurately describes the change that the system will undergo if water is added?

Accepted Answer

A) The color will become more blue. 
B) The equilibrium will shift to the right. 
C) More water will be produced. 
D) More chloride ions will be produced. 
E) There will be less of the hydrated cobalt ion at the new equilibrium position. 
A) The color will become more blue. 
B) The equilibrium will shift to the right. 
C) More water will be produced. 
D) More chloride ions will be produced. 
E) There will be less of the hydrated cobalt ion at the new equilibrium position.

Question 4

Carbon tetrachloride may react with oxygen to produce chlorine and carbonyl chloride.
2CCl4(g)+ O2(g)  
2COCl2(g)+ 2Cl2(g); Kc = 9.9 × 1051
What is Kc for the following equilibrium?
COCl2(g)+ Cl2(g)  
CCl4(g)+ 1/2O2(g)

Accepted Answer

A) 9.9 × 10-51 
B) 5.0 × 10-53 
C) 1.0 × 10-26 
D) 1.0 × 10-52 
E) -9.9 × 1051 
A) 9.9 × 10-51 
B) 5.0 × 10-53 
C) 1.0 × 10-26 
D) 1.0 × 10-52 
E) -9.9 × 1051

Question 5

What is the reaction quotient (Q)for the equilibrium
​
TlSCN(s)  
Tl+(aq)+ SCN-(aq)
​
When 0.1837 L of  
M Tl+ is combined with 0.1335 L of  
M SCN- in the presence of an excess of TlSCN(s)?

Accepted Answer

A)    
B)    
C)    
D)    
E)    
A)    
B)    
C)    
D)    
E)

Question 6

For the reaction Br2(g)+ Cl2(g)   2BrCl(g),at equilibrium,it is found that the concentrations of Br2,Cl2,and BrCl are 0.484 M,0.105 M,and 1.24 × 10-3 M,respectively.What is the value of Kc?

Accepted Answer

A) 3.01 × 10-5 
B) 1.20 × 10-4 
C) 2.43 × 10-2 
D) 4.12 × 101 
E) 3.32 × 104 
A) 3.01 × 10-5 
B) 1.20 × 10-4 
C) 2.43 × 10-2 
D) 4.12 × 101 
E) 3.32 × 104

Question 7

At 800 K,Kc for the following equilibrium is 4.2 × 10-3.
2HgO(s)  
2Hg(l)+ O2(g)
Suppose 82.3 g of mercury (II)oxide is placed in a sealed 2.50-L vessel at 800 K.What is the partial pressure of oxygen gas at equilibrium? (R = 0.0821 L ∙ atm/(K ∙ mol))

Accepted Answer

A) 8.7 atm 
B) 4.3 atm 
C) 0.27 atm 
D) 0.0042 atm 
E) 22 atm 
A) 8.7 atm 
B) 4.3 atm 
C) 0.27 atm 
D) 0.0042 atm 
E) 22 atm

Question 8

Which of the following statements is incorrect concerning the addition of a catalyst to an equilibrium reaction system?

Accepted Answer

A) The catalyst speeds up the attainment of equilibrium. 
B) If the reactants are capable of forming many different products,a catalyst may selectively speed up one reaction over another. 
C) The catalyst increases the rate of both the forward and the reverse reaction. 
D) The catalyst increases the yield of the products. 
E) The catalyst is not consumed in either the forward or the reverse reaction. 
A) The catalyst speeds up the attainment of equilibrium. 
B) If the reactants are capable of forming many different products,a catalyst may selectively speed up one reaction over another. 
C) The catalyst increases the rate of both the forward and the reverse reaction. 
D) The catalyst increases the yield of the products. 
E) The catalyst is not consumed in either the forward or the reverse reaction.

Question 9

A sample of ammonia gas was allowed to come to equilibrium at 400 K.
2NH3(g)  
N2(g)+ 3H2(g)
At equilibrium,it was found that the concentration of H2 was 0.0484 M,the concentration of N2 was 0.0161 M,and the concentration of NH3 was 0.295 M.What was the initial concentration of ammonia?

