Question 1

For the following reaction,what is △n required in the conversion of Kc to Kp? KClO3(s)⇌ KClO(s)+ O2(g)

Accepted Answer

A) 3 
B) -1 
C) -2 
D) 2 
E) 1 
A) 3 
B) -1 
C) -2 
D) 2 
E) 1 E

Question 2

Consider the following reaction at equilibrium.What effect will removing NO2 have on the system? 
SO2(g)+ NO2(g)⇌ SO3(g)+ NO(g)

Accepted Answer

A) The reaction will shift in the direction of products. 
B) The reaction will shift to decrease the pressure. 
C) No change will occur since NO2 is not included in the equilibrium expression. 
D) The reaction will shift in the direction of reactants. 
E) The equilibrium constant will decrease. 
A) The reaction will shift in the direction of products. 
B) The reaction will shift to decrease the pressure. 
C) No change will occur since NO2 is not included in the equilibrium expression. 
D) The reaction will shift in the direction of reactants. 
E) The equilibrium constant will decrease. D

Question 3

Consider the following reaction,equilibrium concentrations,and equilibrium constant at a particular temperature.Determine the equilibrium concentration of SO2(g). 
$\quad$$\quad$2SO2(g)+ O2(g)⇌ 2SO3(g)$\quad$$\quad$Kc = 1.7 × 108 M-1
$\quad$$\quad$[SO3]eq = 0.0034 mol L-1 $\quad$$\quad$[O2]eq = 0.0018 mol L-1

Accepted Answer

A) 2.8 × 1013 mol L-1 
B) 1.88 mol L-1 
C) 6.1 × 10-6 mol L-1 
D) 1.0 × 103 mol L-1 
E) 1.4 mol L-1 
A) 2.8 × 1013 mol L-1 
B) 1.88 mol L-1 
C) 6.1 × 10-6 mol L-1 
D) 1.0 × 103 mol L-1 
E) 1.4 mol L-1 C

Question 4

Which of the following statements is TRUE?

Accepted Answer

A) If Q  K,it means the forward reaction will proceed to form more products. 
C) If Q = K,it means the reaction is at equilibrium. 
D) If Q > K,it means the reaction is shifted to the right. 
A) If Q  K,it means the forward reaction will proceed to form more products. 
C) If Q = K,it means the reaction is at equilibrium. 
D) If Q > K,it means the reaction is shifted to the right.

Question 5

The equilibrium constant,Kp,equals 3.40 for the isomerization reaction: cis-2-butene ⇌ trans-2-butene
If a flask initially contains 0.250 bar of cis-2-butene and 0.165 bar of trans-2-butene,what is the equilibrium pressure of each gas?

Accepted Answer

A) P(cis-2-butene)= 0.0485 bar and P(trans-2-butene)= 0.165 bar 
B) P(cis-2-butene)= 0.0458 bar and P(trans-2-butene)= 0.156 bar 
C) P(cis-2-butene)= 0.0735 bar and P(trans-2-butene)= 0.250 bar 
D) P(cis-2-butene)= 0.0943 bar and P(trans-2-butene)= 0.321 bar 
A) P(cis-2-butene)= 0.0485 bar and P(trans-2-butene)= 0.165 bar 
B) P(cis-2-butene)= 0.0458 bar and P(trans-2-butene)= 0.156 bar 
C) P(cis-2-butene)= 0.0735 bar and P(trans-2-butene)= 0.250 bar 
D) P(cis-2-butene)= 0.0943 bar and P(trans-2-butene)= 0.321 bar

Question 6

The equilibrium constant is given for one of two reactions below.Determine the value of the missing equilibrium constant. 
$\quad$H2(g)+ Br2(g)⇌ 2HBr$\quad$(g)K = 3.8 × 104
$\quad$2HBr(g)⇌ H2(g)+ Br2$\quad$(g)K = ?

