Question 1

The equilibrium constant for the reaction Ni(s) + 4CO(g)  →\rarr→  Ni(CO) 4(g) is 5.0 * 104 at 25ºC. What is the equilibrium constant for the reaction Ni(CO) 4(g)   Ni(CO) 4(g) is 5.0 * 104 at 25ºC. What is the equilibrium constant for the reaction Ni(CO) 4(g)     Ni(s) + 4CO(g) ? A) 2.0 * 10-5 B) 2.5 * 109 C) 5.0 * 104 D) 5.0 * 10-4 E) 2.0 * 10-3 " class="answers-bank-image d-inline" rel="preload" >  Ni(s) + 4CO(g) ?

Accepted Answer

A)  2.0 * 10-5
B)  2.5 * 109
C)  5.0 * 104
D)  5.0 * 10-4
E)  2.0 * 10-3 F) C) and D)
G) D) and E)

Question 2

For the reaction PCl3(g) + Cl2(g)  3(g) + Cl2(g)    PCl5(g) at a particular temperature, Kc = 24.3. Suppose a system at that temperature is prepared with [PCl3] = 0.10 M, [Cl2] = 0.15 M, and [PCl5] = 0.60 M. Which of these statements is true? A) The reaction is at equilibrium. B) The reaction will proceed in the direction of forming more PCl5 until equilibrium is reached. C) The reaction will proceed in the direction of forming more PCl3 and Cl2 until equilibrium is reached. D) None of the above statements is true." class="answers-bank-image d-inline" rel="preload" > PCl5(g) at a particular temperature, Kc = 24.3. Suppose a system at that temperature is prepared with [PCl3] = 0.10 M, [Cl2] = 0.15 M, and [PCl5] = 0.60 M. Which of these statements is true?

Accepted Answer

A)  The reaction is at equilibrium.
B)  The reaction will proceed in the direction of forming more PCl5 until equilibrium is reached.
C)  The reaction will proceed in the direction of forming more PCl3 and Cl2 until equilibrium is reached.
D)  None of the above statements is true.E) None of the above
F) C) and D)

Question 3

If the reaction 2H2S(g)  2S(g)     2H2(g) + S2(g) is carried out at 1065°C, Kp = 0.0120. Starting from pure H2S introduced into an evacuated vessel at 1065°C, what will the total pressure in the vessel be at equilibrium if the equilibrated mixture contains 0.300 atm of H2(g) ? A) 1.06 atm B) 1.36 atm C) 2.39 atm D) 4.20 atm E) 1.51 atm" class="answers-bank-image d-inline" rel="preload" >  2H2(g) + S2(g) is carried out at 1065°C, Kp = 0.0120. Starting from pure H2S introduced into an evacuated vessel at 1065°C, what will the total pressure in the vessel be at equilibrium if the equilibrated mixture contains 0.300 atm of H2(g) ?

Accepted Answer

A)  1.06 atm
B)  1.36 atm
C)  2.39 atm
D)  4.20 atm
E)  1.51 atmF) D) and E)
G) None of the above

Question 4

Hydrogen iodide decomposes according to the equation 2HI(g)  2(g) + I2(g) , for which Kc = 0.0156 at 400ºC. 0.550 mol HI was injected into a 2.00 L reaction vessel at 400ºC. Calculate the concentration of HI at equilibrium. A) 0.138 M B) 0.220 M C) 0.550 M D) 0.275 M E) 0.0275 M" class="answers-bank-image d-inline" rel="preload" >H2(g) + I2(g) , for which Kc = 0.0156 at 400ºC. 0.550 mol HI was injected into a 2.00 L reaction vessel at 400ºC. Calculate the concentration of HI at equilibrium.

Accepted Answer

A)  0.138 M
B)  0.220 M
C)  0.550 M
D)  0.275 M
E)  0.0275 MF) B) and D)
G) A) and B)

Question 5

Calculate Kc for the reaction 2HI(g)     c for the reaction 2HI(g)        H2(g) + I2(g) given that the concentrations of each species at equilibrium are as follows: [HI] = 0.85 mol/L, [I2] = 0.60 mol/L, [H2] = 0.27 mol/L. A) 5.25 B) 0.22 C) 4.5 D) 0.19 E) 1.6 * 102" class="answers-bank-image d-inline" rel="preload" >  H2(g) + I2(g) given that the concentrations of each species at equilibrium are as follows: [HI] = 0.85 mol/L, [I2] = 0.60 mol/L, [H2] = 0.27 mol/L.