Accepted Answer

A) 0.161 M 
B) 0.228 M 
C) 0.36 M 
D) 0.311 M 
E) 0.328 M 
A) 0.161 M 
B) 0.228 M 
C) 0.36 M 
D) 0.311 M 
E) 0.328 M

Question 10

For the following reaction system at equilibrium,which one of the changes below would cause the equilibrium to shift to the right?
Br2(g)+ 2NO(g)  
2NOBr(g); ΔH° = -30 kJ

Accepted Answer

A) Remove some NO. 
B) Remove some Br2. 
C) Add some NOBr. 
D) Increase the volume of the reaction vessel. 
E) Decrease the temperature. 
A) Remove some NO. 
B) Remove some Br2. 
C) Add some NOBr. 
D) Increase the volume of the reaction vessel. 
E) Decrease the temperature.

Question 11

When cobalt chloride is added to pure water,the Co2+ ions hydrate.The hydrated form then reacts with the Cl- ions to set up the equilibrium shown here:
Co(H2O)62+ + 4Cl-  
CoCl42- + 6H2O
(pink)
(blue)
Which statement describes the change that the system will undergo if potassium chloride is added?

Accepted Answer

A) It should become more pink. 
B) Nothing will change. 
C) The silver ion will react with the CoCl42-. 
D) Water will be produced. 
E) It should become more blue. 
A) It should become more pink. 
B) Nothing will change. 
C) The silver ion will react with the CoCl42-. 
D) Water will be produced. 
E) It should become more blue.

Question 12

A sample of ammonia gas was allowed to come to equilibrium at 400 K.
2NH3(g)  
N2(g)+ 3H2(g)
At equilibrium,it was found that the concentration of H2 was 0.0372 M,the concentration of N2 was 0.0124 M,and the concentration of NH3 was 0.175 M.What is Kp for this equilibrium? (R = 0.0821 L ∙ atm/(K ∙ mol))

Accepted Answer

A) 4.28 
B) 2.85 
C) 1.70 × 10-2 
D) 1.95 × 10-8 
E) 2.26 × 10-2 
A) 4.28 
B) 2.85 
C) 1.70 × 10-2 
D) 1.95 × 10-8 
E) 2.26 × 10-2

Question 13

When gaseous carbon monoxide and hydrogen are combined in a sealed vessel and heated they will eventually form an equilbrium mixture of reactants and products according to the balanced chemical equilibrium below.
CO(g)+ 3H2(g)  
CH4(g)+ H2O(g)
In one such reaction 3 moles of one reactant were combined with 1 mole of the other reactant in a fixed volume vessel and heated to 1200 K.Analysis of the reaction mixture at various times gave the results below.Which component of the reaction mixture is represented by curve B?

Accepted Answer

A) carbon monoxide 
B) either methane or water 
C) hydrogen 
D) either hydrogen or carbon monoxide 
E) not enough information to decide 
A) carbon monoxide 
B) either methane or water 
C) hydrogen 
D) either hydrogen or carbon monoxide 
E) not enough information to decide

Question 14

The following equilibrium is established in a sealed,rigid container.How could the partial pressure of SO2 at equilibrium be increased?
SO2Cl2(g)  
SO2(g)+ Cl2(g); ΔH = +67 kJ

Accepted Answer

A) by adding an inert gas such as helium 
B) by increasing the temperature 
C) by removing SO2Cl2 as it is formed 
D) by adding Cl2 to the system 
E) by decreasing the volume of the reaction vessel 
A) by adding an inert gas such as helium 
B) by increasing the temperature 
C) by removing SO2Cl2 as it is formed 
D) by adding Cl2 to the system 
E) by decreasing the volume of the reaction vessel

Question 15

A sample of ammonia gas was allowed to come to equilibrium at 400 K.
2NH3(g)  
N2(g)+ 3H2(g)
At equilibrium,it was found that the concentration of H2 was 0.0551 M,the concentration of N2 was 0.0183 M,and the concentration of NH3 was 0.383 M.What is Kc for this equilibrium?

Accepted Answer

A) 3.97 × 10-3 
B) 1.58 × 10-5 
C) 2.10 × 10-5 
D) 2.40 × 10-1 
E) 2.65 × 10-3 
A) 3.97 × 10-3 
B) 1.58 × 10-5 
C) 2.10 × 10-5 
D) 2.40 × 10-1 
E) 2.65 × 10-3

Question 16

Consider the following reaction:
2HF(g)  
H2(g)+ F2(g)(Kc = 1.00 × 10-2)
Given that 1.00 mol of HF(g),0.200 mol of H2(g),and 0.750 mol of F2(g)are mixed in a 5.00-L flask,determine the reaction quotient,Q.

