Enter your answer in the provided box. For reactions carried out under standard-state conditions, the equation ΔG = ΔH − TΔS becomes ΔG o = H o − TΔS o . Assuming ΔH o and ΔS o are independent of temperature, one can derive the equation: ln K2 K1 = ΔH o R ( T2 − T1 T1T2 ) where K1 and K2 are the equilibrium constants at T1 and T2, respectively. Given that at 25.0°C, Kc is 4.63 × 10−3 for the reaction N2O4(g) ⇆ 2NO2(g) ΔH o = 58.0 kJ/mol calculate the equilibrium constant at 49.0°C. Kc =
It is given that the equilibrium constant for the reaction
We have to find out
We are given for the above reaction.
Now, the equilibrium constants at two different temperatures are related as follows:
Hence, putting in the values, we can calculate the value of equilibrium constant at 49.0 C as follows:
Hence, the equilibrium constant Kc at 49.0 C is about . (Rounded to three significant figures).
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