Accepted Answer

A) 1.9 × 104 
B) 5.3 × 10-5 
C) 2.6 × 10-5 
D) 6.4 × 10-4 
E) 1.6 × 103 
A) 1.9 × 104 
B) 5.3 × 10-5 
C) 2.6 × 10-5 
D) 6.4 × 10-4 
E) 1.6 × 103

Question 7

The reaction below has a Kc value of 61 M-2.What is the value of Kp for this reaction at 500 K? 
$\quad$N2(g)+ 3H2(g)⇌ 2NH3(g)

Accepted Answer

A) 15 bar-2 
B) 61 bar-2 
C) 28 bar-2 
D) 3.6 × 10-2 bar-2 
E) 1.9 × 10-2 bar-2 
A) 15 bar-2 
B) 61 bar-2 
C) 28 bar-2 
D) 3.6 × 10-2 bar-2 
E) 1.9 × 10-2 bar-2

Question 8

Express the equilibrium constant for the following reaction: 
2 CH3Cl(g)+ Cl2(g)? 2 CH2Cl2(g)+ H2(g)

Accepted Answer

A) Kp = $\frac { \mathrm { P } \left( \mathrm { CH } _ { 2 } \mathrm { Cl } _ { 2 } \right) \times \mathrm { P } \left( \mathrm { H } _ { 2 } \right) } { \mathrm { P } \left( \mathrm { CH } _ { 3 } \mathrm { Cl } \right) \times \mathrm { P } \left( \mathrm { Cl } _ { 2 } \right) }$ 
B) KP = $\frac { \mathrm { P } ^ { 2 } \left( \mathrm { CH } _ { 2 } \mathrm { Cl } _ { 2 } \right) \times \mathrm { P } \left( \mathrm { H } _ { 2 } \right) } { \mathrm { P } ^ { 2 } \left( \mathrm { CH } _ { 3 } \mathrm { Cl } \right) \times \mathrm { P } \left( \mathrm { Cl } _ { 2 } \right) }$ 
C) KP = $\frac { \mathrm { P } ^ { 2 } \left( \mathrm { CH } _ { 3 } \mathrm { Cl } \right) \times \mathrm { P } \left( \mathrm { Cl } _ { 2 } \right) } { \mathrm { P } ^ { 2 } \left( \mathrm { CH } _ { 2 } \mathrm { Cl } _ { 2 } \right) \times \mathrm { P } \left( \mathrm { H } _ { 2 } \right) }$ 
D) KP = $\frac { \mathrm { P } \left( \mathrm { CH } _ { 3 } \mathrm { Cl } \right) \times \mathrm { P } \left( \mathrm { Cl } _ { 2 } \right) } { \mathrm { P } \left( \mathrm { CH } _ { 2 } \mathrm { Cl } _ { 2 } \right) \times \mathrm { P } \left( \mathrm { H } _ { 2 } \right) }$ 
E) KP = $\frac { \mathrm { P } 1 / 2 \left( \mathrm { CH } _ { 3 } \mathrm { Cl } \right) \times \mathrm { P } \left( \mathrm { Cl } _ { 2 } \right) } { \mathrm { P } ^ { 1 / 2 } \left( \mathrm { CH } _ { 2 } \mathrm { Cl } _ { 2 } \right) \times \mathrm { P } \left( \mathrm { H } _ { 2 } \right) }$ 
A) Kp = $\frac { \mathrm { P } \left( \mathrm { CH } _ { 2 } \mathrm { Cl } _ { 2 } \right) \times \mathrm { P } \left( \mathrm { H } _ { 2 } \right) } { \mathrm { P } \left( \mathrm { CH } _ { 3 } \mathrm { Cl } \right) \times \mathrm { P } \left( \mathrm { Cl } _ { 2 } \right) }$ 
B) KP = $\frac { \mathrm { P } ^ { 2 } \left( \mathrm { CH } _ { 2 } \mathrm { Cl } _ { 2 } \right) \times \mathrm { P } \left( \mathrm { H } _ { 2 } \right) } { \mathrm { P } ^ { 2 } \left( \mathrm { CH } _ { 3 } \mathrm { Cl } \right) \times \mathrm { P } \left( \mathrm { Cl } _ { 2 } \right) }$ 
C) KP = $\frac { \mathrm { P } ^ { 2 } \left( \mathrm { CH } _ { 3 } \mathrm { Cl } \right) \times \mathrm { P } \left( \mathrm { Cl } _ { 2 } \right) } { \mathrm { P } ^ { 2 } \left( \mathrm { CH } _ { 2 } \mathrm { Cl } _ { 2 } \right) \times \mathrm { P } \left( \mathrm { H } _ { 2 } \right) }$ 
D) KP = $\frac { \mathrm { P } \left( \mathrm { CH } _ { 3 } \mathrm { Cl } \right) \times \mathrm { P } \left( \mathrm { Cl } _ { 2 } \right) } { \mathrm { P } \left( \mathrm { CH } _ { 2 } \mathrm { Cl } _ { 2 } \right) \times \mathrm { P } \left( \mathrm { H } _ { 2 } \right) }$ 
E) KP = $\frac { \mathrm { P } 1 / 2 \left( \mathrm { CH } _ { 3 } \mathrm { Cl } \right) \times \mathrm { P } \left( \mathrm { Cl } _ { 2 } \right) } { \mathrm { P } ^ { 1 / 2 } \left( \mathrm { CH } _ { 2 } \mathrm { Cl } _ { 2 } \right) \times \mathrm { P } \left( \mathrm { H } _ { 2 } \right) }$