Accepted Answer

A)  5.25
B)  0.22
C)  4.5
D)  0.19
E)  1.6 * 102F) B) and E)
G) A) and E)

Question 6

Consider the reaction N2(g)+ 3H2(g)  2NH3(g). If we use a catalyst, which way will the reaction shift?

Accepted Answer

Question 7

Equilibrium constants are known for the following reactions:
S(s)+ 3/2O2(g)  SO3(g)Kc = 9.2 * 1023
 SO3(g)  SO2(g)+ 1/2O2(g)Kc = 4.8 * 10- 4
Thus, for the reaction S(s)+ O2(g)$\rarr$ SO2(g), Kc = 4.4 * 1020.

Accepted Answer

A) True 
 B)False

Question 8

The reaction 2SO3(g)  3(g)    2SO2(g) + O2(g) is endothermic. If the temperature is increased, A) more SO3 will be produced. B) Kc will decrease. C) no change will occur in Kc . D) Kc will increase. E) the pressure will decrease." class="answers-bank-image d-inline" rel="preload" > 2SO2(g) + O2(g) is endothermic. If the temperature is increased,

Accepted Answer

A)  more SO3 will be produced.
B)  Kc will decrease.
C)  no change will occur in Kc .
D)  Kc will increase.
E)  the pressure will decrease.F) C) and D)
G) A) and B)

Question 9

Equilibrium is established for the reaction 2X(s) + Y(g)  →\rarr→  2Z(g) at 500K, Kc = 100. Determine the concentration of Z in equilibrium with 0.2 mol X and 0.50 M Y at 500K.

Accepted Answer

A)  3.2 M
B)  3.5 M
C)  4.5 M
D)  7.1 M
E)  None of these. F) None of the above
G) B) and D)

Question 10

The dissociation of solid silver chloride in water to produce silver ions and chloride ions has an equilibrium constant of 1.8 *  10-18. Based on the magnitude of the equilibrium constant, is silver chloride very soluble in water? Why?

Accepted Answer

K_c here will be [Ag⁺

Question 11

The brown gas NO2 and the colorless gas N2O4 exist in equilibrium, 2NO2 2 and the colorless gas N2O4 exist in equilibrium, 2NO2    N2O4. In an experiment, 0.625 mole of N2O4 was introduced into a 5.00 L vessel and was allowed to decompose until equilibrium was reached. The concentration of N2O4 at equilibrium was 0.0750 M. Calculate Kc for the reaction. A) 7.5 B) 0.125 C) 0.0750 D) 0.10 E) 0.050" class="answers-bank-image d-inline" rel="preload" >  N2O4. In an experiment, 0.625 mole of N2O4 was introduced into a 5.00 L vessel and was allowed to decompose until equilibrium was reached. The concentration of N2O4 at equilibrium was 0.0750 M. Calculate Kc for the reaction.

Accepted Answer

A)  7.5
B)  0.125
C)  0.0750
D)  0.10
E)  0.050F) A) and E)
G) A) and B)

Question 12

Phosgene, COCl2, a poisonous gas, decomposes according to the equation COCl2(g)  2, a poisonous gas, decomposes according to the equation COCl2(g)     CO(g) + Cl2(g) . Calculate Kp for this reaction if Kc = 0.083 at 900ºC. A) 0.125 B) 8.0 C) 6.1 D) 0.16 E) 0.083" class="answers-bank-image d-inline" rel="preload" >  CO(g) + Cl2(g) . Calculate Kp for this reaction if Kc = 0.083 at 900ºC.

