Question 1

The following reaction occurred when a 1.0-liter reaction vessel was initially charged with 2.0 moles of N2(g)and 4.0 moles of H2(g):

Once equilibrium was established,the concentration of NH3(g)was determined to be 0.59 M at 700.°C.The value for Kc at 700.°C for the formation of ammonia is:

Accepted Answer

A)   3.5  ×	imes×  10-1
B)   6.8  ×	imes×  10-3
C)   1.1  ×	imes×  10-1
D)   6.6  ×	imes×  10-2
E)   none of these  B

Question 2

At a high temperature,equal concentrations of 0.160 mol/L of H2(g)and I2(g)are initially present in a flask.The H2 and I2 react according to the balanced equation below.

When equilibrium is reached,the concentration of H2(g)has decreased to 0.036 mol/L.What is the equilibrium constant,Kc,for the reaction?

Accepted Answer

A)   3.4
B)   4.0
C)   12
D)   22
E)   48 E

Question 3

A 2.5 L flask is filled with 0.25 mol SO3,0.20 mol SO2,and 0.40 mol O2,and allowed to reach equilibrium.Assume the temperature of the mixture is chosen so that Kc = 0.12.Predict the effect on the concentration of SO3 as equilibrium is achieved by using Q,the reaction quotient.
2 SO3(g)  2 SO2(g)+ O2(g)

Accepted Answer

A)   [SO3] will decrease because Q > K.
B)   [SO3] will decrease because Q 
C)   [SO3] will increase because Q 
D)   [SO3] will increase because Q > K.
E)   [SO3] will remain the same because Q = K. B

Question 4

In which of the following reactions does a decrease in the volume of the reaction vessel at constant temperature favor formation of the products?

Accepted Answer

A)   2H2(g) + O2(g)  2(g) + O2(g)    2H2O(g)  
B)   NO2(g) + CO(g)    NO(g) + CO2(g)  
C)   H2(g) + I2(g)    2HI(g)  
D)   2O3(g)    3O2(g)  
E)   MgCO3(s)    MgO(s) + CO2(g) " class="answers-bank-image d-inline" rel="preload" > 2H2O(g) 
B)   NO2(g) + CO(g)  2(g) + O2(g)    2H2O(g)  
B)   NO2(g) + CO(g)    NO(g) + CO2(g)  
C)   H2(g) + I2(g)    2HI(g)  
D)   2O3(g)    3O2(g)  
E)   MgCO3(s)    MgO(s) + CO2(g) " class="answers-bank-image d-inline" rel="preload" > NO(g) + CO2(g) 
C)   H2(g) + I2(g)  2(g) + O2(g)    2H2O(g)  
B)   NO2(g) + CO(g)    NO(g) + CO2(g)  
C)   H2(g) + I2(g)    2HI(g)  
D)   2O3(g)    3O2(g)  
E)   MgCO3(s)    MgO(s) + CO2(g) " class="answers-bank-image d-inline" rel="preload" > 2HI(g) 
D)   2O3(g)  2(g) + O2(g)    2H2O(g)  
B)   NO2(g) + CO(g)    NO(g) + CO2(g)  
C)   H2(g) + I2(g)    2HI(g)  
D)   2O3(g)    3O2(g)  
E)   MgCO3(s)    MgO(s) + CO2(g) " class="answers-bank-image d-inline" rel="preload" > 3O2(g) 
E)   MgCO3(s)  2(g) + O2(g)    2H2O(g)  
B)   NO2(g) + CO(g)    NO(g) + CO2(g)  
C)   H2(g) + I2(g)    2HI(g)  
D)   2O3(g)    3O2(g)  
E)   MgCO3(s)    MgO(s) + CO2(g) " class="answers-bank-image d-inline" rel="preload" > MgO(s) + CO2(g)

Question 5

Consider the following equilibrium:
PCl5(g)  PCl3(g)+ Cl2(g); $~~~~~~~~$ $\Delta$H = 92 kJ
The concentration of PCl3 at equilibrium may be increased by

Accepted Answer

A)   decreasing the temperature.
B)   adding Cl2 to the system.
C)   adding PCl5 to the system.
D)   increasing the pressure.
E)   adding a catalyst.

Question 6

For which of the following equilibria does Kc = Kp?