Question 9

Express the equilibrium constant for the following reaction: 
KClO3(s)? KClO(s)+ O2(g)

Accepted Answer

A) Kc = $\frac { [ \mathrm { KClO } ] \left[ \mathrm { O } _ { 2 } \right] } { \left[ \mathrm { KClO } _ { 3 } \right] }$ 
B) Kc = [O2]-1 
C) Kc = $\frac { [ \mathrm { KClO } ] ^ { 2 } \left[ \mathrm { O } _ { 2 } \right] ^ { 2 } } { \left[ \mathrm { KClO } _ { 3 } \right] ^ { 2 } }$ 
D) Kc = $\left[ \mathrm { KClO } _ { 3 } \right]$
$[ \mathrm { KClO } ] \left[ \mathrm { O } _ { 2 } \right]$

$\frac {[{ KClO } _ { 3 }] } { \mathrm [{ KClO } ] \left[ \mathrm { O } _ { 2 } \right] }$ 
E) Kc = [O2] 
A) Kc = $\frac { [ \mathrm { KClO } ] \left[ \mathrm { O } _ { 2 } \right] } { \left[ \mathrm { KClO } _ { 3 } \right] }$ 
B) Kc = [O2]-1 
C) Kc = $\frac { [ \mathrm { KClO } ] ^ { 2 } \left[ \mathrm { O } _ { 2 } \right] ^ { 2 } } { \left[ \mathrm { KClO } _ { 3 } \right] ^ { 2 } }$ 
D) Kc = $\left[ \mathrm { KClO } _ { 3 } \right]$
$[ \mathrm { KClO } ] \left[ \mathrm { O } _ { 2 } \right]$

$\frac {[{ KClO } _ { 3 }] } { \mathrm [{ KClO } ] \left[ \mathrm { O } _ { 2 } \right] }$ 
E) Kc = [O2]

Question 10

Express the equilibrium constant for the following reaction: 
PCl5(g)? PCl3(g)+ Cl2(g)