Accepted Answer

A)  0.125
B)  8.0
C)  6.1
D)  0.16
E)  0.083F) D) and E)
G) A) and B)

Question 13

A quantity of liquid methanol, CH3OH, is introduced into a rigid 3.00-L vessel, the vessel is sealed, and the temperature is raised to 500K. At this temperature, the methanol vaporizes and decomposes according to the reaction CH3OH(g)  3OH, is introduced into a rigid 3.00-L vessel, the vessel is sealed, and the temperature is raised to 500K. At this temperature, the methanol vaporizes and decomposes according to the reaction CH3OH(g)     CO(g) + 2 H2(g) , Kc= 6.90 * 10-2. If the concentration of H2 in the equilibrium mixture is 0.426M, what mass of methanol was initially introduced into the vessel? A) 147 g B) 74.3 g C) 33.9 g D) 49.0 g E) 24.8 g" class="answers-bank-image d-inline" rel="preload" >  CO(g) + 2 H2(g) , Kc= 6.90 * 10-2.
If the concentration of H2 in the equilibrium mixture is 0.426M, what mass of methanol was initially introduced into the vessel?

Accepted Answer

A)  147 g
B)  74.3 g
C)  33.9 g
D)  49.0 g
E)  24.8 gF) B) and E)
G) A) and B)

Question 14

For the reaction 2NOCl(g)  2(g) , Kc = 8.0 at a certain temperature. What concentration of NOCl must be put into an empty 4.00 L reaction vessel in order that the equilibrium concentration of NOCl be 1.00 M? A) 1.26 M B) 2.25 M C) 2.50 M D) 3.52 M E) 11.0 M" class="answers-bank-image d-inline" rel="preload" > 2NO(g) + Cl2(g) , Kc = 8.0 at a certain temperature. What concentration of NOCl must be put into an empty 4.00 L reaction vessel in order that the equilibrium concentration of NOCl be 1.00 M?

Accepted Answer

A)  1.26 M
B)  2.25 M
C)  2.50 M
D)  3.52 M
E)  11.0 MF) A) and E)
G) A) and C)

Question 15

Consider this reaction at equilibrium: 2SO2(g) + O2(g)  2(g) + O2(g)    2SO3(g) ,  \Delta Hºrxn = -198 kJ/mol If the volume of the system is compressed at constant temperature, what change will occur in the position of the equilibrium? A) A shift to produce more SO2 B) A shift to produce more O2 C) No change D) A shift to produce more SO3 " class="answers-bank-image d-inline" rel="preload" > 2SO3(g) ,  Δ\DeltaΔ Hºrxn = -198 kJ/mol
If the volume of the system is compressed at constant temperature, what change will occur in the position of the equilibrium?

Accepted Answer

A)  A shift to produce more SO2
B)  A shift to produce more O2
C)  No change
D)  A shift to produce more SO3 E) None of the above
F) All of the above

Question 16

Consider the equilibrium equation C(s)+ H2O(g)+ 2296 J  CO(g)+ H2(g). What will happen to the concentration of carbon monoxide if the temperature of this system is raised?

Accepted Answer

Question 17

For the following reaction at equilibrium in a reaction vessel, which one of these changes would cause the Br2 concentration to decrease? 2NOBr(g)  2 concentration to decrease? 2NOBr(g)    2NO(g) + Br2(g) ,  \Delta Hºrxn= 30 kJ/mol A) Increase the temperature. B) Remove some NO. C) Add more NOBr. D) Compress the gas mixture into a smaller volume. " class="answers-bank-image d-inline" rel="preload" > 2NO(g) + Br2(g) ,  Δ\DeltaΔ Hºrxn= 30 kJ/mol

Accepted Answer

A)  Increase the temperature.
B)  Remove some NO.
C)  Add more NOBr.
D)  Compress the gas mixture into a smaller volume. E) None of the above
F) C) and D)

Question 18

Consider this gas phase equilibrium system: PCl5(g)  5(g)   PCl3(g) + Cl2(g)  \Delta Hºrxn = +87.8 kJ/mol. Which of these statements is false? A) Increasing the system volume shifts the equilibrium to the right. B) Increasing the temperature shifts the equilibrium to the right. C) A catalyst speeds up the approach to equilibrium and shifts the position of equilibrium to the right. D) Decreasing the total pressure of the system shifts the equilibrium to the right. E) Increasing the temperature causes the equilibrium constant to increase. " class="answers-bank-image d-inline" rel="preload" >PCl3(g) + Cl2(g)  Δ\DeltaΔ Hºrxn = +87.8 kJ/mol.
Which of these statements is false?

