Question 1

The molar solubility of SrF2 in water is 8.8×10 - 4 M. What is the solubility product constant, K sp, for this substance?

Accepted Answer

A)   K sp = 6.81×10 - 10
B)   K sp = 2.73×10 - 9
C)   K sp = 7.74×10 - 7
D)   K sp = 1.55×10 - 6
E)   K sp = 2.64×10 - 3

Question 2

A simplifying assumption can be made when solving problems in equilibrium which assumes that "x" is considerably small (approaches zero)  in the sum or difference of an expression. As such, it drops out of the expression and the Algebra becomes much easier. When is it valid to use a simplifying assumption?

Accepted Answer

A)   It is valid to make this assumption when the ratio: "x"/[reactant A]o * 100% > 5%
B)   It is valid to make this assumption when 95 out of 100 scientists chose to do so.
C)   It is valid to make this assumption when "x" is comparable in magnitude to the initial concentration of the reactant A. (i.e., x ~ [A]o) 
D)   It is valid to make this assumption when the ratio: "x"/[reactant A]o 
E)   It is valid to make this assumption when the ratio: "x"/[reactant A]o * 100% < 5%

Question 3

The equilibrium constant for the reaction below is 1.7*1017 at 25 C.
H₂ (g)  + Br₂(g)  17 at 25 C. H₂ (g)  + Br₂(g)    2 HBr (g)  K c (25 C)  = 1.7*1017  What can be stated about the relative equilibrium distribution for this mixture? A)  The mixture contains predominantly H2 at equilibrium. B)  The mixture contains predominantly Br2 at equilibrium. C)  The mixture contains predominantly HBr at equilibrium. D)  The mixture contains predominantly H2 and Br2 at equilibrium. E)  The mixture contains relatively equal amounts of H2, Br2 and HBr at equilibrium." class="answers-bank-image d-inline" rel="preload" > 2 HBr (g)  K c (25 C)  = 1.7*1017 
What can be stated about the relative equilibrium distribution for this mixture?

Accepted Answer

A)   The mixture contains predominantly H2 at equilibrium.
B)   The mixture contains predominantly Br2 at equilibrium.
C)   The mixture contains predominantly HBr at equilibrium.
D)   The mixture contains predominantly H2 and Br2 at equilibrium.
E)   The mixture contains relatively equal amounts of H2, Br2 and HBr at equilibrium.

Question 4

What is the molar solubility of Ag2SO4 in the presence of 0.22 M aqueous solution of AgNO3?
K sp(Ag2SO4)  = 1.5×10 - 5

Accepted Answer

A)   [Ag2SO4] = 7.8×10 - 5 M
B)   [Ag2SO4] = 1.6×10 - 4 M
C)   [Ag2SO4] = 3.1×10 - 4 M
D)   [Ag2SO4] = 6.1×10 - 4 M
E)   [Ag2SO4] = 1.6×10 - 2 M

Question 5

At a certain temperature K c = 9.0 for the equilibrium N₂O4 (g)  4 (g)    2 NO₂ . What is K c at the same temperature for: NO₂ (g)    1 / 2 N₂O4 (g)  A)  1.1 B)  3.0 C)  0.33 D)  9.0 E)  none of these" class="answers-bank-image d-inline" rel="preload" > 2 NO₂ . What is K c at the same temperature for:
NO₂ (g)  4 (g)    2 NO₂ . What is K c at the same temperature for: NO₂ (g)    1 / 2 N₂O4 (g)  A)  1.1 B)  3.0 C)  0.33 D)  9.0 E)  none of these" class="answers-bank-image d-inline" rel="preload" > 1 / 2 N₂O4 (g)

Accepted Answer

A)   1.1
B)   3.0
C)   0.33
D)   9.0
E)   none of these

Question 6

K c = 0.35 for the reaction:
H₂ (g)  + I2 (g)  2 (g)    2 HI (g)  If one mole of H₂ and one mole of I2 are placed in a 1.0 liter container, the equilibrium concentration of HI is: A)  0.46 M B)  0.77 M C)  0.23 M D)  0.63 M E)  0.30 M" class="answers-bank-image d-inline" rel="preload" > 2 HI (g) 
If one mole of H₂ and one mole of I2 are placed in a 1.0 liter container, the equilibrium concentration of HI is:

