Question 1

At 700 C, the equilibrium constant ( K c )  for the reaction
N₂(g)  + 3 H₂ (g)  c. C)  the value of Q is equal to K c. D)  the reaction is at equilibrium. E)  the value of Q is less than K c." class="answers-bank-image d-inline" rel="preload" > 2 NH₃(g)  is 2.37 10 - 3 .
If 0.683 mol of N₂, 8.80 mol of H₂ and 0.744 mole of NH₃are mixed in a 1.00 L container at 700 C:

Accepted Answer

A)   the value of Q is unknown.
B)   the value of Q is greater than K c.
C)   the value of Q is equal to K c.
D)   the reaction is at equilibrium.
E)   the value of Q is less than K c.

Question 2

At 1073 K, the pressure of CO₂ is 0.236 atm when produced by the reaction:
CaCO3(s)  3(s)    CaO (s)  + CO₂ (g)  The value of K c for this reaction at 1073 K is (R = 0.0821 L atm/(mol K) ) : A)  0.236 B)  3.59×10 - 3 C)  2.65×10 - 5 D)  2.68×10 - 3 E)  3.55×10 - 5" class="answers-bank-image d-inline" rel="preload" > CaO (s)  + CO₂ (g)  The value of K c for this reaction at 1073 K is (R = 0.0821 L atm/(mol K) ) :

Accepted Answer

A)   0.236
B)   3.59×10 - 3
C)   2.65×10 - 5
D)   2.68×10 - 3
E)   3.55×10 - 5

Question 3

What is the equilibrium constant expression for the following unbalanced equation at equilibrium?
(Pay careful attention to the phase indicators!)  Na2 O₂(s)  + CO₂ (g)  2 O₂(s)  + CO₂ (g)    Na2 CO3(s)  + O₂(g)  A)    B)    C)    D)    E)   " class="answers-bank-image d-inline" rel="preload" > Na2 CO3(s)  + O₂(g)

Accepted Answer

A)   2 O₂(s)  + CO₂ (g)    Na2 CO3(s)  + O₂(g)  
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
B)   2 O₂(s)  + CO₂ (g)    Na2 CO3(s)  + O₂(g)  
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
C)   2 O₂(s)  + CO₂ (g)    Na2 CO3(s)  + O₂(g)  
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
D)   2 O₂(s)  + CO₂ (g)    Na2 CO3(s)  + O₂(g)  
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
E)   2 O₂(s)  + CO₂ (g)    Na2 CO3(s)  + O₂(g)  
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >

Question 4

Consider solving for the molar solubility of a 1:3 electrolyte such as Al(OH) 3. After constructing an ICE table and writing a solubility constant expression for this process, what solubility product expression listed below would be suitable for solving for "x" which could then be directly related to the solubility of Al(OH) 3 in water?

Accepted Answer

A)   K sp = 3x3
B)   K sp = 27x3
C)   K sp = x4
D)   K sp = 3x4
E)   K sp = 27x4

Question 5

Given:
2 Cl₂ (g)  + 2 H₂ O (g)   - 3 B)  0.0376 C)  0.0752 D)  0.150 E)  0.274" class="answers-bank-image d-inline" rel="preload" > 4 HCl (g)  + O₂(g)  K c (480 C)  = 0.0752 What would be the equilibrium constant, K c , for the equation that follows?
Cl₂ (g)  + H₂ O (g)   - 3 B)  0.0376 C)  0.0752 D)  0.150 E)  0.274" class="answers-bank-image d-inline" rel="preload" > 2 HCl (g)  + 1 / 2 O₂(g)  K c (480 C)  = ??

Accepted Answer

A)   5.66×10 - 3
B)   0.0376
C)   0.0752
D)   0.150
E)   0.274

Question 6

Consider the following reaction at 1200 K:
CH4 (g)  + H₂ O (g)  4 (g)  + H₂ O (g)    CO (g)  + 3 H₂ (g)  K c = 0.26 What is the pressure equilibrium constant, K p ? A)  K p = 0.26; K p and K c are always equivalent. B)  K p = 2.7×10 - 5 C)  K p = 1.5×10 - 3 D)  K p = 6.6×102 E)  K p = 2.5×103" class="answers-bank-image d-inline" rel="preload" > CO (g)  + 3 H₂ (g)  K c = 0.26 What is the pressure equilibrium constant, K p ?