Accepted Answer

A) Q = 0.0375 
B) Q = 0.150 
C) Q = 0.0300 
D) Q = 1.95 
E) none of these 
A) Q = 0.0375 
B) Q = 0.150 
C) Q = 0.0300 
D) Q = 1.95 
E) none of these

Question 17

For the reaction 2HI(g)   H2(g)+ I2(g),Kc = 0.290 at 400 K.If the initial concentrations of HI,H2,and I2 are all 1.50 × 10-3 M at 400 K,which one of the following statements is correct?

Accepted Answer

A) The concentrations of HI and I2 will increase as the system is approaching equilibrium. 
B) The concentrations of H2 and I2 will increase as the system is approaching equilibrium. 
C) The system is at equilibrium. 
D) The concentrations of H2 and HI will decrease as the system is approaching equilibrium. 
E) The concentration of HI will increase as the system is approaching equilibrium. 
A) The concentrations of HI and I2 will increase as the system is approaching equilibrium. 
B) The concentrations of H2 and I2 will increase as the system is approaching equilibrium. 
C) The system is at equilibrium. 
D) The concentrations of H2 and HI will decrease as the system is approaching equilibrium. 
E) The concentration of HI will increase as the system is approaching equilibrium.

Question 18

A 35.00-L vessel at 700 K initially contains HI(g)at a pressure of 5.80 atm; at equilibrium,it is found that the partial pressure of H2(g)is 0.56 atm.What is the partial pressure of HI(g)at equilibrium?
2HI(g)  
H2(g)+ I2(g)

Accepted Answer

A) 5.8 atm 
B) 5.23 atm 
C) 4.67 atm 
D) 6.36 atm 
E) 0.561 atm 
A) 5.8 atm 
B) 5.23 atm 
C) 4.67 atm 
D) 6.36 atm 
E) 0.561 atm

Question 19

Consider the following equilibrium:
CO2(g)+ C(graphite)  
2CO(g); ΔH = 172.5 kJ
The equilibrium constant for this reaction will

Accepted Answer

A) increase if the temperature is decreased. 
B) decrease with increasing temperature. 
C) increase at some pressures and decrease at other pressures. 
D) increase with increasing temperature. 
E) not change if the temperature is increased. 
A) increase if the temperature is decreased. 
B) decrease with increasing temperature. 
C) increase at some pressures and decrease at other pressures. 
D) increase with increasing temperature. 
E) not change if the temperature is increased.

Question 20

In which of the following reactions does an instantaneous increase in the volume of the reaction vessel favor formation of the products?

Accepted Answer

A) PCl5(g)   PCl3(g)+ Cl2(g) 
B) N2(g)+ 3H2(g)   2NH3(g) 
C) H2(g)+ I2(g)   2HI(g) 
D) MgO(s)+ CO2(g)   MgCO3(s) 
E) N2(g)+ O2(g)   2NO(g) 
A) PCl5(g)   PCl3(g)+ Cl2(g) 
B) N2(g)+ 3H2(g)   2NH3(g) 
C) H2(g)+ I2(g)   2HI(g) 
D) MgO(s)+ CO2(g)   MgCO3(s) 
E) N2(g)+ O2(g)   2NO(g)

The _____ is an economical process for making nitric acid in which nitric oxide is prepared by the oxidation of ammonia.

For the equilibrium PCl₅(g) PCl₃(g)+ Cl₂(g),K_c = 2.0 × 10¹ at 240°C.If pure PCl₅ is placed in a 1.00-L container and allowed to come to equilibrium,and the equilibrium concentration of PCl₃(g)is 0.27 M,what is the equilibrium concentration of PCl₅(g)?

Carbon tetrachloride may react with oxygen to produce chlorine and carbonyl chloride. 2CCl₄(g)+ O₂(g) 2COCl₂(g)+ 2Cl₂(g); K_c = 9.9 × 10⁵¹ What is K_c for the following equilibrium? COCl₂(g)+ Cl₂(g) CCl₄(g)+ 1/2O₂(g)

What is the reaction quotient (Q)for the equilibrium TlSCN(s) Tl⁺(aq)+ SCN^-(aq) When 0.1837 L of M Tl⁺ is combined with 0.1335 L of M SCN^- in the presence of an excess of TlSCN(s)?

