E6B.3(b) The standard enthalpy of a certain reaction is approximately constant at +125 kJ mol from 800 K up to 1500 K. The standard reaction Gibbs e is +22 kJ molat 1120 K. Estimate the temperature at which the equilibrium energy constant becomes greater than 1.

Suppose you have an exothermic reaction with H = 15 kJ and a S of +150 J/K. Calculate G and Keq at 10, 100, and 1000 K.

Given the following data: PtCl42(aq)+2ePt(s)+4Cl(aq)Ered=0.73VPt2+(aq)+2ePt(s)Ered=1.20V Find Kffor PtCl42- at 25°C.

At a certain temperature, K=0.29 for the decomposition of two moles of iodine trichloride, ICl3(s), to chlorine and iodine gases. The partial pressure of chlorine gas at equilibrium is three times that of iodine gas. What are the partial pressures of iodine and chlorine at equilibrium?

Describe a nonchemical system that is not in equilibrium, and explain why equilibrium has not been achieved.

The equilibrium constant for the gas-phase isomerization of borneol, C10H17OH, to isoborneol at 503 K is 0.106. A mixture consisting of 6.70 g of borneol and 12 .5 g of isoborneol in a container of volume 5.0 dm3 is heated to 503 K and allowed to come to equilibrium. Calculate the mole fractionsof the two substances at equilibrium.

At 298 K, the equilibrium constant for the reaction Fe,O3(s) + 3 H2(g) 2 2 Fe(s) + 3 H¿O(€) is 4.0 × 10-6, and that for CO2(g) + H2(g) 2 CO(g) + H,O(€) is 3.2 x 10-4. Suppose some solid Fe,O3, solid Fe, and liquid H2O are brought into equilibrium with CO(g) and CO2(g) in a closed container at 298 K. Calculate the ratio of the partial pressure of CO(g) to that of CO2(g) at equilibrium.

It is determined that a particular chemical reaction has AH° = 42.2 kJ mol 1 and Aso, | = 124.5 JK-1 mol 1. rxn rxn Determine the equilibrium constant for the reaction, K, at 298 K.

The decomposition of a generic diatomic element in its standard state is represented by the equation....

Please don't provide handwritten solution ....