If the following reaction at 698 K has equilibrium concentration values of 0.584 M HI, 0.0793 M H₂, and 0.0793 M 12, what is the value of the equilibrium constant? 2H1 H₂(g) + 1₂ (g) 2 (0.584m) → 0.0793 M + 0.0793 M L -3
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.
![**Equilibrium Constant Calculation for the Reaction 2HI ⇌ H₂ + I₂**
**Problem Statement:**
At 698 K, the equilibrium concentrations for the reaction 2HI (g) ⇌ H₂ (g) + I₂ (g) are given as:
- [HI] = 0.584 M
- [H₂] = 0.0793 M
- [I₂] = 0.0793 M
**Objective:**
Calculate the equilibrium constant (Kc) for this reaction.
**Solution:**
1. **Balanced Reaction:**
\[
2HI (g) \rightarrow H₂ (g) + I₂ (g)
\]
2. **Expression for the Equilibrium Constant (Kc):**
\[
Kc = \frac{[H₂][I₂]}{[HI]^2}
\]
3. **Substitute the Equilibrium Concentrations into the Expression:**
- [HI] = 0.584 M
- [H₂] = 0.0793 M
- [I₂] = 0.0793 M
\[
Kc = \frac{(0.0793)(0.0793)}{(0.584)^2}
\]
4. **Calculate:**
\[
Kc = \frac{0.0793 \times 0.0793}{0.584^2}
\]
\[
Kc = \frac{0.00628049}{0.341056} \approx 5.80 \times 10^{-3}
\]
**Conclusion:**
The equilibrium constant \( Kc \) for the reaction at 698 K is approximately \( 5.80 \times 10^{-3} \).](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fb0ffec19-af41-4c50-af1b-66e883fc2bb8%2F749d85d8-20d7-41da-b4b6-3091796ab1ae%2Fyk1tmi8_processed.jpeg&w=3840&q=75)
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