Accepted Answer

A)   0.46 M
B)   0.77 M
C)   0.23 M
D)   0.63 M
E)   0.30 M

Question 7

At 25 C, K p = 0.240 for the reaction:
2 ICl (g)  2 (g)  + Cl₂ (g)  If 2.66 atm of ICl are placed in a 1.0 L flask, what is the equilibrium pressure of I2 ? A)  0.658 atm B)  1.52 atm C)  8.33 atm D)  0.585 atm E)  0.24 atm" class="answers-bank-image d-inline" rel="preload" > I2 (g)  + Cl₂ (g) 
If 2.66 atm of ICl are placed in a 1.0 L flask, what is the equilibrium pressure of I2 ?

Accepted Answer

A)   0.658 atm
B)   1.52 atm
C)   8.33 atm
D)   0.585 atm
E)   0.24 atm

Question 8

Consider the following system at equilibrium. A reaction vessel is charged witH₂ .46 atm of NO, 2.46 atm of H₂ O and 1.23 atm of H₂ gases. Equilibrium is established as shown in the reaction below. 2 NO (g)  + 2 H₂ (g)   N₂(g)  + 2 H₂ O (g)  At equilibrium, the partial pressure of NO is 1.53 atm. What is the equilibrium partial pressure of N₂gas in this mixture?

Accepted Answer

A)   0.00 atm
B)   0.465 atm
C)   0.765 atm
D)   0.930 atm
E)   1.86 atm

Question 9

The K sp for PbBr2 is 4.0×10 - 5 at a particular temperature. What is the solubility of PbBr2 in pure water?

Accepted Answer

A)   6.3×10 - 3 M
B)   2.2×10 - 2 M
C)   3.4×10 - 2 M
D)   4.0×10 - 5 M
E)   3.2×10 - 3 M

Question 10

In water saturated with BaF2 at a particular temperature, the equilibrium concentration of fluoride ions is 1.5×10 - 2 M . What is the K sp of barium fluoride?

Accepted Answer

A)   1.7×10 - 6
B)   2.2×10 - 4
C)   9.0×10 - 4
D)   3.4×10 - 6
E)   4.6×10 - 10

Question 11

When the reversible reaction, N₂+ O₂  2 NO
Has reached a state of dynamic equilibrium , which statement(s)  below is(are)  true?
I. Both the forward and reverse reactions shut down and no more NO, N₂or O₂are produced.
II. The rate of the forward reaction equals the rate of the reverse reaction.
III. The rate constant of the forward reaction equals the rate constant of the reverse reaction.

Accepted Answer

A)   I only
B)   II only
C)   III only
D)   I and II
E)   All of these.

Question 12

What is the equilibrium constant expression for the following equation at equilibrium?
(Pay careful attention to the phase indicators!)  2 HCl (g)  + Mg(OH) 2(s)  2(s)    MgCl₂ (aq)  + 2 H₂ O (   )  A)    B)    C)    D)    E)   " class="answers-bank-image d-inline" rel="preload" > MgCl₂ (aq)  + 2 H₂ O ( 2(s)    MgCl₂ (aq)  + 2 H₂ O (   )  A)    B)    C)    D)    E)   " class="answers-bank-image d-inline" rel="preload" > )

Accepted Answer

A)   2(s)    MgCl₂ (aq)  + 2 H₂ O (   )  
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
B)   2(s)    MgCl₂ (aq)  + 2 H₂ O (   )  
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
C)   2(s)    MgCl₂ (aq)  + 2 H₂ O (   )  
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
D)   2(s)    MgCl₂ (aq)  + 2 H₂ O (   )  
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
E)   2(s)    MgCl₂ (aq)  + 2 H₂ O (   )  
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >

Question 13

What is the effect upon addition of Argon (an inert gas)  to the equilibrium reaction shown below?
N₂O4 (g)  4 (g)    2 NO₂ (g)  A)  No effect B)  The reaction shifts to the right. C)  The reaction shifts to the left. D)  More information is needed." class="answers-bank-image d-inline" rel="preload" > 2 NO₂ (g)

Accepted Answer

A)   No effect
B)   The reaction shifts to the right.
C)   The reaction shifts to the left.
D)   More information is needed.