Accepted Answer

A)   N2(g) + 3H2(g)  c = Kp? 
A)   N2(g) + 3H2(g)    2NH3(g)  
B)   CO(g) + H2O(g)    CO2(g) + H2(g)  
C)   CO(g) + 3H2(g)    CH4(g) + H2O(g)  
D)   CaO(s) + CO2(g)    CaCO3(s)  
E)   HBr(g)    ½H2(g) + ½Br2(l) " class="answers-bank-image d-inline" rel="preload" > 2NH3(g) 
B)   CO(g) + H2O(g)  c = Kp? 
A)   N2(g) + 3H2(g)    2NH3(g)  
B)   CO(g) + H2O(g)    CO2(g) + H2(g)  
C)   CO(g) + 3H2(g)    CH4(g) + H2O(g)  
D)   CaO(s) + CO2(g)    CaCO3(s)  
E)   HBr(g)    ½H2(g) + ½Br2(l) " class="answers-bank-image d-inline" rel="preload" > CO2(g) + H2(g) 
C)   CO(g) + 3H2(g)  c = Kp? 
A)   N2(g) + 3H2(g)    2NH3(g)  
B)   CO(g) + H2O(g)    CO2(g) + H2(g)  
C)   CO(g) + 3H2(g)    CH4(g) + H2O(g)  
D)   CaO(s) + CO2(g)    CaCO3(s)  
E)   HBr(g)    ½H2(g) + ½Br2(l) " class="answers-bank-image d-inline" rel="preload" > CH4(g) + H2O(g) 
D)   CaO(s) + CO2(g)  c = Kp? 
A)   N2(g) + 3H2(g)    2NH3(g)  
B)   CO(g) + H2O(g)    CO2(g) + H2(g)  
C)   CO(g) + 3H2(g)    CH4(g) + H2O(g)  
D)   CaO(s) + CO2(g)    CaCO3(s)  
E)   HBr(g)    ½H2(g) + ½Br2(l) " class="answers-bank-image d-inline" rel="preload" > CaCO3(s) 
E)   HBr(g)  c = Kp? 
A)   N2(g) + 3H2(g)    2NH3(g)  
B)   CO(g) + H2O(g)    CO2(g) + H2(g)  
C)   CO(g) + 3H2(g)    CH4(g) + H2O(g)  
D)   CaO(s) + CO2(g)    CaCO3(s)  
E)   HBr(g)    ½H2(g) + ½Br2(l) " class="answers-bank-image d-inline" rel="preload" > ½H2(g) + ½Br2(l)

Question 7

When 0.20 mole HF is dissolved in water to a volume of 1.00 L,5.8% of the HF dissociates to form F-(aq).What is the equilibrium constant for the reaction?

Accepted Answer

A)   1.3  ×	imes×  10-4
B)   7.1  ×	imes×  10-4
C)   1.2  ×	imes×  10-2
D)   1.7  ×	imes×  10-2
E)   6.2  ×	imes×  10-2

Question 8

When 1.0 mole of acetic acid is diluted with water to a volume of 1.0 L at 25 S1U1P1$\circ$S1S1P0C,0.42% of the acetic acid ionizes to form acetate ion and hydronium ion.CH₃CO₂H(aq)+ H₂O( ) CH₃CO₂^-(aq)+ H₃O⁺(aq) What percentage of the acid ionizes when 0.75 mole of acetic acid is diluted with water to 1.0 L at 25 S1U1P1$\circ$S1S1P0C?

Accepted Answer

The answer of When 1.0 mole of acetic acid is...

Question 9

Nitrogen trifluoride decomposes at to form nitrogen and fluorine gases according to the following equation:

6.00-L reaction vessel is initially charged with 1.96 mol of NF3 and allowed to come to equilibrium at 800 K.Once equilibrium is established,the reaction vessel is found to contain 0.0380 mol of N2.What is the value of Kp at this temperature? (R = 0.0821 L.atm.mol.K)

Accepted Answer

A)   1.53  ×	imes×  10-5
B)   1.91  ×	imes×  10-3
C)   1.76  ×	imes×  10-3
D)   1.59  ×	imes×  10-5
E)   4.43  ×	imes×  10-7

Question 10

For the reaction N2O4(g)  2NO2(g),Kp = 0.148 at a temperature of 298 K.What is Kp for the following reaction?
14NO2(g)  7N2O4(g)

Accepted Answer

A)   6.43  ×	imes×  105
B)   1.04
C)   1.56  ×	imes×  10-6
D)   0.965
E)   6.76

Question 11

Write a balanced chemical equation which corresponds to the following equilibrium constant expression.