Accepted Answer

A)   K p = 0.26; K p and K c are always equivalent.
B)   K p = 2.7×10 - 5
C)   K p = 1.5×10 - 3
D)   K p = 6.6×102
E)   K p = 2.5×103

Question 7

For the reaction 2 SO₂ (g)  + Cl₂ (g)   2 SO₂ Cl₂ (g) , the expression for K c is

Accepted Answer

A)   
B)   
C)   
D)   
E)

Question 8

For the high temperature equilibrium system, 2 H₂ O (g)  2 B)  (1)  increases while (2)  decreases the concentration of O2 C)  (1)  decreases while (2)  increases the concentration of O2 D)  (1)  and (2)  decrease the concentration of O2 E)  none of these" class="answers-bank-image d-inline" rel="preload" > 2 H₂ (g)  + O₂(g) , what will be the effect on the equilibrium concentration of O₂(g)  upon:
(1)  adding H₂ O (g)  and (2)  decreasing the pressure of the system?

Accepted Answer

A)   (1)  and (2)  increase the concentration of O2
B)   (1)  increases while (2)  decreases the concentration of O2
C)   (1)  decreases while (2)  increases the concentration of O2
D)   (1)  and (2)  decrease the concentration of O2
E)   none of these

Question 9

For the reaction 2 KClO3(s)  3(s)    2 KCl (s)  + 3 O₂(g) , K c = 2.0 at 750 C. What is the equilibrium concentration of O₂? A)  2.0 M B)  (2.0) 1/3 M C)  (2.0)  - 1/3 M D)  8.0 M E)  (8.0)  - 1 M" class="answers-bank-image d-inline" rel="preload" > 2 KCl (s)  + 3 O₂(g) , K c = 2.0 at 750 C. What is the equilibrium concentration of O₂?

Accepted Answer

A)   2.0 M
B)   (2.0) 1/3 M
C)   (2.0)  - 1/3 M
D)   8.0 M
E)   (8.0)  - 1 M

Question 10

What is the concentration of Ag+ ions in a saturated solution of Ag2CrO4 in water?
K sp = 9.0×10 - 12 for Ag2CrO4.

Accepted Answer

A)   2.1×10 - 4 M
B)   1.0 M
C)   2.6×10 - 4 M
D)   1.3×10 - 4 M
E)   3.0×10 - 6 M

Question 11

Mg(OH) 2 ( K sp = 8.9×10 - 12)  is precipitated by the addition of strong base to a 0.10 M solution of MgCl2. At what [OH - ] will Mg(OH) 2 begin to precipitate?

Accepted Answer

A)   1.0 M
B)   0.10 M
C)   9.4×10 - 6 M
D)   2.1×10 - 4 M
E)   8.9×10 - 12 M

Question 12

Inert helium gas was injected into a reaction vessel of fixed volume containing an equilibrium mixture of 2 SO₂ (g)  + O₂(g)  3(g) . The pressure was increased from 1.0 atm to 2.0 atm by the adding helium. Which of the following statements describes the new equilibrium system? A)  [SO3] increases B)  [SO2] increases C)  [SO3] decreases D)  [O2] increases E)  [SO3], [SO2], and [O2] remain unchanged" class="answers-bank-image d-inline" rel="preload" > 2 SO3(g) . The pressure was increased from 1.0 atm to 2.0 atm by the adding helium. Which of the following statements describes the new equilibrium system?

Accepted Answer

A)   [SO3] increases
B)   [SO2] increases
C)   [SO3] decreases
D)   [O2] increases
E)   [SO3], [SO2], and [O2] remain unchanged

Question 13

What is the solubility of PbSO4 ( K sp = 2.0×10 - 8)  in a solution that contains 100.0 g of Na2SO4 in 1.00 L?

