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The value of K for the reaction O(3)(g...

The value of K for the reaction
`O_(3)(g)+OH(g) hArr H(g)+2O_(2)(g)`
Changed from `0.096` at `298 K` to `1.4` at `373 K`. Above what temperature will the reaction become thermodynamically spontaneous in the forward direction assuming that `DeltaH^(ɵ)` and `DeltaS^(ɵ)` values for the reaction do not change with change in temperature? Given that `DeltaS_(298)^(ɵ)=10.296 J K^(-1)`.

Text Solution

AI Generated Solution

To determine the temperature above which the reaction becomes thermodynamically spontaneous in the forward direction, we can follow these steps: ### Step 1: Use the Van 't Hoff Equation We start with the Van 't Hoff equation, which relates the change in the equilibrium constant (K) with temperature (T) and the enthalpy change (ΔH) of the reaction: \[ \log \frac{K_2}{K_1} = \frac{\Delta H}{2.303 R} \left( \frac{1}{T_1} - \frac{1}{T_2} \right) \] ...
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