Accepted Answer

A)   PbF2(aq)  2(aq)    Pb(s) + F2(aq)  
B)   PbF2(s)    Pb2+(aq) + 2 F-(aq)  
C)   Pb2+(aq) + 2 F-(aq)    PbF2(s)  
D)   Pb(s) + F2(aq)    PbF2(aq)  
E)   PbF+(aq) + F-(aq)    PbF2(aq) " class="answers-bank-image d-inline" rel="preload" > Pb(s) + F2(aq) 
B)   PbF2(s)  2(aq)    Pb(s) + F2(aq)  
B)   PbF2(s)    Pb2+(aq) + 2 F-(aq)  
C)   Pb2+(aq) + 2 F-(aq)    PbF2(s)  
D)   Pb(s) + F2(aq)    PbF2(aq)  
E)   PbF+(aq) + F-(aq)    PbF2(aq) " class="answers-bank-image d-inline" rel="preload" > Pb2+(aq) + 2 F-(aq) 
C)   Pb2+(aq) + 2 F-(aq)  2(aq)    Pb(s) + F2(aq)  
B)   PbF2(s)    Pb2+(aq) + 2 F-(aq)  
C)   Pb2+(aq) + 2 F-(aq)    PbF2(s)  
D)   Pb(s) + F2(aq)    PbF2(aq)  
E)   PbF+(aq) + F-(aq)    PbF2(aq) " class="answers-bank-image d-inline" rel="preload" > PbF2(s) 
D)   Pb(s) + F2(aq)  2(aq)    Pb(s) + F2(aq)  
B)   PbF2(s)    Pb2+(aq) + 2 F-(aq)  
C)   Pb2+(aq) + 2 F-(aq)    PbF2(s)  
D)   Pb(s) + F2(aq)    PbF2(aq)  
E)   PbF+(aq) + F-(aq)    PbF2(aq) " class="answers-bank-image d-inline" rel="preload" > PbF2(aq) 
E)   PbF+(aq) + F-(aq)  2(aq)    Pb(s) + F2(aq)  
B)   PbF2(s)    Pb2+(aq) + 2 F-(aq)  
C)   Pb2+(aq) + 2 F-(aq)    PbF2(s)  
D)   Pb(s) + F2(aq)    PbF2(aq)  
E)   PbF+(aq) + F-(aq)    PbF2(aq) " class="answers-bank-image d-inline" rel="preload" > PbF2(aq)

Question 12

Given the following chemical equilibria,
N2(g)+ O2(g)  2 NO(g) $~~~~~~~~$ $~~~~~~~~$ K1
N2(g)+ 3 H2(g)   2 NH3(g)$~~~~~~~~$ $~~  ~~~$ K2
H2(g)+ 1/2 O2(g)  H2O(g)$~~~~~~~~$ $~~~~  ~$ K3
Determine the method used to calculate the equilibrium constant for the reaction below.
4 NH3(g)+ 5 O2(g)  4 NO(g)+ 6 H2O(g)$~~~~~~~~$ K c

