Math Problem Statement
4 NO2(g) + O2(g) equilibrium reaction arrow 2 N2O5(g) Kp = 7.66 ✕ 10−6 at 25°CConvert the values of Kc to values of Kp or the values of Kp to values of Kc.
Solution
To convert between the equilibrium constants (based on partial pressures) and (based on concentrations) for a gas-phase reaction, we use the following formula:
Where:
- is the equilibrium constant in terms of pressure.
- is the equilibrium constant in terms of concentration.
- is the gas constant ().
- is the temperature in Kelvin (for 25°C, ).
- is the change in the number of moles of gas, calculated as:
Step 1: Calculate
The balanced reaction is:
- Moles of gaseous products = 2 (from )
- Moles of gaseous reactants = 4 + 1 = 5 (from and )
So, .
Step 2: Rearrange the formula to solve for
Step 3: Plug in the values
Now, calculate:
Let me calculate this for you.The value of is approximately 0.112 at 25°C.
Would you like further details or have any questions?
Here are 5 related questions to deepen understanding:
- How does the change in temperature affect the relationship between and ?
- What happens to the equilibrium position if the pressure of this reaction is increased?
- Can you explain why affects the relationship between and ?
- What are the typical units of and , and how do they differ?
- How would you calculate if were given instead?
Tip: Always remember that temperature must be in Kelvin when using gas laws or equilibrium constants.
Ask a new question for Free
By Image
Drop file here or Click Here to upload
Math Problem Analysis
Mathematical Concepts
Equilibrium Constants
Gas Laws
Chemical Kinetics
Formulas
Kp = Kc (RT)^Δn
Kc = Kp / (RT)^Δn
Theorems
Ideal Gas Law
Suitable Grade Level
Grades 11-12 (Advanced Chemistry)
Related Recommendation
Equilibrium Constant for the Reaction 4NO + 3O2 ↔ 2N2O5
Equilibrium Calculations for NO2 and N2O4 Reaction at 200°C
Equilibrium Constant (Kc) Calculation for 2CO + 2NO ⇌ 2CO2 + N2
Calculate Equilibrium Pressure of NO for Reaction 2 NO₂ ⇌ 2 NO + O₂
Equilibrium Problem: Calculating Molarity Changes for NO2 and NO Reaction