Question 14

Which of the following reactions is product favored by a higher temperature ?
I. N₂(g)  + 2 O₂+ Heat 4 (g)  + 3 O₂(g)    2 CO₂ (g)  + 2 H₂ O (g)  ( D H 0)  A)  I only B)  II only C)  III only D)  I and II E)  I and III " class="answers-bank-image d-inline" rel="preload" > 2 NO₂ (g) 
II. 2 N₂(g)  + 6 H₂ O (g)  4 (g)  + 3 O₂(g)    2 CO₂ (g)  + 2 H₂ O (g)  ( D H 0)  A)  I only B)  II only C)  III only D)  I and II E)  I and III " class="answers-bank-image d-inline" rel="preload" > 4 NH₃(g)  + 3 O₂(g)  (endothermic reaction) 
III. C₂ H4 (g)  + 3 O₂(g)  4 (g)  + 3 O₂(g)    2 CO₂ (g)  + 2 H₂ O (g)  ( D H 0)  A)  I only B)  II only C)  III only D)  I and II E)  I and III " class="answers-bank-image d-inline" rel="preload" > 2 CO₂ (g)  + 2 H₂ O (g)  ( D H 0)

Accepted Answer

A)   I only
B)   II only
C)   III only
D)   I and II
E)   I and III

Question 15

A solution is prepared such that the concentrations of the ions F - , Cl - , Br - , and I -  are all 0.0010 M . Solid Pb(NO3) 2 is added to the solution. Which insoluble lead salt precipitates last?
PbF2 K sp = 3.7×10 - 8 PbCl2 K  sp = 1.7×10 - 5 PbBr2 K sp = 6.3×10 - 6 PbI2 K sp = 8.7×10 - 9

Accepted Answer

A)   PbI2
B)   PbBr2
C)   PbCl2
D)   PbF2
E)   impossible to determine

Question 16

Which ionic compound(s)  listed below would increase in solubility upon lowering the pH?
I. CaF2
II. Ni(OH) 2
III. PbCl2

Accepted Answer

A)   I only
B)   II only
C)   III only
D)   I and II
E)   All of these

Question 17

What is the partial pressure equilibrium constant, K p , for the following reaction if the concentration equilibrium constant K c = 7.17*1015 at 200 K?
N₂(g)  + 3 H₂ (g)  15 at 200 K? N₂(g)  + 3 H₂ (g)    2 NH₃(g)  A)  K p = 7.21×10 - 35 B)  K p = 2.66×1013 C)  K p = 4.37×1014 D)  K p = 1.18×1017 E)  K p = 1.93×1018" class="answers-bank-image d-inline" rel="preload" > 2 NH₃(g)

Accepted Answer

A)   K p = 7.21×10 - 35
B)   K p = 2.66×1013
C)   K p = 4.37×1014
D)   K p = 1.18×1017
E)   K p = 1.93×1018

Question 18

The reaction 2 NaHSO₄(s)  2 S2O 7 (s)  + H₂ O (g)  is endothermic at 298 K. Therefore, A)  D H ° rxn is positive. B)  The partial pressure of H2O would be higher at 500K. C)  K p would increase with increasing temperature. D)  All of a, b, and c are correct. E)  None of a, b, and c are correct." class="answers-bank-image d-inline" rel="preload" > Na2 S2O 7 (s)  + H₂ O (g)  is endothermic at 298 K. Therefore,

Accepted Answer

A)   D H ° rxn is positive.
B)   The partial pressure of H2O would be higher at 500K.
C)   K p would increase with increasing temperature.
D)   All of a, b, and c are correct.
E)   None of a, b, and c are correct.

Question 19

The equilibrium governed by the reaction 4 NH₃(g)  + 5 O₂(g)  2O decreases. B)  The number of moles of NO remains the same. C)  The number of moles of NH3 decreases. D)  The value of K c increases. E)  The number of moles of both H2O and O2 decrease." class="answers-bank-image d-inline" rel="preload" > 4 NO (g)  + 6 H₂ O (g)  undergoes a change in volume from 1.0 L to 2.0 L at 600 C. Choose the correct statement below.