Accepted Answer

A)   2(g) + O2(g)    2 NO(g)   ~~~~~~~~   ~~~~~~~~  K1 N2(g) + 3 H2(g)     2 NH3(g)  ~~~~~~~~   ~~  ~~~  K2 H2(g) + 1/2 O2(g)    H2O(g)  ~~~~~~~~   ~~~~  ~  K3 Determine the method used to calculate the equilibrium constant for the reaction below. 4 NH3(g) + 5 O2(g)    4 NO(g) + 6 H2O(g)  ~~~~~~~~  K c 
A)     
B)     
C)     
D)     
E)     " class="answers-bank-image d-inline" rel="preload" >
B)   2(g) + O2(g)    2 NO(g)   ~~~~~~~~   ~~~~~~~~  K1 N2(g) + 3 H2(g)     2 NH3(g)  ~~~~~~~~   ~~  ~~~  K2 H2(g) + 1/2 O2(g)    H2O(g)  ~~~~~~~~   ~~~~  ~  K3 Determine the method used to calculate the equilibrium constant for the reaction below. 4 NH3(g) + 5 O2(g)    4 NO(g) + 6 H2O(g)  ~~~~~~~~  K c 
A)     
B)     
C)     
D)     
E)     " class="answers-bank-image d-inline" rel="preload" >
C)   2(g) + O2(g)    2 NO(g)   ~~~~~~~~   ~~~~~~~~  K1 N2(g) + 3 H2(g)     2 NH3(g)  ~~~~~~~~   ~~  ~~~  K2 H2(g) + 1/2 O2(g)    H2O(g)  ~~~~~~~~   ~~~~  ~  K3 Determine the method used to calculate the equilibrium constant for the reaction below. 4 NH3(g) + 5 O2(g)    4 NO(g) + 6 H2O(g)  ~~~~~~~~  K c 
A)     
B)     
C)     
D)     
E)     " class="answers-bank-image d-inline" rel="preload" >
D)   2(g) + O2(g)    2 NO(g)   ~~~~~~~~   ~~~~~~~~  K1 N2(g) + 3 H2(g)     2 NH3(g)  ~~~~~~~~   ~~  ~~~  K2 H2(g) + 1/2 O2(g)    H2O(g)  ~~~~~~~~   ~~~~  ~  K3 Determine the method used to calculate the equilibrium constant for the reaction below. 4 NH3(g) + 5 O2(g)    4 NO(g) + 6 H2O(g)  ~~~~~~~~  K c 
A)     
B)     
C)     
D)     
E)     " class="answers-bank-image d-inline" rel="preload" >
E)   2(g) + O2(g)    2 NO(g)   ~~~~~~~~   ~~~~~~~~  K1 N2(g) + 3 H2(g)     2 NH3(g)  ~~~~~~~~   ~~  ~~~  K2 H2(g) + 1/2 O2(g)    H2O(g)  ~~~~~~~~   ~~~~  ~  K3 Determine the method used to calculate the equilibrium constant for the reaction below. 4 NH3(g) + 5 O2(g)    4 NO(g) + 6 H2O(g)  ~~~~~~~~  K c 
A)     
B)     
C)     
D)     
E)     " class="answers-bank-image d-inline" rel="preload" >

Question 13

Nitrogen and oxygen gases may react to form nitrogen monoxide.
At 1500 S1U1P1$\circ$S1S1P0C,Kc equals 1.0 $\times$10-5.N2(g)+ O2(g)  2 NO(g)
If 0.030 mol N2 and 0.030 mol O2 are sealed in a 1.0 L flask at 1500 S1U1P1$\circ$S1S1P0C,what is the concentration of NO(g)when equilibrium is established?

Accepted Answer

A)   3.0  ×	imes×  10-7 M
B)   4.7  ×	imes×  10-5 M
C)   9.5  ×	imes×  10-5 M
D)   3.0  ×	imes×  10-2 M
E)   9.1  ×	imes× 101 M

Question 14

At 700 K,Kp for the following equilibrium is 
5.6 $\times$ 10-3.2HgO(s)  2Hg(l)+ O2(g)
Suppose 51.2 g of mercury(II)oxide is placed in a sealed 3.00-L vessel at 700 K.What is the partial pressure of oxygen gas at equilibrium? (R = 0.0821 L · atm/(K · mol))

Accepted Answer

A)   0.075 atm
B)   0.0056 atm
C)   4.5 atm
D)   19 atm
E)   2.3 atm

Question 15

A 10.0-g sample of solid NH4Cl is heated in a 5.00-L container to 900.°C.At equilibrium the pressure of NH3(g)is 1.47 atm.
NH4Cl(s)  NH3(g)+ HCl(g)
The equilibrium constant,Kp,for the reaction is:

Accepted Answer

A)   2.16
B)   7.78
C)   1.47
D)   2.94
E)   none of these

Question 16

The equilibrium constant at 25 S1U1P1$\circ$S1S1P0C for the dissolution of silver iodide is 
8.5 $\times$ 10-17.AgI(s)  Ag+(aq)+ I-(aq)
If an excess quantity of AgI(s)is added to water and allowed to equilibrate,what is the equilibrium concentration of I-?