For the reaction Br₂(g)+ Cl₂(g) 2BrCl(g),at equilibrium,it is found that the concentrations of Br₂,Cl₂,and BrCl are 0.484 M,0.105 M,and 1.24 × 10^-3 M,respectively.What is the value of K_c?

At 800 K,K_c for the following equilibrium is 4.2 × 10^-3. 2HgO(s) 2Hg(l)+ O₂(g) Suppose 82.3 g of mercury (II)oxide is placed in a sealed 2.50-L vessel at 800 K.What is the partial pressure of oxygen gas at equilibrium? (R = 0.0821 L ∙ atm/(K ∙ mol))

Which of the following statements is incorrect concerning the addition of a catalyst to an equilibrium reaction system?

A sample of ammonia gas was allowed to come to equilibrium at 400 K. 2NH₃(g) N₂(g)+ 3H₂(g) At equilibrium,it was found that the concentration of H₂ was 0.0484 M,the concentration of N₂ was 0.0161 M,and the concentration of NH₃ was 0.295 M.What was the initial concentration of ammonia?

For the following reaction system at equilibrium,which one of the changes below would cause the equilibrium to shift to the right? Br₂(g)+ 2NO(g) 2NOBr(g); ΔH° = -30 kJ

The following equilibrium is established in a sealed,rigid container.How could the partial pressure of SO₂ at equilibrium be increased? SO₂Cl₂(g) SO₂(g)+ Cl₂(g); ΔH = +67 kJ

A sample of ammonia gas was allowed to come to equilibrium at 400 K. 2NH₃(g) N₂(g)+ 3H₂(g) At equilibrium,it was found that the concentration of H₂ was 0.0551 M,the concentration of N₂ was 0.0183 M,and the concentration of NH₃ was 0.383 M.What is K_c for this equilibrium?

Consider the following reaction: 2HF(g) H₂(g)+ F₂(g)(K_c = 1.00 × 10^-2) Given that 1.00 mol of HF(g),0.200 mol of H₂(g),and 0.750 mol of F₂(g)are mixed in a 5.00-L flask,determine the reaction quotient,Q.

For the reaction 2HI(g) H₂(g)+ I₂(g),K_c = 0.290 at 400 K.If the initial concentrations of HI,H₂,and I₂ are all 1.50 × 10^-3 M at 400 K,which one of the following statements is correct?

A 35.00-L vessel at 700 K initially contains HI(g)at a pressure of 5.80 atm; at equilibrium,it is found that the partial pressure of H₂(g)is 0.56 atm.What is the partial pressure of HI(g)at equilibrium? 2HI(g) H₂(g)+ I₂(g)

Consider the following equilibrium: CO₂(g)+ C(graphite) 2CO(g); ΔH = 172.5 kJ The equilibrium constant for this reaction will

In which of the following reactions does an instantaneous increase in the volume of the reaction vessel favor formation of the products?

Chemistry and Measurement

Atoms, molecules, and Ions

Calculations With Chemical Formulas and Equations

Chemical Reactions

The Gaseous State

Thermochemistry

Quantum Theory of the Atom

Electron Configurations and Periodicity

Ionic and Covalent Bonding

Molecular Geometry and Chemical Bonding Theory

States of Matter; Liquids and Solids

Solutions

Rates of Reaction

Acids and Bases

Acid-Base Equilibria

Solubility and Complex-Ion Equilibria

Thermodynamics and Equilibrium

Electrochemistry

Nuclear Chemistry

Chemistry of the Main-Group Metals

The Transition Elements and Coordination Compounds

Organic Chemistry

Polymer Materials: Synthetic and Biological

Filters

Exam 14: Chemical Equilibrium

The _____ is an economical process for making nitric acid in which nitric oxide is prepared by the oxidation of ammonia.

For the equilibrium PCl5(g) PCl3(g)+ Cl2(g),Kc = 2.0 × 101 at 240°C.If pure PCl5 is placed in a 1.00-L container and allowed to come to equilibrium,and the equilibrium concentration of PCl3(g)is 0.27 M,what is the equilibrium concentration of PCl5(g)?