Accepted Answer

A) KP = $\frac { \mathrm { P } \left( \mathrm { PCl } _ { 5 } \right) } { \mathrm { P } \left( \mathrm { PCl } _ { 3 } \right) \times \mathrm { P } \left( \mathrm { Cl } _ { 2 } \right) }$ 
B) KP = $\frac { \mathrm { P } ^ { 2 } \left( \mathrm { PCl } _ { 3 } \right) \times \mathrm { P } ^ { 2 } \left( \mathrm { Cl } _ { 2 } \right) } { \mathrm { P } ^ { 2 } \left( \mathrm { PCl } _ { 5 } \right) }$ 
C) KP = $\frac { \mathrm { P } \left( \mathrm { PCl } _ { 3 } \right) \times \mathrm { P } ^ { 2 } ( \mathrm { Cl } ) } { \mathrm { P } \left( \mathrm { PCl } _ { 5 } \right) }$ 
D) KP = $\frac { \mathrm { P } \left( \mathrm { PCl } _ { 3 } \right) \times \mathrm { P } \left( \mathrm { Cl } _ { 2 } \right) } { \mathrm { P } \left( \mathrm { PCl } _ { 5 } \right) }$ 
E) KP = $\frac { \mathrm { P } ^ { 1 / 2 } \left( \mathrm { PCl } _ { 5 } \right) } { \mathrm { P } ^ { 1 / 2 } \left( \mathrm { PCl } _ { 3 } \right) \times \mathrm { P } ^ { 1 / 2 } \left( \mathrm { Cl } _ { 2 } \right) }$ 
A) KP = $\frac { \mathrm { P } \left( \mathrm { PCl } _ { 5 } \right) } { \mathrm { P } \left( \mathrm { PCl } _ { 3 } \right) \times \mathrm { P } \left( \mathrm { Cl } _ { 2 } \right) }$ 
B) KP = $\frac { \mathrm { P } ^ { 2 } \left( \mathrm { PCl } _ { 3 } \right) \times \mathrm { P } ^ { 2 } \left( \mathrm { Cl } _ { 2 } \right) } { \mathrm { P } ^ { 2 } \left( \mathrm { PCl } _ { 5 } \right) }$ 
C) KP = $\frac { \mathrm { P } \left( \mathrm { PCl } _ { 3 } \right) \times \mathrm { P } ^ { 2 } ( \mathrm { Cl } ) } { \mathrm { P } \left( \mathrm { PCl } _ { 5 } \right) }$ 
D) KP = $\frac { \mathrm { P } \left( \mathrm { PCl } _ { 3 } \right) \times \mathrm { P } \left( \mathrm { Cl } _ { 2 } \right) } { \mathrm { P } \left( \mathrm { PCl } _ { 5 } \right) }$ 
E) KP = $\frac { \mathrm { P } ^ { 1 / 2 } \left( \mathrm { PCl } _ { 5 } \right) } { \mathrm { P } ^ { 1 / 2 } \left( \mathrm { PCl } _ { 3 } \right) \times \mathrm { P } ^ { 1 / 2 } \left( \mathrm { Cl } _ { 2 } \right) }$

Question 11

Give the direction of the reaction if K << 1.

Accepted Answer

A) The forward reaction is favoured. 
B) The reverse reaction is favoured. 
C) Neither direction is favoured. 
D) If the temperature is raised,then the forward reaction is favoured. 
E) If the temperature is raised,then the reverse reaction is favoured. 
A) The forward reaction is favoured. 
B) The reverse reaction is favoured. 
C) Neither direction is favoured. 
D) If the temperature is raised,then the forward reaction is favoured. 
E) If the temperature is raised,then the reverse reaction is favoured.

Question 12

Express the equilibrium constant for the following reaction: 
2NH3(g)? N2(g)+ 3H2(g)