Accepted Answer

A)   7.2  ×	imes×  10-33 M
B)   4.3  ×	imes×  10-17 M
C)   8.5  ×	imes×  10-17 M
D)   6.5  ×	imes×  10-9 M
E)   9.2  ×	imes×  10-9 M

Question 17

Given the following equilibria,
PbBr2(s)  Pb2+(aq)+ 2 Br-(aq) $~~~~~~~~$ $~~~~~~~~~~~~$ K1 = 6.6 $\times$0 10-6
Pb(OH)2(s)   Pb2+(aq)+ 2 OH-(aq)$~~~~~~~~$ $~~~~~~~~$ K2 = 1.4 $\times$ 10-15
Determine the equilibrium constant,Kc,for the following reaction.
PbBr2(s)+ 2 OH-(aq)  Pb(OH)2(s)+ 2 Br-(aq)

Accepted Answer

A)   9.2  ×	imes×  10-21
B)   2.1  ×	imes×  10-10
C)   6.6  ×	imes×  10-6
D)   4.7  ×	imes×  109
E)   1.1  ×	imes×  1020

Question 18

What balanced equation is the following equilibrium expression derived from?

Accepted Answer

A)   2(g) +   I2(g)      HI(g)  
B)     HI(g)      H2(g) +   I2(g)  
C)     H2(aq) +   I2(aq)      HI(aq)  
D)     HI(aq)      H2(aq) +   I2(aq)  
E)   2HI(g)    H2(g) + I2(g) " class="answers-bank-image d-inline" rel="preload" > H2(g) + 2(g) +   I2(g)      HI(g)  
B)     HI(g)      H2(g) +   I2(g)  
C)     H2(aq) +   I2(aq)      HI(aq)  
D)     HI(aq)      H2(aq) +   I2(aq)  
E)   2HI(g)    H2(g) + I2(g) " class="answers-bank-image d-inline" rel="preload" > I2(g)  2(g) +   I2(g)      HI(g)  
B)     HI(g)      H2(g) +   I2(g)  
C)     H2(aq) +   I2(aq)      HI(aq)  
D)     HI(aq)      H2(aq) +   I2(aq)  
E)   2HI(g)    H2(g) + I2(g) " class="answers-bank-image d-inline" rel="preload" > 2(g) +   I2(g)      HI(g)  
B)     HI(g)      H2(g) +   I2(g)  
C)     H2(aq) +   I2(aq)      HI(aq)  
D)     HI(aq)      H2(aq) +   I2(aq)  
E)   2HI(g)    H2(g) + I2(g) " class="answers-bank-image d-inline" rel="preload" > HI(g) 
B)   2(g) +   I2(g)      HI(g)  
B)     HI(g)      H2(g) +   I2(g)  
C)     H2(aq) +   I2(aq)      HI(aq)  
D)     HI(aq)      H2(aq) +   I2(aq)  
E)   2HI(g)    H2(g) + I2(g) " class="answers-bank-image d-inline" rel="preload" > HI(g)  2(g) +   I2(g)      HI(g)  
B)     HI(g)      H2(g) +   I2(g)  
C)     H2(aq) +   I2(aq)      HI(aq)  
D)     HI(aq)      H2(aq) +   I2(aq)  
E)   2HI(g)    H2(g) + I2(g) " class="answers-bank-image d-inline" rel="preload" > 2(g) +   I2(g)      HI(g)  
B)     HI(g)      H2(g) +   I2(g)  
C)     H2(aq) +   I2(aq)      HI(aq)  
D)     HI(aq)      H2(aq) +   I2(aq)  
E)   2HI(g)    H2(g) + I2(g) " class="answers-bank-image d-inline" rel="preload" > H2(g) + 2(g) +   I2(g)      HI(g)  
B)     HI(g)      H2(g) +   I2(g)  
C)     H2(aq) +   I2(aq)      HI(aq)  
D)     HI(aq)      H2(aq) +   I2(aq)  
E)   2HI(g)    H2(g) + I2(g) " class="answers-bank-image d-inline" rel="preload" > I2(g) 
C)   2(g) +   I2(g)      HI(g)  
B)     HI(g)      H2(g) +   I2(g)  
C)     H2(aq) +   I2(aq)      HI(aq)  
D)     HI(aq)      H2(aq) +   I2(aq)  
E)   2HI(g)    H2(g) + I2(g) " class="answers-bank-image d-inline" rel="preload" > H2(aq) + 2(g) +   I2(g)      HI(g)  
B)     HI(g)      H2(g) +   I2(g)  
C)     H2(aq) +   I2(aq)      HI(aq)  
D)     HI(aq)      H2(aq) +   I2(aq)  
E)   2HI(g)    H2(g) + I2(g) " class="answers-bank-image d-inline" rel="preload" > I2(aq)  2(g) +   I2(g)      HI(g)  
B)     HI(g)      H2(g) +   I2(g)  
C)     H2(aq) +   I2(aq)      HI(aq)  
D)     HI(aq)      H2(aq) +   I2(aq)  
E)   2HI(g)    H2(g) + I2(g) " class="answers-bank-image d-inline" rel="preload" > 2(g) +   I2(g)      HI(g)  
B)     HI(g)      H2(g) +   I2(g)  
C)     H2(aq) +   I2(aq)      HI(aq)  
D)     HI(aq)      H2(aq) +   I2(aq)  
E)   2HI(g)    H2(g) + I2(g) " class="answers-bank-image d-inline" rel="preload" > HI(aq) 
D)   2(g) +   I2(g)      HI(g)  
B)     HI(g)      H2(g) +   I2(g)  
C)     H2(aq) +   I2(aq)      HI(aq)  
D)     HI(aq)      H2(aq) +   I2(aq)  
E)   2HI(g)    H2(g) + I2(g) " class="answers-bank-image d-inline" rel="preload" > HI(aq)  2(g) +   I2(g)      HI(g)  
B)     HI(g)      H2(g) +   I2(g)  
C)     H2(aq) +   I2(aq)      HI(aq)  
D)     HI(aq)      H2(aq) +   I2(aq)  
E)   2HI(g)    H2(g) + I2(g) " class="answers-bank-image d-inline" rel="preload" > 2(g) +   I2(g)      HI(g)  
B)     HI(g)      H2(g) +   I2(g)  
C)     H2(aq) +   I2(aq)      HI(aq)  
D)     HI(aq)      H2(aq) +   I2(aq)  
E)   2HI(g)    H2(g) + I2(g) " class="answers-bank-image d-inline" rel="preload" > H2(aq) + 2(g) +   I2(g)      HI(g)  
B)     HI(g)      H2(g) +   I2(g)  
C)     H2(aq) +   I2(aq)      HI(aq)  
D)     HI(aq)      H2(aq) +   I2(aq)  
E)   2HI(g)    H2(g) + I2(g) " class="answers-bank-image d-inline" rel="preload" > I2(aq) 
E)   2HI(g)  2(g) +   I2(g)      HI(g)  
B)     HI(g)      H2(g) +   I2(g)  
C)     H2(aq) +   I2(aq)      HI(aq)  
D)     HI(aq)      H2(aq) +   I2(aq)  
E)   2HI(g)    H2(g) + I2(g) " class="answers-bank-image d-inline" rel="preload" > H2(g) + I2(g)