Accepted Answer

A)   1.7×10 - 4 M
B)   2.0×10 - 10 M
C)   2.4×10 - 8 M
D)   2.8×10 - 8 M
E)   2.0×10 - 8 M

Question 14

One liter of solution is made containing 10 - 4 moles of Mn2+ and 10 - 5 moles of Fe2+. The [OH - ] is adjusted to 1.82×10 - 4 M . Which of the following statements is true, given K sp [Mn(OH) 2] = 4.5×10 - 14 and K sp [Fe(OH) 2] = 2.0×10 - 15?

Accepted Answer

A)   Both Mn and Fe will precipitate as hydroxides.
B)   Only Fe2+ will precipitate.
C)   Only Mn2+ will precipitate.
D)   Neither will precipitate.
E)   Need more information to draw a conclusion.

Question 15

What is the molar solubility of Ag2SO4 in 0.11 M Na2SO4?
K sp(Ag2SO4)  = 1.5×10 - 5

Accepted Answer

A)   [Ag2SO4] = 1.2×10 - 9 M
B)   [Ag2SO4] = 3.4×10 - 5 M
C)   [Ag2SO4] = 6.8×10 - 5 M
D)   [Ag2SO4] = 5.8×10 - 3 M
E)   [Ag2SO4] = 8.3×10 - 3 M

Question 16

Consider solving for the molar solubility of a 3:2 electrolyte such as Mg3(PO4) 2. What solubility product expression listed below would be suitable for solving for "x" which could then be related to the solubility of Mg3(PO4) 2?

Accepted Answer

A)   K sp = x5
B)   K sp = 4x3
C)   K sp = 6x5
D)   K sp = 5x5
E)   K sp = 108x5

Question 17

Exhibit 14-6 Consider the reaction at equilibrium below and its corresponding equilibrium constant to answer the following question(s) . 2 NO₂ (g)  - 13 A pressure of 0.45 atm of NO₂ is introduced into a container and allowed to come to equilibrium. Complete the ICE equilibrium table shown below to get started. Partial pressure S2NO₂ 2 NO O₂Initial 0.45 M Change At equilibrium -Refer to Exhibit 14-6. Upon constructing an ICE table, what expression would be obtained that represents the equilibrium partial pressure of NO₂ as it reaches equilibrium? A)  equilibrium PNO2 = 0.45 atm - x B)  equilibrium PNO2 = 0.45 atm + x C)  equilibrium PNO2 = 0.45 atm - 2x D)  equilibrium PNO2 = 0.45 atm + 2x E)  equilibrium PNO2 = 0.45 atm + 1/2 x" class="answers-bank-image d-inline" rel="preload" > 2 NO (g)  + O₂(g)  K p = 4.48*10- 13 A pressure of 0.45 atm of NO₂ is introduced into a container and allowed to come to equilibrium. Complete the ICE equilibrium table shown below to get started. Partial pressure S2NO₂ 2 NO O₂Initial 0.45 M Change At equilibrium
-Refer to Exhibit 14-6. Upon constructing an ICE table, what expression would be obtained that represents the equilibrium partial pressure of NO₂ as it reaches equilibrium?

Accepted Answer

A)   equilibrium PNO2 = 0.45 atm - x
B)   equilibrium PNO2 = 0.45 atm + x
C)   equilibrium PNO2 = 0.45 atm - 2x
D)   equilibrium PNO2 = 0.45 atm + 2x
E)   equilibrium PNO2 = 0.45 atm + 1/2 x

Question 18

At a certain temperature, for the reaction NH ₄Cl (s)   NH₃(g)  + HCl (g) , K p = 9.0.
What is the equilibrium partial pressure of NH₃?

Accepted Answer

A)   9.0 atm
B)   0.11 atm
C)   3.0 atm
D)   0.33 atm
E)   0.91 atm

Question 19

A reaction vessel is charged with 1.720 atm of N₂O4 and 1.220 atm of NO₂ at 25 C. The equilibrium reaction is given in the equation below. N₂O4 (g)  4 and 1.220 atm of NO₂ at 25 C. The equilibrium reaction is given in the equation below. N₂O4 (g)    2 NO₂ (g)  After equilibrium is reached, the partial pressure of NO₂ is 0.555 atm. What is the value for the equilibrium constant, K c , of this reaction at 25 C? A)  K c = 0.129 B)  K c = 0.150 C)  K c = 0.222 D)  K c = 0.270 E)  K c = 6.67" class="answers-bank-image d-inline" rel="preload" > 2 NO₂ (g) 
After equilibrium is reached, the partial pressure of NO₂ is 0.555 atm. What is the value for the equilibrium constant, K c , of this reaction at 25 C?