Accepted Answer

A) KP = $\frac { \mathrm { P } \left( \mathrm { N } _ { 2 } \right) \times \mathrm { P } ^{1 / 3} \left( \mathrm { H } _ { 2 } \right) } { \mathrm { P } ^{1 / 2} \left( \mathrm { NH } _ { 3 } \right) }$ 
B) KP = $\frac { \mathrm { P } ^ { 6 } \left( \mathrm { NH } _ { 3 } \right) } { \left[ \mathrm { N } _ { 2 } \right] ^ { 3 } \left[ \mathrm { H } _ { 2 } \right] ^ { 9 } }$ 
C) KP = $\frac { \mathrm { P } ^ { 2 } \left( \mathrm { NH } _ { 3 } \right) } { \mathrm { P } \left( \mathrm { N } _ { 2 } \right) \times \mathrm { P } ^ { 3 } \left( \mathrm { H } _ { 2 } \right) }$ 
D) KP = $\frac { \mathrm { P } \left( \mathrm { N } _ { 2 } \right) \times \mathrm { P } ^ { 3 } \left( \mathrm { H } _ { 2 } \right) } { \mathrm { P } ^ { 2 } \left( \mathrm { NH } _ { 3 } \right) }$ 
E) KP = $\frac { \mathrm { P } ^ { 1 / 2 } \left( \mathrm { NH } _ { 3 } \right) } { \mathrm { P } \left( \mathrm { N } _ { 2 } \right) \times \mathrm { P } ^ { 1 / 3 } \left( \mathrm { H } _ { 2 } \right) }$ 
A) KP = $\frac { \mathrm { P } \left( \mathrm { N } _ { 2 } \right) \times \mathrm { P } ^{1 / 3} \left( \mathrm { H } _ { 2 } \right) } { \mathrm { P } ^{1 / 2} \left( \mathrm { NH } _ { 3 } \right) }$ 
B) KP = $\frac { \mathrm { P } ^ { 6 } \left( \mathrm { NH } _ { 3 } \right) } { \left[ \mathrm { N } _ { 2 } \right] ^ { 3 } \left[ \mathrm { H } _ { 2 } \right] ^ { 9 } }$ 
C) KP = $\frac { \mathrm { P } ^ { 2 } \left( \mathrm { NH } _ { 3 } \right) } { \mathrm { P } \left( \mathrm { N } _ { 2 } \right) \times \mathrm { P } ^ { 3 } \left( \mathrm { H } _ { 2 } \right) }$ 
D) KP = $\frac { \mathrm { P } \left( \mathrm { N } _ { 2 } \right) \times \mathrm { P } ^ { 3 } \left( \mathrm { H } _ { 2 } \right) } { \mathrm { P } ^ { 2 } \left( \mathrm { NH } _ { 3 } \right) }$ 
E) KP = $\frac { \mathrm { P } ^ { 1 / 2 } \left( \mathrm { NH } _ { 3 } \right) } { \mathrm { P } \left( \mathrm { N } _ { 2 } \right) \times \mathrm { P } ^ { 1 / 3 } \left( \mathrm { H } _ { 2 } \right) }$

Question 13

Define Le Châtelier's principle.

Accepted Answer

Le Châtelier's principle state

Question 14

Kc is 1.67 × 1020 mol3 L-3 at 25 °C for the formation of iron(III)oxalate complex ion: Fe3+(aq)+ 3C2O42-(aq)⇌ [Fe(C2O4)3]3-(aq)
If 0.0200 mol L-1 Fe3+ is initially mixed with 1.00 mol L-1 oxalate ion,what is the concentration of Fe3+ ion at equilibrium?

Accepted Answer

A) 1.44 × 10-22 mol L-1 
B) 0.0100 mol L-1 
C) 8.35 × 1019 mol L-1 
D) 6.94 × 1021 mol L-1 
A) 1.44 × 10-22 mol L-1 
B) 0.0100 mol L-1 
C) 8.35 × 1019 mol L-1 
D) 6.94 × 1021 mol L-1

Question 15

Consider the following reaction: 
NO(g)+ SO3(g)⇌ NO2(g)+ SO2(g)
A reaction mixture initially contains 0.86 bar NO and 0.86 bar SO3.Determine the equilibrium pressure of NO2 if Kp for the reaction at this temperature is 0.0118.

Accepted Answer

A) 0.78 bar 
B) 0.084 bar 
C) 0.012 bar 
D) 0.85 bar 
E) 0.048 bar 
A) 0.78 bar 
B) 0.084 bar 
C) 0.012 bar 
D) 0.85 bar 
E) 0.048 bar

Question 16

How is the reaction quotient different from an equilibrium constant for a given reaction?

Accepted Answer

The expressions for both are identical.H

Question 17

Cyclohexane,C6H12,undergoes a molecular rearrangement in the presence of AlCl3 to form methylcyclopentane,CH3C5H9, according to the equation: 
$\quad$$\quad$C6H12 ⇌ CH3C5H9
If Kc = 0.143 at 25 °C for this reaction,find the equilibrium concentrations of C6H12 and CH3C5H9 if the initial concentrations are 0.200 mol L-1 and 0.075 mol L-1,respectively.