Question 19

What is the Kc equilibrium-constant expression for the following equilibrium?

Accepted Answer

A)   c equilibrium-constant expression for the following equilibrium?   
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
B)   c equilibrium-constant expression for the following equilibrium?   
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
C)   c equilibrium-constant expression for the following equilibrium?   
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
D)   c equilibrium-constant expression for the following equilibrium?   
A)     
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Question 20

An aqueous mixture of phenol and ammonia has initial concentrations of 0.200 M C6H5OH(aq)and 0.120 M NH3(aq).At equilibrium,the C6H5O-(aq)concentration is 0.050 M.Calculate K for the reaction.
C6H5OH(aq)+ NH3(aq)  C6H5O- + NH4+(aq)

Accepted Answer

A)   0.10
B)   0.24
C)   2.1
D)   4.2
E)   4.8

Exam 16: Principles of Reactivity: Chemical Equilibria

In which of the following reactions does a decrease in the volume of the reaction vessel at constant temperature favor formation of the products?

For which of the following equilibria does K_c = K_p?

Write a balanced chemical equation which corresponds to the following equilibrium constant expression.

A 10.0-g sample of solid NH₄Cl is heated in a 5.00-L container to 900.°C.At equilibrium the pressure of NH₃(g) is 1.47 atm. NH₄Cl(s) NH₃(g) + HCl(g) The equilibrium constant,K_p,for the reaction is:

What balanced equation is the following equilibrium expression derived from?

What is the K_c equilibrium-constant expression for the following equilibrium?