Accepted Answer

A)   K c = 0.129
B)   K c = 0.150
C)   K c = 0.222
D)   K c = 0.270
E)   K c = 6.67

Question 20

What is the molar solubility of Al(OH) 3, given K sp[Al(OH) 3] = 3×10 - 34?

Accepted Answer

A)   [Al(OH) 3] = 2.2×10 - 12 M
B)   [Al(OH) 3] = 1.8×10 - 9 M
C)   [Al(OH) 3] = 3.2×10 - 9 M
D)   [Al(OH) 3] = 4.2×10 - 9 M
E)   [Al(OH) 3] = 9.5×10 - 9 M

Exam 14: Chemical Equilibrium

For the reaction 2 KClO₃(s) 2 KCl (s) + 3 O₂(g) , K c = 2.0 at 750 C. What is the equilibrium concentration of O₂?

Correct Answer
verified

Inert helium gas was injected into a reaction vessel of fixed volume containing an equilibrium mixture of 2 SO₂ (g) + O₂(g) 2 SO₃(g) . The pressure was increased from 1.0 atm to 2.0 atm by the adding helium. Which of the following statements describes the new equilibrium system?

Correct Answer
verified

At 700 C, the equilibrium constant ( K c ) for the reaction N₂(g) + 3 H₂ (g) 2 NH₃(g) is 2.37 10 - 3 . If 0.683 mol of N₂, 8.80 mol of H₂ and 0.744 mole of NH₃are mixed in a 1.00 L container at 700 C:

Correct Answer
verified

Consider solving for the molar solubility of a 3:2 electrolyte such as Mg₃(PO₄) ₂. What solubility product expression listed below would be suitable for solving for "x" which could then be related to the solubility of Mg₃(PO₄) ₂?

Correct Answer
verified

Mg(OH) ₂ ( K _sp = 8.9×10^{- 12}) is precipitated by the addition of strong base to a 0.10 M solution of MgCl₂. At what [OH^-] will Mg(OH) ₂ begin to precipitate?

Correct Answer
verified

Given: 2 Cl₂ (g) + 2 H₂ O (g) 4 HCl (g) + O₂(g) K c (480 C) = 0.0752 What would be the equilibrium constant, K c , for the equation that follows? Cl₂ (g) + H₂ O (g) 2 HCl (g) + 1 / 2 O₂(g) K c (480 C) = ??

Correct Answer
verified

At a certain temperature, for the reaction NH ₄Cl (s) NH₃(g) + HCl (g) , K p = 9.0. What is the equilibrium partial pressure of NH₃?

Correct Answer
verified

Correct Answer
verified

For the reaction 2 SO₂ (g) + Cl₂ (g) 2 SO₂ Cl₂ (g) , the expression for K c is

Correct Answer
verified

Correct Answer
verified

At 1073 K, the pressure of CO₂ is 0.236 atm when produced by the reaction: CaCO₃(s) CaO (s) + CO₂ (g) The value of K c for this reaction at 1073 K is (R = 0.0821 L atm/(mol K) ) :

Correct Answer
verified

Consider the following reaction at 1200 K: CH₄ (g) + H₂ O (g) CO (g) + 3 H₂ (g) K c = 0.26 What is the pressure equilibrium constant, K p ?

Correct Answer
verified

What is the solubility of PbSO₄ ( K _sp = 2.0×10^{- 8}) in a solution that contains 100.0 g of Na₂SO₄ in 1.00 L?

Correct Answer
verified

For the high temperature equilibrium system, 2 H₂ O (g) 2 H₂ (g) + O₂(g) , what will be the effect on the equilibrium concentration of O₂(g) upon: (1) adding H₂ O (g) and (2) decreasing the pressure of the system?