Accepted Answer

A) [C6H12] = 0.041 mol L-1,[CH3C5H9] = 0.041 mol L-1 
B) [C6H12] = 0.159 mol L-1,[CH3C5H9] = 0.116 mol L-1 
C) [C6H12] = 0.241 mol L-1,[CH3C5H9] = 0.034 mol L-1 
D) [C6H12] = 0.253 mol L-1,[CH3C5H9] = 0.022 mol L-1 
A) [C6H12] = 0.041 mol L-1,[CH3C5H9] = 0.041 mol L-1 
B) [C6H12] = 0.159 mol L-1,[CH3C5H9] = 0.116 mol L-1 
C) [C6H12] = 0.241 mol L-1,[CH3C5H9] = 0.034 mol L-1 
D) [C6H12] = 0.253 mol L-1,[CH3C5H9] = 0.022 mol L-1

Question 18

Consider the following reaction: 
CH4(g)+ 2H2S(g)⇌ CS2(g)+ 4H2(g)
A reaction mixture initially contains 0.50 mol L-1 CH4 and 0.75 mol L-1 H2S.If the equilibrium concentration of H2 is 0.44 mol L-1,find the equilibrium constant (mol L-1)for the reaction.

Accepted Answer

A) 0.23 mol2 L-2 
B) 0.038 mol2 L-2 
C) 2.9 mol2 L-2 
D) 10.mol2 L-2 
E) 0.34 mol2 L-2 
A) 0.23 mol2 L-2 
B) 0.038 mol2 L-2 
C) 2.9 mol2 L-2 
D) 10.mol2 L-2 
E) 0.34 mol2 L-2

Question 19

Consider the following reaction: 
NO(g)+ SO3(g)⇌ NO2(g)+ SO2(g)
A reaction mixture initially contains 1.24 bar NO and 0.92 bar SO3.Determine the equilibrium pressure of NO2 if Kp for the reaction at this temperature is 0.0118.

Accepted Answer

A) 0.32 bar 
B) 1.32 bar 
C) 0.10 bar 
D) 0.74 bar 
E) 0.022 bar 
A) 0.32 bar 
B) 1.32 bar 
C) 0.10 bar 
D) 0.74 bar 
E) 0.022 bar

Question 20

In a reaction mixture containing only products,what is the value of Q?

Accepted Answer

A) -1 
B) 1 
C) ∞ 
D) 0 
E) Q = K 
A) -1 
B) 1 
C) ∞ 
D) 0 
E) Q = K

Exam 14: Chemical Equilibrium

For the following reaction,what is △n required in the conversion of Kc to Kp? KClO3(s)⇌ KClO(s)+ O2(g)

Consider the following reaction at equilibrium.What effect will removing NO2 have on the system? SO2(g)+ NO2(g)⇌ SO3(g)+ NO(g)

Which of the following statements is TRUE?

The equilibrium constant,Kp,equals 3.40 for the isomerization reaction: cis-2-butene ⇌ trans-2-butene If a flask initially contains 0.250 bar of cis-2-butene and 0.165 bar of trans-2-butene,what is the equilibrium pressure of each gas?

The equilibrium constant is given for one of two reactions below.Determine the value of the missing equilibrium constant. \quad H2(g)+ Br2(g)⇌ 2HBr \quad (g)K = 3.8 × 104 \quad 2HBr(g)⇌ H2(g)+ Br2 \quad (g)K = ?

The reaction below has a Kc value of 61 M-2.What is the value of Kp for this reaction at 500 K? \quad N2(g)+ 3H2(g)⇌ 2NH3(g)

Express the equilibrium constant for the following reaction: 2 CH3Cl(g)+ Cl2(g)? 2 CH2Cl2(g)+ H2(g)

Express the equilibrium constant for the following reaction: KClO3(s)? KClO(s)+ O2(g)

Express the equilibrium constant for the following reaction: PCl5(g)? PCl3(g)+ Cl2(g)

Give the direction of the reaction if K << 1.

Express the equilibrium constant for the following reaction: 2NH3(g)? N2(g)+ 3H2(g)

Define Le Châtelier's principle.

Kc is 1.67 × 1020 mol3 L-3 at 25 °C for the formation of iron(III)oxalate complex ion: Fe3+(aq)+ 3C2O42-(aq)⇌ [Fe(C2O4)3]3-(aq) If 0.0200 mol L-1 Fe3+ is initially mixed with 1.00 mol L-1 oxalate ion,what is the concentration of Fe3+ ion at equilibrium?