An aqueous mixture of phenol and ammonia has initial concentrations of 0.200 M C₆H₅OH(aq) and 0.120 M NH₃(aq) .At equilibrium,the C₆H₅O^-(aq) concentration is 0.050 M.Calculate K for the reaction. C₆H₅OH(aq) + NH₃(aq) C₆H₅O^- + NH₄⁺(aq)

Exam 16: Principles of Reactivity: Chemical Equilibria

The following reaction occurred when a 1.0-liter reaction vessel was initially charged with 2.0 moles of N2(g) and 4.0 moles of H2(g) : Once equilibrium was established,the concentration of NH3(g) was determined to be 0.59 M at 700.°C.The value for Kc at 700.°C for the formation of ammonia is:

In which of the following reactions does a decrease in the volume of the reaction vessel at constant temperature favor formation of the products?

Consider the following equilibrium: PCl5(g) PCl3(g) + Cl2(g) ; ~~~~~~~~ Δ\DeltaΔ H = 92 kJ The concentration of PCl3 at equilibrium may be increased by

For which of the following equilibria does Kc = Kp?

When 0.20 mole HF is dissolved in water to a volume of 1.00 L,5.8% of the HF dissociates to form F-(aq) .What is the equilibrium constant for the reaction?

For the reaction N2O4(g) 2NO2(g) ,Kp = 0.148 at a temperature of 298 K.What is Kp for the following reaction? 14NO2(g) 7N2O4(g)

Write a balanced chemical equation which corresponds to the following equilibrium constant expression.

Nitrogen and oxygen gases may react to form nitrogen monoxide. At 1500 ∘\circ∘ C,Kc equals 1.0 ×\times× 10-5.N2(g) + O2(g) 2 NO(g) If 0.030 mol N2 and 0.030 mol O2 are sealed in a 1.0 L flask at 1500 ∘\circ∘ C,what is the concentration of NO(g) when equilibrium is established?

At 700 K,Kp for the following equilibrium is 5.6 ×\times× 10-3.2HgO(s) 2Hg(l) + O2(g) Suppose 51.2 g of mercury(II) oxide is placed in a sealed 3.00-L vessel at 700 K.What is the partial pressure of oxygen gas at equilibrium? (R = 0.0821 L · atm/(K · mol) )

A 10.0-g sample of solid NH4Cl is heated in a 5.00-L container to 900.°C.At equilibrium the pressure of NH3(g) is 1.47 atm. NH4Cl(s) NH3(g) + HCl(g) The equilibrium constant,Kp,for the reaction is:

The equilibrium constant at 25 ∘\circ∘ C for the dissolution of silver iodide is 8.5 ×\times× 10-17.AgI(s) Ag+(aq) + I-(aq) If an excess quantity of AgI(s) is added to water and allowed to equilibrate,what is the equilibrium concentration of I-?

Given the following equilibria, PbBr2(s) Pb2+(aq) + 2 Br-(aq) ~~~~~~~~ ~~~~~~~~~~~~ K1 = 6.6 ×\times× 0 10-6 Pb(OH) 2(s) Pb2+(aq) + 2 OH-(aq) ~~~~~~~~ ~~~~~~~~ K2 = 1.4 ×\times× 10-15 Determine the equilibrium constant,Kc,for the following reaction. PbBr2(s) + 2 OH-(aq) Pb(OH) 2(s) + 2 Br-(aq)

What balanced equation is the following equilibrium expression derived from?

What is the Kc equilibrium-constant expression for the following equilibrium?

An aqueous mixture of phenol and ammonia has initial concentrations of 0.200 M C6H5OH(aq) and 0.120 M NH3(aq) .At equilibrium,the C6H5O-(aq) concentration is 0.050 M.Calculate K for the reaction. C6H5OH(aq) + NH3(aq) C6H5O- + NH4+(aq)

For which of the following equilibria does K_c = K_p?

A 10.0-g sample of solid NH₄Cl is heated in a 5.00-L container to 900.°C.At equilibrium the pressure of NH₃(g) is 1.47 atm. NH₄Cl(s) NH₃(g) + HCl(g) The equilibrium constant,K_p,for the reaction is:

What is the K_c equilibrium-constant expression for the following equilibrium?

An aqueous mixture of phenol and ammonia has initial concentrations of 0.200 M C₆H₅OH(aq) and 0.120 M NH₃(aq) .At equilibrium,the C₆H₅O^-(aq) concentration is 0.050 M.Calculate K for the reaction. C₆H₅OH(aq) + NH₃(aq) C₆H₅O^- + NH₄⁺(aq)