Correct Answer
verified

Correct Answer
verified

What is the molar solubility of Ag₂SO₄ in 0.11 M Na₂SO₄? K _sp(Ag₂SO₄) = 1.5×10^{- 5}

Correct Answer
verified

What is the molar solubility of Al(OH) ₃, given K _sp[Al(OH) ₃] = 3×10^{- 34}?

Correct Answer
verified

What is the equilibrium constant expression for the following unbalanced equation at equilibrium? (Pay careful attention to the phase indicators!) Na₂ O₂(s) + CO₂ (g) Na₂ CO₃(s) + O₂(g)

Correct Answer
verified

One liter of solution is made containing 10^{- 4} moles of Mn²⁺ and 10^{- 5} moles of Fe²⁺. The [OH^-] is adjusted to 1.82×10^{- 4} M . Which of the following statements is true, given K _sp [Mn(OH) ₂] = 4.5×10^{- 14} and K _sp [Fe(OH) ₂] = 2.0×10^{- 15}?

Correct Answer
verified

What is the concentration of Ag⁺ ions in a saturated solution of Ag₂CrO₄ in water? K _sp = 9.0×10^{- 12} for Ag₂CrO₄.

Correct Answer
verified

Exam 14: Chemical Equilibrium

For the reaction 2 KClO3(s) 2 KCl (s) + 3 O₂(g) , K c = 2.0 at 750 C. What is the equilibrium concentration of O₂?

Correct AnswerverifiedShow Answer

Inert helium gas was injected into a reaction vessel of fixed volume containing an equilibrium mixture of 2 SO₂ (g) + O₂(g) 2 SO3(g) . The pressure was increased from 1.0 atm to 2.0 atm by the adding helium. Which of the following statements describes the new equilibrium system?

Correct AnswerverifiedShow Answer

At 700 C, the equilibrium constant ( K c ) for the reaction N₂(g) + 3 H₂ (g) 2 NH₃(g) is 2.37 10 - 3 . If 0.683 mol of N₂, 8.80 mol of H₂ and 0.744 mole of NH₃are mixed in a 1.00 L container at 700 C:

Correct AnswerverifiedShow Answer

Consider solving for the molar solubility of a 3:2 electrolyte such as Mg3(PO4) 2. What solubility product expression listed below would be suitable for solving for "x" which could then be related to the solubility of Mg3(PO4) 2?

Correct AnswerverifiedShow Answer

Mg(OH) 2 ( K sp = 8.9×10 - 12) is precipitated by the addition of strong base to a 0.10 M solution of MgCl2. At what [OH - ] will Mg(OH) 2 begin to precipitate?

Correct AnswerverifiedShow Answer

Given: 2 Cl₂ (g) + 2 H₂ O (g) 4 HCl (g) + O₂(g) K c (480 C) = 0.0752 What would be the equilibrium constant, K c , for the equation that follows? Cl₂ (g) + H₂ O (g) 2 HCl (g) + 1 / 2 O₂(g) K c (480 C) = ??

Correct AnswerverifiedShow Answer

At a certain temperature, for the reaction NH ₄Cl (s) NH₃(g) + HCl (g) , K p = 9.0. What is the equilibrium partial pressure of NH₃?

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

For the reaction 2 SO₂ (g) + Cl₂ (g) 2 SO₂ Cl₂ (g) , the expression for K c is

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

At 1073 K, the pressure of CO₂ is 0.236 atm when produced by the reaction: CaCO3(s) CaO (s) + CO₂ (g) The value of K c for this reaction at 1073 K is (R = 0.0821 L atm/(mol K) ) :

Correct AnswerverifiedShow Answer

Consider the following reaction at 1200 K: CH4 (g) + H₂ O (g) CO (g) + 3 H₂ (g) K c = 0.26 What is the pressure equilibrium constant, K p ?

Correct AnswerverifiedShow Answer

What is the solubility of PbSO4 ( K sp = 2.0×10 - 8) in a solution that contains 100.0 g of Na2SO4 in 1.00 L?

Correct AnswerverifiedShow Answer

For the high temperature equilibrium system, 2 H₂ O (g) 2 H₂ (g) + O₂(g) , what will be the effect on the equilibrium concentration of O₂(g) upon: (1) adding H₂ O (g) and (2) decreasing the pressure of the system?