Consider the following reaction: NO(g)+ SO3(g)⇌ NO2(g)+ SO2(g) A reaction mixture initially contains 0.86 bar NO and 0.86 bar SO3.Determine the equilibrium pressure of NO2 if Kp for the reaction at this temperature is 0.0118.

How is the reaction quotient different from an equilibrium constant for a given reaction?

Consider the following reaction: CH4(g)+ 2H2S(g)⇌ CS2(g)+ 4H2(g) A reaction mixture initially contains 0.50 mol L-1 CH4 and 0.75 mol L-1 H2S.If the equilibrium concentration of H2 is 0.44 mol L-1,find the equilibrium constant (mol L-1)for the reaction.

Consider the following reaction: NO(g)+ SO3(g)⇌ NO2(g)+ SO2(g) A reaction mixture initially contains 1.24 bar NO and 0.92 bar SO3.Determine the equilibrium pressure of NO2 if Kp for the reaction at this temperature is 0.0118.

In a reaction mixture containing only products,what is the value of Q?

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For the following reaction,what is △n required in the conversion of K_c to K_p? KClO₃(s)⇌ KClO(s)+ O₂(g)

Consider the following reaction at equilibrium.What effect will removing NO₂ have on the system? SO₂(g)+ NO₂(g)⇌ SO₃(g)+ NO(g)

The equilibrium constant,K_p,equals 3.40 for the isomerization reaction: cis-2-butene ⇌ trans-2-butene If a flask initially contains 0.250 bar of cis-2-butene and 0.165 bar of trans-2-butene,what is the equilibrium pressure of each gas?

The equilibrium constant is given for one of two reactions below.Determine the value of the missing equilibrium constant. $\quad$ H₂(g)+ Br₂(g)⇌ 2HBr $\quad$ (g)K = 3.8 × 10⁴ $\quad$ 2HBr(g)⇌ H₂(g)+ Br₂ $\quad$ (g)K = ?

The reaction below has a K_c value of 61 M^-2.What is the value of K_p for this reaction at 500 K? $\quad$ N₂(g)+ 3H₂(g)⇌ 2NH₃(g)

Express the equilibrium constant for the following reaction: 2 CH₃Cl(g)+ Cl₂(g)? 2 CH₂Cl₂(g)+ H₂(g)

Express the equilibrium constant for the following reaction: KClO₃(s)? KClO(s)+ O₂(g)

Express the equilibrium constant for the following reaction: PCl₅(g)? PCl₃(g)+ Cl₂(g)

Express the equilibrium constant for the following reaction: 2NH₃(g)? N₂(g)+ 3H₂(g)

K_c is 1.67 × 10²⁰ mol³ L^-3 at 25 °C for the formation of iron(III)oxalate complex ion: Fe³⁺(aq)+ 3C₂O₄^2-(aq)⇌ [Fe(C₂O₄)₃]^3-(aq) If 0.0200 mol L^-1 Fe³⁺ is initially mixed with 1.00 mol L^-1 oxalate ion,what is the concentration of Fe³⁺ ion at equilibrium?

Consider the following reaction: NO(g)+ SO₃(g)⇌ NO₂(g)+ SO₂(g) A reaction mixture initially contains 0.86 bar NO and 0.86 bar SO₃.Determine the equilibrium pressure of NO₂ if K_p for the reaction at this temperature is 0.0118.

Consider the following reaction: CH₄(g)+ 2H₂S(g)⇌ CS₂(g)+ 4H₂(g) A reaction mixture initially contains 0.50 mol L^-1 CH₄ and 0.75 mol L^-1 H₂S.If the equilibrium concentration of H₂ is 0.44 mol L^-1,find the equilibrium constant (mol L^-1)for the reaction.

Consider the following reaction: NO(g)+ SO₃(g)⇌ NO₂(g)+ SO₂(g) A reaction mixture initially contains 1.24 bar NO and 0.92 bar SO₃.Determine the equilibrium pressure of NO₂ if K_p for the reaction at this temperature is 0.0118.