The standard free energy change (ΔG°) for 50% dissociation of N2O4 into NO2 at 27 °C and 1 atm pressure is −x J mol−1 . The value of x

For the reactionN2O4⇌2NO2(g), the degree of dissociation at equilibrium is 0.2 at 1 atm. ThenKpwill be1/21/41/6

The standard heat of formation of N2H4(g) is 62 kJ mol−1. Then the bond energy of N≡N is _____Given: The bond dissociation energies of N−N,H−H and N−H bonds are 159 kJ mol−1,436 kJ mol−1,398 kJ mol−1 respectively.

The following reaction is performed at 298 K. 2NO(g) + O2(g) ⇌ 2NO2(g), Kp = 1.6 × 1012The standard free energy of formation of NO(g) is 86.6 kJ/mol at 298 K. What is the standard free energy of formation of NO2(g) (in J mol–1) at 298 K ?

alculate the standard free energy change at 25°C for the reaction2 NO(g) + O2(g) → 2 NO2(g).Group of answer choices-532.6 kJ-157.8 kJ-4.7 kJ-72.6 kJ

The equilibria between NO2 and N2O4 is provided below:N2O4(g) ⇌ 2NO2(g)Fill in the table based on the observed colour change of your NO2/N2O4 mixture in response to changes in temperature.Colour change Forward/reverse reaction favouredLow temperature High temperature