When cobalt chloride is added to pure water,the Co2+ ions hydrate.The hydrated form then reacts with the Cl- ions to set up the equilibrium shown here: Co(H2O)62+ + 4Cl- CoCl42- + 6H2O (pink) (blue) Which statement accurately describes the change that the system will undergo if water is added?

Carbon tetrachloride may react with oxygen to produce chlorine and carbonyl chloride. 2CCl4(g)+ O2(g) 2COCl2(g)+ 2Cl2(g); Kc = 9.9 × 1051 What is Kc for the following equilibrium? COCl2(g)+ Cl2(g) CCl4(g)+ 1/2O2(g)

What is the reaction quotient (Q)for the equilibrium ​ TlSCN(s) Tl+(aq)+ SCN-(aq) ​ When 0.1837 L of M Tl+ is combined with 0.1335 L of M SCN- in the presence of an excess of TlSCN(s)?

For the reaction Br2(g)+ Cl2(g) 2BrCl(g),at equilibrium,it is found that the concentrations of Br2,Cl2,and BrCl are 0.484 M,0.105 M,and 1.24 × 10-3 M,respectively.What is the value of Kc?

At 800 K,Kc for the following equilibrium is 4.2 × 10-3. 2HgO(s) 2Hg(l)+ O2(g) Suppose 82.3 g of mercury (II)oxide is placed in a sealed 2.50-L vessel at 800 K.What is the partial pressure of oxygen gas at equilibrium? (R = 0.0821 L ∙ atm/(K ∙ mol))

Which of the following statements is incorrect concerning the addition of a catalyst to an equilibrium reaction system?

A sample of ammonia gas was allowed to come to equilibrium at 400 K. 2NH3(g) N2(g)+ 3H2(g) At equilibrium,it was found that the concentration of H2 was 0.0484 M,the concentration of N2 was 0.0161 M,and the concentration of NH3 was 0.295 M.What was the initial concentration of ammonia?

For the following reaction system at equilibrium,which one of the changes below would cause the equilibrium to shift to the right? Br2(g)+ 2NO(g) 2NOBr(g); ΔH° = -30 kJ

When cobalt chloride is added to pure water,the Co2+ ions hydrate.The hydrated form then reacts with the Cl- ions to set up the equilibrium shown here: Co(H2O)62+ + 4Cl- CoCl42- + 6H2O (pink) (blue) Which statement describes the change that the system will undergo if potassium chloride is added?

The following equilibrium is established in a sealed,rigid container.How could the partial pressure of SO2 at equilibrium be increased? SO2Cl2(g) SO2(g)+ Cl2(g); ΔH = +67 kJ

A sample of ammonia gas was allowed to come to equilibrium at 400 K. 2NH3(g) N2(g)+ 3H2(g) At equilibrium,it was found that the concentration of H2 was 0.0551 M,the concentration of N2 was 0.0183 M,and the concentration of NH3 was 0.383 M.What is Kc for this equilibrium?

Consider the following reaction: 2HF(g) H2(g)+ F2(g)(Kc = 1.00 × 10-2) Given that 1.00 mol of HF(g),0.200 mol of H2(g),and 0.750 mol of F2(g)are mixed in a 5.00-L flask,determine the reaction quotient,Q.

For the reaction 2HI(g) H2(g)+ I2(g),Kc = 0.290 at 400 K.If the initial concentrations of HI,H2,and I2 are all 1.50 × 10-3 M at 400 K,which one of the following statements is correct?

A 35.00-L vessel at 700 K initially contains HI(g)at a pressure of 5.80 atm; at equilibrium,it is found that the partial pressure of H2(g)is 0.56 atm.What is the partial pressure of HI(g)at equilibrium? 2HI(g) H2(g)+ I2(g)

Consider the following equilibrium: CO2(g)+ C(graphite) 2CO(g); ΔH = 172.5 kJ The equilibrium constant for this reaction will

In which of the following reactions does an instantaneous increase in the volume of the reaction vessel favor formation of the products?