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

What is the molar solubility of Ag2SO4 in 0.11 M Na2SO4? K sp(Ag2SO4) = 1.5×10 - 5

Correct AnswerverifiedShow Answer

What is the molar solubility of Al(OH) 3, given K sp[Al(OH) 3] = 3×10 - 34?

Correct AnswerverifiedShow Answer

What is the equilibrium constant expression for the following unbalanced equation at equilibrium? (Pay careful attention to the phase indicators!) Na2 O₂(s) + CO₂ (g) Na2 CO3(s) + O₂(g)

Correct AnswerverifiedShow Answer

One liter of solution is made containing 10 - 4 moles of Mn2+ and 10 - 5 moles of Fe2+. The [OH - ] is adjusted to 1.82×10 - 4 M . Which of the following statements is true, given K sp [Mn(OH) 2] = 4.5×10 - 14 and K sp [Fe(OH) 2] = 2.0×10 - 15?

Correct AnswerverifiedShow Answer

What is the concentration of Ag+ ions in a saturated solution of Ag2CrO4 in water? K sp = 9.0×10 - 12 for Ag2CrO4.

Correct AnswerverifiedShow Answer

For the reaction 2 KClO₃(s) 2 KCl (s) + 3 O₂(g) , K c = 2.0 at 750 C. What is the equilibrium concentration of O₂?

Correct Answer
verified

Inert helium gas was injected into a reaction vessel of fixed volume containing an equilibrium mixture of 2 SO₂ (g) + O₂(g) 2 SO₃(g) . The pressure was increased from 1.0 atm to 2.0 atm by the adding helium. Which of the following statements describes the new equilibrium system?

Correct Answer
verified

Correct Answer
verified

Consider solving for the molar solubility of a 3:2 electrolyte such as Mg₃(PO₄) ₂. What solubility product expression listed below would be suitable for solving for "x" which could then be related to the solubility of Mg₃(PO₄) ₂?

Correct Answer
verified

Mg(OH) ₂ ( K _sp = 8.9×10^{- 12}) is precipitated by the addition of strong base to a 0.10 M solution of MgCl₂. At what [OH^-] will Mg(OH) ₂ begin to precipitate?

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

At 1073 K, the pressure of CO₂ is 0.236 atm when produced by the reaction: CaCO₃(s) CaO (s) + CO₂ (g) The value of K c for this reaction at 1073 K is (R = 0.0821 L atm/(mol K) ) :

Correct Answer
verified

Consider the following reaction at 1200 K: CH₄ (g) + H₂ O (g) CO (g) + 3 H₂ (g) K c = 0.26 What is the pressure equilibrium constant, K p ?

Correct Answer
verified

What is the solubility of PbSO₄ ( K _sp = 2.0×10^{- 8}) in a solution that contains 100.0 g of Na₂SO₄ in 1.00 L?

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

What is the molar solubility of Ag₂SO₄ in 0.11 M Na₂SO₄? K _sp(Ag₂SO₄) = 1.5×10^{- 5}

Correct Answer
verified

What is the molar solubility of Al(OH) ₃, given K _sp[Al(OH) ₃] = 3×10^{- 34}?

Correct Answer
verified

What is the equilibrium constant expression for the following unbalanced equation at equilibrium? (Pay careful attention to the phase indicators!) Na₂ O₂(s) + CO₂ (g) Na₂ CO₃(s) + O₂(g)

Correct Answer
verified

One liter of solution is made containing 10^{- 4} moles of Mn²⁺ and 10^{- 5} moles of Fe²⁺. The [OH^-] is adjusted to 1.82×10^{- 4} M . Which of the following statements is true, given K _sp [Mn(OH) ₂] = 4.5×10^{- 14} and K _sp [Fe(OH) ₂] = 2.0×10^{- 15}?

Correct Answer
verified

What is the concentration of Ag⁺ ions in a saturated solution of Ag₂CrO₄ in water? K _sp = 9.0×10^{- 12} for Ag₂CrO₄.

Correct Answer
verified