An aqueous mixture of hydrocyanic acid and ammonia has initial concentrations of 0.100 M HCN (aq) and 0.140 M NH3 (aq). At equilibrium, the CN (aq) concentration is 0.055 M. Calculate k for the reaction. HCN (aq) + NH3(aq) = CN (aq) + NH4 (aq).
Ionic Equilibrium
Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.
Arrhenius Acid
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Bronsted Lowry Base In Inorganic Chemistry
Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.
![5. Consider the reaction A(aq) = 2 B(aq) where K = 4.1 at 25 °C, If 0,50 M A(aq) and 1.5 M B(aq) are
CHEM 102
Equilibrium Study Guide
initially present in a 1.0 L flask at 25 °C. what change in concentrations (if any) will occur in time?
a. [A] will decrease and [B] will decrease.
76. [A] will decrease and [B] will increase.
c. [A] will increase and [B] will decrease.
d.
= [4 51
[0.50]
Q>Kc
[A] will increase and [B] will increase.
[A] and [B] remain unchanged.
e.
6. An aqueous mixture of hydrocyanie acid and ammonia has initial concentrations of 0.100 M HCN(aq) and
0.140 M NH3(aq). At equilibrium, the CN (ag) concentration is 0.055 M. Calculate K for the reaction.
HCN(aq) + NH3(aq) = CN (aq) + NH,"(aq)
0.22
a.
b.
0.79
с.
1.5
d. 3.9
e.
14
7. Nitrosyl bromide decomposes according to the chemical equation below.
2 NOBr(g) = 2 NO(g) + Br2(g)
When 0.260 atm of NOBR is sealed in a flask and allowed to reach equilibrium, 22% of the NOBr
decomposes. What is the equilibrium constant, Kp, for the reaction?
2.3 x 10-3
b. 4.5 x 10-3
3.5 x 10-2
a.
с.
d.
4.8 x 10-2
e. 8.0 x 10-2
8. The equilibrium constant, Ke, for the following reaction is 1.0 x 10-5 at 1500 K.
N2(g) + O2(g) =2 NO(g)
If 0.570 M N2 and 0.570 M O2 are allowed to equilibrate at 1500 K, what is the concentration of NO?
5.7 x 106 M
b. 9.0 x 104 M
a.
c. 2.4 x 104 M
d. 1.8 x 10-3 M
e. 2.4 x 103 M
9. The equilibrium constant (Ke) for the following reaction is 6.7 x 10-10 at 630 °C.
N2(s) + O2(g) =2 NO(g)
What is the equilibrium constant for the reaction below at the same temperature?
NO(g) = 1/2 N2(g) + 1/2 O2(g)
a. 3.9 x 104
b. 5.5 x 104
c. 7.5 x 10%
d. 1.5 x 10°
e. 3.0 x 10°](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F325a91f3-8d85-4e09-afe5-577f0476af29%2F54db2799-cbe3-4e0c-8d2c-278e5eeacc19%2Fkyxhnw_processed.jpeg&w=3840&q=75)
Given: Initial concentration of HCN= 0.100M
Initial concentration of NH3= 0.140M
At equilibrium CN- concentration is 0.055M
To find: K for the reaction
Solution: Equilibrium constant for a reaction is the ratio of concentration of products to that of reactants with there coefficient as powers.
Equilibrium constant is denoted by K.
If equilibrium constant is greater than 1 the reaction will go in forward direction and will favour the formation of products.
If equilibrium constant is lesser than 1 the reaction will go in backward direction and will favour the formation of reactants.
If the equilibrium constant is equal to 1 than it is said to be in equilibrium with each other.
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