Accepted Answer

A)   The number of moles of H2O decreases.
B)   The number of moles of NO remains the same.
C)   The number of moles of NH3 decreases.
D)   The value of K c increases.
E)   The number of moles of both H2O and O2 decrease.

Question 20

One mole of SO₂ , two moles of O₂, and two moles of SO3 are placed in a 1.0 liter flask. If K c for the reaction 2 SO₂ (g)  + O₂(g)  3 are placed in a 1.0 liter flask. If K c for the reaction 2 SO₂ (g)  + O₂(g)    2 SO3(g)  is 0.50 at this temperature, what occurs in the flask as equilibrium is approached? A)  [SO3] increases B)  [O2] increases C)  [SO2] decreases D)  No reaction occurs since the system is at equilibrium. E)  The equilibrium concentrations of [O2] and [SO2] are very small." class="answers-bank-image d-inline" rel="preload" > 2 SO3(g)  is 0.50 at this temperature, what occurs in the flask as equilibrium is approached?

Accepted Answer

A)   [SO3] increases
B)   [O2] increases
C)   [SO2] decreases
D)   No reaction occurs since the system is at equilibrium.
E)   The equilibrium concentrations of [O2] and [SO2] are very small.

Exam 14: Chemical Equilibrium

What is the equilibrium constant expression for the following equation at equilibrium? (Pay careful attention to the phase indicators!) 2 HCl (g) + Mg(OH) ₂(s) MgCl₂ (aq) + 2 H₂ O ( )

Correct Answer
verified

The molar solubility of SrF₂ in water is 8.8×10^{- 4} M. What is the solubility product constant, K _sp, for this substance?

Correct Answer
verified

At 25 C, K p = 0.240 for the reaction: 2 ICl (g) I₂ (g) + Cl₂ (g) If 2.66 atm of ICl are placed in a 1.0 L flask, what is the equilibrium pressure of I₂ ?

Correct Answer
verified

What is the molar solubility of Ag₂SO₄ in the presence of 0.22 M aqueous solution of AgNO₃? K _sp(Ag₂SO₄) = 1.5×10^{- 5}

Correct Answer
verified

Correct Answer
verified

What is the effect upon addition of Argon (an inert gas) to the equilibrium reaction shown below? N₂O₄ (g) 2 NO₂ (g)

Correct Answer
verified

Which of the following reactions is product favored by a higher temperature ? I. N₂(g) + 2 O₂+ Heat 2 NO₂ (g) II. 2 N₂(g) + 6 H₂ O (g) 4 NH₃(g) + 3 O₂(g) (endothermic reaction) III. C₂ H₄ (g) + 3 O₂(g) 2 CO₂ (g) + 2 H₂ O (g) ( D H 0)

Correct Answer
verified

What is the partial pressure equilibrium constant, K p , for the following reaction if the concentration equilibrium constant K c = 7.17*10¹⁵ at 200 K? N₂(g) + 3 H₂ (g) 2 NH₃(g)

Correct Answer
verified

The equilibrium governed by the reaction 4 NH₃(g) + 5 O₂(g) 4 NO (g) + 6 H₂ O (g) undergoes a change in volume from 1.0 L to 2.0 L at 600 C. Choose the correct statement below.

Correct Answer
verified

Correct Answer
verified

Which ionic compound(s) listed below would increase in solubility upon lowering the pH? I. CaF₂ II. Ni(OH) ₂ III. PbCl₂

Correct Answer
verified

One mole of SO₂ , two moles of O₂, and two moles of SO₃ are placed in a 1.0 liter flask. If K c for the reaction 2 SO₂ (g) + O₂(g) 2 SO₃(g) is 0.50 at this temperature, what occurs in the flask as equilibrium is approached?

Correct Answer
verified

Correct Answer
verified

In water saturated with BaF₂ at a particular temperature, the equilibrium concentration of fluoride ions is 1.5×10^{- 2} M . What is the K _sp of barium fluoride?

Correct Answer
verified

The reaction 2 NaHSO₄(s) Na₂ S₂O 7 (s) + H₂ O (g) is endothermic at 298 K. Therefore,

Correct Answer
verified

K c = 0.35 for the reaction: H₂ (g) + I₂ (g) 2 HI (g) If one mole of H₂ and one mole of I₂ are placed in a 1.0 liter container, the equilibrium concentration of HI is:

Correct Answer
verified

The equilibrium constant for the reaction below is 1.710¹⁷ at 25 C. H₂ (g) + Br₂(g) 2 HBr (g) K c (25 C) = 1.710¹⁷ What can be stated about the relative equilibrium distribution for this mixture?

