The equllibrium constant `K_c` for the reaction. `N_2O_4 hArr2NO_2(g)` `"is" 4.63xx10^(-3) "at" 25^@C` (i) What is the value of `K_p` at this temperature. (ii) At `25^@C` , if partial pressure of `N_2O_4(g)` at equllibrium is 0.20 atm, calculate equilibrium pressure of `NO-2`
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To solve the problem step by step, we will address both parts of the question: (i) calculating the value of \( K_p \) and (ii) calculating the equilibrium pressure of \( NO_2 \).
### Step 1: Calculate \( K_p \) using the relation between \( K_c \) and \( K_p \)
The relationship between \( K_p \) and \( K_c \) is given by the formula:
\[
K_p = K_c \cdot R \cdot T^{\Delta N_g}
...
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