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
Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.
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.
Write equilibrium constant (K) expressions for the following reactions: C and D
C: 4NO2 (g) + 6H2O (g) ---> <---- 4NH3 (g) + 7O2 (g)
D: attached Below
![### Equilibrium Constant Expression
Given the chemical reaction:
\[ \text{NH}_3(g) + \text{HCl}(g) \leftrightarrow \text{NH}_4\text{Cl}(s) \]
Determine the correct expression for the equilibrium constant \( K \).
**Options:**
1. \( K = \frac{P_{\text{NH}_4\text{Cl}}}{(P_{\text{NH}_3})(P_{\text{HCl}})} \)
2. \( K = P_{\text{NH}_3} \)
3. \( K = \frac{(P_{\text{NH}_3})(P_{\text{HCl}})}{P_{\text{NH}_4\text{Cl}}} \)
4. \( K = \frac{1}{(P_{\text{NH}_3})(P_{\text{HCl}})} \)
5. \( K = (P_{\text{NH}_3})(P_{\text{HCl}}) \)
6. \( K = \frac{1}{P_{\text{NH}_3}} \)
### Explanation of Symbols
- \( P_{\text{NH}_3} \): Partial pressure of ammonia gas \( \text{NH}_3 \).
- \( P_{\text{HCl}} \): Partial pressure of hydrogen chloride gas \( \text{HCl} \).
- \( P_{\text{NH}_4\text{Cl}} \): Partial pressure of ammonium chloride \( \text{NH}_4\text{Cl} \) (however, since \( \text{NH}_4\text{Cl} \) is a solid, its activity is considered constant and does not appear in the equilibrium expression).
### Understanding the Equilibrium Constant, \( K \)
The equilibrium constant, \( K \), for the reaction involving gases is generally given by the ratio of the partial pressures (or concentrations, in case of solutions) of the products to the reactants, each raised to the power of their respective coefficients in the balanced chemical equation.
Since \( \text{NH}_4\text{Cl} \) is a solid, it does not appear in the expression for the equilibrium constant for this reaction. Therefore, the correct expression for the equilibrium constant \( K \) is:
\[ K = \frac{1}{(P_{\text{NH}_3})(P_{\text{H](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fdba2aaf3-9d4f-48e5-a260-55d7aa0dddc9%2F01fd13bc-613d-45f1-a270-c8a09ac71333%2Fofqtos_processed.jpeg&w=3840&q=75)
Step by step
Solved in 2 steps with 2 images
