Answer:
A) 5.83*10^-2
Explanation:
The information given from the exercise is:
- Kp value: 1.45x10^-5
- Temperature (T): 500°C
- Chemical reaction
We can calculate the value of Kc by replacing the values of R (gas constant: 0.082 atm*L/mol*K), temperature (T) and Δn in the Kp formula:
[tex]K_p=K_c*(R*T)^{\Delta n}[/tex]
In this formula, Δn is the result of the difference between the products coefficients and the reactants ccoefficents:
[tex]\begin{gathered} \Delta n=n_{products}-n_{reactants} \\ \Delta n=2-4 \\ \Delta n=-2 \end{gathered}[/tex]
It is important to convert the unit of temperature from °C to K:
[tex]500\text{ + }273=773K[/tex]
Now we can replace the values:
[tex]\begin{gathered} K_p=K_c*(R*T)^{\Delta n} \\ 1.45*10^{-5}=K_c*(0.082*773)^{(-2)} \\ 1.45*10^{-5}=K_c*(2.48*10^{-4}) \\ \frac{1.45*10^{-5}}{2.48*10^{-4}}=K_c \\ 5.83*10^{-2}=K_c \end{gathered}[/tex]
So, the value of Kc is 5.83*10^-2.
