Question

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 =

Answer #1

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 K _{c} at 49.0 C
is about
.**

ADVERTISEMENT

Get Answers For Free

Most questions answered within 1 hours.

ADVERTISEMENT

asked 5 minutes ago

asked 20 minutes ago

asked 20 minutes ago

asked 28 minutes ago

asked 35 minutes ago

asked 48 minutes ago

asked 52 minutes ago

asked 52 minutes ago

asked 54 minutes ago

asked 54 minutes ago

asked 54 minutes ago

asked 54 minutes ago