Calculate the number of moles of HI that are at equilibrium with 1.25 mol of H₂ and 1.25 mol of 12 in a 5.00-L flask at 448 °C. H₂+12=2HI Kc = 50.2 at 448 °C
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 Calculation Example
**Problem Statement:**
Calculate the number of moles of HI that are at equilibrium with 1.25 mol of H₂ and 1.25 mol of I₂ in a 5.00-L flask at 448 °C.
The balanced chemical equation for the reaction is:
\[ \text{H}_2 + \text{I}_2 \rightleftharpoons 2\text{HI} \]
The equilibrium constant (\( K_c \)) for this reaction at 448 °C is given as:
\[ K_c = 50.2 \text{ at 448 °C} \]
In this problem, we need to find the equilibrium concentration of HI in the flask.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Ff90913a8-510d-485a-8226-8a0b61f2c858%2Fb03c265b-cc96-4cad-9498-81438b4c756f%2F5k8bjqd_processed.png&w=3840&q=75)
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