Chemistry and Measurement

Atoms, molecules, and Ions

Calculations With Chemical Formulas and Equations

Chemical Reactions

The Gaseous State

Thermochemistry

Quantum Theory of the Atom

Electron Configurations and Periodicity

Ionic and Covalent Bonding

Molecular Geometry and Chemical Bonding Theory

States of Matter; Liquids and Solids

Solutions

Rates of Reaction

Acids and Bases

Acid-Base Equilibria

Solubility and Complex-Ion Equilibria

Thermodynamics and Equilibrium

Electrochemistry

Nuclear Chemistry

Chemistry of the Main-Group Metals

The Transition Elements and Coordination Compounds

Organic Chemistry

Polymer Materials: Synthetic and Biological

Filters

For the equilibrium PCl₅(g) PCl₃(g)+ Cl₂(g),K_c = 2.0 × 10¹ at 240°C.If pure PCl₅ is placed in a 1.00-L container and allowed to come to equilibrium,and the equilibrium concentration of PCl₃(g)is 0.27 M,what is the equilibrium concentration of PCl₅(g)?

Carbon tetrachloride may react with oxygen to produce chlorine and carbonyl chloride. 2CCl₄(g)+ O₂(g) 2COCl₂(g)+ 2Cl₂(g); K_c = 9.9 × 10⁵¹ What is K_c for the following equilibrium? COCl₂(g)+ Cl₂(g) CCl₄(g)+ 1/2O₂(g)

What is the reaction quotient (Q)for the equilibrium TlSCN(s) Tl⁺(aq)+ SCN^-(aq) When 0.1837 L of M Tl⁺ is combined with 0.1335 L of M SCN^- in the presence of an excess of TlSCN(s)?

For the reaction Br₂(g)+ Cl₂(g) 2BrCl(g),at equilibrium,it is found that the concentrations of Br₂,Cl₂,and BrCl are 0.484 M,0.105 M,and 1.24 × 10^-3 M,respectively.What is the value of K_c?

At 800 K,K_c for the following equilibrium is 4.2 × 10^-3. 2HgO(s) 2Hg(l)+ O₂(g) Suppose 82.3 g of mercury (II)oxide is placed in a sealed 2.50-L vessel at 800 K.What is the partial pressure of oxygen gas at equilibrium? (R = 0.0821 L ∙ atm/(K ∙ mol))

A sample of ammonia gas was allowed to come to equilibrium at 400 K. 2NH₃(g) N₂(g)+ 3H₂(g) At equilibrium,it was found that the concentration of H₂ was 0.0484 M,the concentration of N₂ was 0.0161 M,and the concentration of NH₃ was 0.295 M.What was the initial concentration of ammonia?

For the following reaction system at equilibrium,which one of the changes below would cause the equilibrium to shift to the right? Br₂(g)+ 2NO(g) 2NOBr(g); ΔH° = -30 kJ

The following equilibrium is established in a sealed,rigid container.How could the partial pressure of SO₂ at equilibrium be increased? SO₂Cl₂(g) SO₂(g)+ Cl₂(g); ΔH = +67 kJ

A sample of ammonia gas was allowed to come to equilibrium at 400 K. 2NH₃(g) N₂(g)+ 3H₂(g) At equilibrium,it was found that the concentration of H₂ was 0.0551 M,the concentration of N₂ was 0.0183 M,and the concentration of NH₃ was 0.383 M.What is K_c for this equilibrium?

Consider the following reaction: 2HF(g) H₂(g)+ F₂(g)(K_c = 1.00 × 10^-2) Given that 1.00 mol of HF(g),0.200 mol of H₂(g),and 0.750 mol of F₂(g)are mixed in a 5.00-L flask,determine the reaction quotient,Q.

For the reaction 2HI(g) H₂(g)+ I₂(g),K_c = 0.290 at 400 K.If the initial concentrations of HI,H₂,and I₂ are all 1.50 × 10^-3 M at 400 K,which one of the following statements is correct?

A 35.00-L vessel at 700 K initially contains HI(g)at a pressure of 5.80 atm; at equilibrium,it is found that the partial pressure of H₂(g)is 0.56 atm.What is the partial pressure of HI(g)at equilibrium? 2HI(g) H₂(g)+ I₂(g)

Consider the following equilibrium: CO₂(g)+ C(graphite) 2CO(g); ΔH = 172.5 kJ The equilibrium constant for this reaction will