Accepted Answer

A)  Increasing the system volume shifts the equilibrium to the right.
B)  Increasing the temperature shifts the equilibrium to the right.
C)  A catalyst speeds up the approach to equilibrium and shifts the position of equilibrium to the right.
D)  Decreasing the total pressure of the system shifts the equilibrium to the right.
E)  Increasing the temperature causes the equilibrium constant to increase. F) B) and C)
G) A) and E)

Question 19

Calculate Kp for the reaction 2NOCl(g)  p for the reaction 2NOCl(g)     2NO(g) + Cl2(g) at 400°C if Kc at 400°C for this reaction is 2.1 *10-2. A) 2.1 * 10-2 B) 1.7 * 10-3 C) 0.70 D) 1.2 E) 3.8 * 10-4" class="answers-bank-image d-inline" rel="preload" >  2NO(g) + Cl2(g) at 400°C if Kc at 400°C for this reaction is 2.1 *10-2.

Accepted Answer

A)  2.1 * 10-2
B)  1.7 * 10-3
C)  0.70
D)  1.2
E)  3.8 * 10-4F) All of the above
G) A) and B)

Question 20

Consider the following equilibrium,
4NH3(g)+ 3O2(g)  2N2(g)+ 6H2O(g)+ 1531 kJ
State whether the concentrations of the products would increase, decrease, or remain constant when the temperature is increased.

Accepted Answer

Exam 15: Chemical Equilibrium

Correct Answer
verified

Consider the reaction N₂(g)+ 3H₂(g) 2NH₃(g). If we use a catalyst, which way will the reaction shift?

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Consider the following equilibrium, 4NH₃(g)+ 3O₂(g) 2N₂(g)+ 6H₂O(g)+ 1531 kJ State whether the concentrations of the products would increase, decrease, or remain constant when the temperature is increased.

Correct Answer
verified

Correct Answer
verified

Consider the equilibrium equation C(s)+ H₂O(g)+ 2296 J CO(g)+ H₂(g). What will happen to the concentration of carbon monoxide if the temperature of this system is raised?

Correct Answer
verified

Calculate K_c for the reaction 2HI(g) H₂(g) + I₂(g) given that the concentrations of each species at equilibrium are as follows: [HI] = 0.85 mol/L, [I₂] = 0.60 mol/L, [H₂] = 0.27 mol/L.

Correct Answer
verified

For the reaction 2NOCl(g) 2NO(g) + Cl₂(g) , K_c = 8.0 at a certain temperature. What concentration of NOCl must be put into an empty 4.00 L reaction vessel in order that the equilibrium concentration of NOCl be 1.00 M?

Correct Answer
verified

For the reaction PCl₃(g) + Cl₂(g) PCl₅(g) at a particular temperature, K_c = 24.3. Suppose a system at that temperature is prepared with [PCl₃] = 0.10 M, [Cl₂] = 0.15 M, and [PCl₅] = 0.60 M. Which of these statements is true?

Correct Answer
verified

If the reaction 2H₂S(g) 2H₂(g) + S₂(g) is carried out at 1065°C, K_p = 0.0120. Starting from pure H₂S introduced into an evacuated vessel at 1065°C, what will the total pressure in the vessel be at equilibrium if the equilibrated mixture contains 0.300 atm of H₂(g) ?

Correct Answer
verified

Correct Answer
verified

The dissociation of solid silver chloride in water to produce silver ions and chloride ions has an equilibrium constant of 1.8 * 10^-18. Based on the magnitude of the equilibrium constant, is silver chloride very soluble in water? Why?

Correct Answer
verified
K_c here will be [Ag^{+View Answer}

Equilibrium is established for the reaction 2X(s) + Y(g) $\rarr$ 2Z(g) at 500K, K_c = 100. Determine the concentration of Z in equilibrium with 0.2 mol X and 0.50 M Y at 500K.

Correct Answer
verified

Calculate K_p for the reaction 2NOCl(g) 2NO(g) + Cl₂(g) at 400°C if K_c at 400°C for this reaction is 2.1 *10^-2.

Correct Answer
verified

The reaction 2SO₃(g) 2SO₂(g) + O₂(g) is endothermic. If the temperature is increased,

Correct Answer
verified

Hydrogen iodide decomposes according to the equation 2HI(g) H₂(g) + I₂(g) , for which K_c = 0.0156 at 400ºC. 0.550 mol HI was injected into a 2.00 L reaction vessel at 400ºC. Calculate the concentration of HI at equilibrium.