Correct Answer
verified

At a certain temperature K c = 9.0 for the equilibrium N₂O₄ (g) 2 NO₂ . What is K c at the same temperature for: NO₂ (g) 1 / 2 N₂O₄ (g)

Correct Answer
verified

Correct Answer
verified

The K _sp for PbBr₂ is 4.0×10^{- 5} at a particular temperature. What is the solubility of PbBr₂ in pure water?

Correct Answer
verified

Exam 14: Chemical Equilibrium

What is the equilibrium constant expression for the following equation at equilibrium? (Pay careful attention to the phase indicators!) 2 HCl (g) + Mg(OH) 2(s) MgCl₂ (aq) + 2 H₂ O ( )

Correct AnswerverifiedShow Answer

The molar solubility of SrF2 in water is 8.8×10 - 4 M. What is the solubility product constant, K sp, for this substance?

Correct AnswerverifiedShow Answer

At 25 C, K p = 0.240 for the reaction: 2 ICl (g) I2 (g) + Cl₂ (g) If 2.66 atm of ICl are placed in a 1.0 L flask, what is the equilibrium pressure of I2 ?

Correct AnswerverifiedShow Answer

What is the molar solubility of Ag2SO4 in the presence of 0.22 M aqueous solution of AgNO3? K sp(Ag2SO4) = 1.5×10 - 5

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

What is the effect upon addition of Argon (an inert gas) to the equilibrium reaction shown below? N₂O4 (g) 2 NO₂ (g)

Correct AnswerverifiedShow Answer

Which of the following reactions is product favored by a higher temperature ? I. N₂(g) + 2 O₂+ Heat 2 NO₂ (g) II. 2 N₂(g) + 6 H₂ O (g) 4 NH₃(g) + 3 O₂(g) (endothermic reaction) III. C₂ H4 (g) + 3 O₂(g) 2 CO₂ (g) + 2 H₂ O (g) ( D H 0)

Correct AnswerverifiedShow Answer

What is the partial pressure equilibrium constant, K p , for the following reaction if the concentration equilibrium constant K c = 7.17*1015 at 200 K? N₂(g) + 3 H₂ (g) 2 NH₃(g)

Correct AnswerverifiedShow Answer

The equilibrium governed by the reaction 4 NH₃(g) + 5 O₂(g) 4 NO (g) + 6 H₂ O (g) undergoes a change in volume from 1.0 L to 2.0 L at 600 C. Choose the correct statement below.

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

Which ionic compound(s) listed below would increase in solubility upon lowering the pH? I. CaF2 II. Ni(OH) 2 III. PbCl2

Correct AnswerverifiedShow Answer

One mole of SO₂ , two moles of O₂, and two moles of SO3 are placed in a 1.0 liter flask. If K c for the reaction 2 SO₂ (g) + O₂(g) 2 SO3(g) is 0.50 at this temperature, what occurs in the flask as equilibrium is approached?

Correct AnswerverifiedShow Answer

A solution is prepared such that the concentrations of the ions F - , Cl - , Br - , and I - are all 0.0010 M . Solid Pb(NO3) 2 is added to the solution. Which insoluble lead salt precipitates last? PbF2 K sp = 3.7×10 - 8 PbCl2 K sp = 1.7×10 - 5 PbBr2 K sp = 6.3×10 - 6 PbI2 K sp = 8.7×10 - 9

Correct AnswerverifiedShow Answer

In water saturated with BaF2 at a particular temperature, the equilibrium concentration of fluoride ions is 1.5×10 - 2 M . What is the K sp of barium fluoride?

Correct AnswerverifiedShow Answer

The reaction 2 NaHSO₄(s) Na2 S2O 7 (s) + H₂ O (g) is endothermic at 298 K. Therefore,

Correct AnswerverifiedShow Answer

K c = 0.35 for the reaction: H₂ (g) + I2 (g) 2 HI (g) If one mole of H₂ and one mole of I2 are placed in a 1.0 liter container, the equilibrium concentration of HI is:

Correct AnswerverifiedShow Answer

The equilibrium constant for the reaction below is 1.7*1017 at 25 C. H₂ (g) + Br₂(g) 2 HBr (g) K c (25 C) = 1.7*1017 What can be stated about the relative equilibrium distribution for this mixture?

Correct AnswerverifiedShow Answer

At a certain temperature K c = 9.0 for the equilibrium N₂O4 (g) 2 NO₂ . What is K c at the same temperature for: NO₂ (g) 1 / 2 N₂O4 (g)

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

The K sp for PbBr2 is 4.0×10 - 5 at a particular temperature. What is the solubility of PbBr2 in pure water?

Correct AnswerverifiedShow Answer

What is the equilibrium constant expression for the following equation at equilibrium? (Pay careful attention to the phase indicators!) 2 HCl (g) + Mg(OH) ₂(s) MgCl₂ (aq) + 2 H₂ O ( )

Correct Answer
verified

The molar solubility of SrF₂ in water is 8.8×10^{- 4} M. What is the solubility product constant, K _sp, for this substance?

Correct Answer
verified

At 25 C, K p = 0.240 for the reaction: 2 ICl (g) I₂ (g) + Cl₂ (g) If 2.66 atm of ICl are placed in a 1.0 L flask, what is the equilibrium pressure of I₂ ?

Correct Answer
verified

What is the molar solubility of Ag₂SO₄ in the presence of 0.22 M aqueous solution of AgNO₃? K _sp(Ag₂SO₄) = 1.5×10^{- 5}

Correct Answer
verified

Correct Answer
verified

What is the effect upon addition of Argon (an inert gas) to the equilibrium reaction shown below? N₂O₄ (g) 2 NO₂ (g)

Correct Answer
verified

Which of the following reactions is product favored by a higher temperature ? I. N₂(g) + 2 O₂+ Heat 2 NO₂ (g) II. 2 N₂(g) + 6 H₂ O (g) 4 NH₃(g) + 3 O₂(g) (endothermic reaction) III. C₂ H₄ (g) + 3 O₂(g) 2 CO₂ (g) + 2 H₂ O (g) ( D H 0)

Correct Answer
verified

What is the partial pressure equilibrium constant, K p , for the following reaction if the concentration equilibrium constant K c = 7.17*10¹⁵ at 200 K? N₂(g) + 3 H₂ (g) 2 NH₃(g)

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Which ionic compound(s) listed below would increase in solubility upon lowering the pH? I. CaF₂ II. Ni(OH) ₂ III. PbCl₂

Correct Answer
verified

One mole of SO₂ , two moles of O₂, and two moles of SO₃ are placed in a 1.0 liter flask. If K c for the reaction 2 SO₂ (g) + O₂(g) 2 SO₃(g) is 0.50 at this temperature, what occurs in the flask as equilibrium is approached?

Correct Answer
verified

Correct Answer
verified

In water saturated with BaF₂ at a particular temperature, the equilibrium concentration of fluoride ions is 1.5×10^{- 2} M . What is the K _sp of barium fluoride?

Correct Answer
verified

The reaction 2 NaHSO₄(s) Na₂ S₂O 7 (s) + H₂ O (g) is endothermic at 298 K. Therefore,

Correct Answer
verified

K c = 0.35 for the reaction: H₂ (g) + I₂ (g) 2 HI (g) If one mole of H₂ and one mole of I₂ are placed in a 1.0 liter container, the equilibrium concentration of HI is:

Correct Answer
verified

The equilibrium constant for the reaction below is 1.710¹⁷ at 25 C. H₂ (g) + Br₂(g) 2 HBr (g) K c (25 C) = 1.710¹⁷ What can be stated about the relative equilibrium distribution for this mixture?

Correct Answer
verified

At a certain temperature K c = 9.0 for the equilibrium N₂O₄ (g) 2 NO₂ . What is K c at the same temperature for: NO₂ (g) 1 / 2 N₂O₄ (g)

Correct Answer
verified

Correct Answer
verified

The K _sp for PbBr₂ is 4.0×10^{- 5} at a particular temperature. What is the solubility of PbBr₂ in pure water?

Correct Answer
verified