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Phosgene, COCl₂, a poisonous gas, decomposes according to the equation COCl₂(g) CO(g) + Cl₂(g) . Calculate K_p for this reaction if K_c = 0.083 at 900ºC.

Correct Answer
verified

Exam 15: Chemical Equilibrium

Equilibrium constants are known for the following reactions: S(s)+ 3/2O2(g) SO3(g)Kc = 9.2 * 1023 SO3(g) SO2(g)+ 1/2O2(g)Kc = 4.8 * 10- 4 Thus, for the reaction S(s)+ O2(g) →\rarr→ SO2(g), Kc = 4.4 * 1020.

Correct AnswerverifiedShow Answer

Consider the reaction N2(g)+ 3H2(g) 2NH3(g). If we use a catalyst, which way will the reaction shift?

Correct AnswerverifiedShow Answer

Consider this reaction at equilibrium: 2SO2(g) + O2(g) 2SO3(g) , Δ\DeltaΔ Hºrxn = -198 kJ/mol If the volume of the system is compressed at constant temperature, what change will occur in the position of the equilibrium?

Correct AnswerverifiedShow Answer

For the following reaction at equilibrium in a reaction vessel, which one of these changes would cause the Br2 concentration to decrease? 2NOBr(g) 2NO(g) + Br2(g) , Δ\DeltaΔ Hºrxn= 30 kJ/mol

Correct AnswerverifiedShow Answer

Consider the following equilibrium, 4NH3(g)+ 3O2(g) 2N2(g)+ 6H2O(g)+ 1531 kJ State whether the concentrations of the products would increase, decrease, or remain constant when the temperature is increased.

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

Consider the equilibrium equation C(s)+ H2O(g)+ 2296 J CO(g)+ H2(g). What will happen to the concentration of carbon monoxide if the temperature of this system is raised?

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Calculate Kc for the reaction 2HI(g) H2(g) + I2(g) given that the concentrations of each species at equilibrium are as follows: [HI] = 0.85 mol/L, [I2] = 0.60 mol/L, [H2] = 0.27 mol/L.

Correct AnswerverifiedShow Answer

For the reaction 2NOCl(g) 2NO(g) + Cl2(g) , Kc = 8.0 at a certain temperature. What concentration of NOCl must be put into an empty 4.00 L reaction vessel in order that the equilibrium concentration of NOCl be 1.00 M?

Correct AnswerverifiedShow Answer

For the reaction PCl3(g) + Cl2(g) PCl5(g) at a particular temperature, Kc = 24.3. Suppose a system at that temperature is prepared with [PCl3] = 0.10 M, [Cl2] = 0.15 M, and [PCl5] = 0.60 M. Which of these statements is true?

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If the reaction 2H2S(g) 2H2(g) + S2(g) is carried out at 1065°C, Kp = 0.0120. Starting from pure H2S introduced into an evacuated vessel at 1065°C, what will the total pressure in the vessel be at equilibrium if the equilibrated mixture contains 0.300 atm of H2(g) ?

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The equilibrium constant for the reaction Ni(s) + 4CO(g) →\rarr→ Ni(CO) 4(g) is 5.0 * 104 at 25ºC. What is the equilibrium constant for the reaction Ni(CO) 4(g) Ni(s) + 4CO(g) ?

Correct AnswerverifiedShow Answer

The dissociation of solid silver chloride in water to produce silver ions and chloride ions has an equilibrium constant of 1.8 * 10-18. Based on the magnitude of the equilibrium constant, is silver chloride very soluble in water? Why?

Correct AnswerverifiedKc here will be [Ag+View AnswerShow Answer

Equilibrium is established for the reaction 2X(s) + Y(g) →\rarr→ 2Z(g) at 500K, Kc = 100. Determine the concentration of Z in equilibrium with 0.2 mol X and 0.50 M Y at 500K.

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Calculate Kp for the reaction 2NOCl(g) 2NO(g) + Cl2(g) at 400°C if Kc at 400°C for this reaction is 2.1 *10-2.

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The reaction 2SO3(g) 2SO2(g) + O2(g) is endothermic. If the temperature is increased,

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Hydrogen iodide decomposes according to the equation 2HI(g) H2(g) + I2(g) , for which Kc = 0.0156 at 400ºC. 0.550 mol HI was injected into a 2.00 L reaction vessel at 400ºC. Calculate the concentration of HI at equilibrium.

Correct AnswerverifiedShow Answer

The brown gas NO2 and the colorless gas N2O4 exist in equilibrium, 2NO2 N2O4. In an experiment, 0.625 mole of N2O4 was introduced into a 5.00 L vessel and was allowed to decompose until equilibrium was reached. The concentration of N2O4 at equilibrium was 0.0750 M. Calculate Kc for the reaction.

Correct AnswerverifiedShow Answer

Consider this gas phase equilibrium system: PCl5(g) PCl3(g) + Cl2(g) Δ\DeltaΔ Hºrxn = +87.8 kJ/mol. Which of these statements is false?

Correct AnswerverifiedShow Answer

Phosgene, COCl2, a poisonous gas, decomposes according to the equation COCl2(g) CO(g) + Cl2(g) . Calculate Kp for this reaction if Kc = 0.083 at 900ºC.

Correct AnswerverifiedShow Answer

Correct Answer
verified

Consider the reaction N₂(g)+ 3H₂(g) 2NH₃(g). If we use a catalyst, which way will the reaction shift?

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Consider the following equilibrium, 4NH₃(g)+ 3O₂(g) 2N₂(g)+ 6H₂O(g)+ 1531 kJ State whether the concentrations of the products would increase, decrease, or remain constant when the temperature is increased.

Correct Answer
verified

Correct Answer
verified

Consider the equilibrium equation C(s)+ H₂O(g)+ 2296 J CO(g)+ H₂(g). What will happen to the concentration of carbon monoxide if the temperature of this system is raised?

Correct Answer
verified

Calculate K_c for the reaction 2HI(g) H₂(g) + I₂(g) given that the concentrations of each species at equilibrium are as follows: [HI] = 0.85 mol/L, [I₂] = 0.60 mol/L, [H₂] = 0.27 mol/L.

Correct Answer
verified

For the reaction 2NOCl(g) 2NO(g) + Cl₂(g) , K_c = 8.0 at a certain temperature. What concentration of NOCl must be put into an empty 4.00 L reaction vessel in order that the equilibrium concentration of NOCl be 1.00 M?

Correct Answer
verified

For the reaction PCl₃(g) + Cl₂(g) PCl₅(g) at a particular temperature, K_c = 24.3. Suppose a system at that temperature is prepared with [PCl₃] = 0.10 M, [Cl₂] = 0.15 M, and [PCl₅] = 0.60 M. Which of these statements is true?

Correct Answer
verified

If the reaction 2H₂S(g) 2H₂(g) + S₂(g) is carried out at 1065°C, K_p = 0.0120. Starting from pure H₂S introduced into an evacuated vessel at 1065°C, what will the total pressure in the vessel be at equilibrium if the equilibrated mixture contains 0.300 atm of H₂(g) ?

Correct Answer
verified

Correct Answer
verified

The dissociation of solid silver chloride in water to produce silver ions and chloride ions has an equilibrium constant of 1.8 * 10^-18. Based on the magnitude of the equilibrium constant, is silver chloride very soluble in water? Why?

Correct Answer
verified
K_c here will be [Ag^{+View Answer}

Equilibrium is established for the reaction 2X(s) + Y(g) $\rarr$ 2Z(g) at 500K, K_c = 100. Determine the concentration of Z in equilibrium with 0.2 mol X and 0.50 M Y at 500K.

Correct Answer
verified

Calculate K_p for the reaction 2NOCl(g) 2NO(g) + Cl₂(g) at 400°C if K_c at 400°C for this reaction is 2.1 *10^-2.

Correct Answer
verified

The reaction 2SO₃(g) 2SO₂(g) + O₂(g) is endothermic. If the temperature is increased,

Correct Answer
verified

Hydrogen iodide decomposes according to the equation 2HI(g) H₂(g) + I₂(g) , for which K_c = 0.0156 at 400ºC. 0.550 mol HI was injected into a 2.00 L reaction vessel at 400ºC. Calculate the concentration of HI at equilibrium.

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Phosgene, COCl₂, a poisonous gas, decomposes according to the equation COCl₂(g) CO(g) + Cl₂(g) . Calculate K_p for this reaction if K_c = 0.083 at 900ºC.

Correct Answer
verified