a. For the reaction H2 (9) + I2(a) 2HI(9) Standard free energy kJ b. For the reaction 2HB1(g)H2 (9) + Brz(9) Standard free energy kJ

H2CO (g) = 219.0 O2 (g) = 205.1 CO2 (g) = 213.7 H2O (l) = 69.9

Use standard thermodynamic data to calculate G at 298.15 K for the following reaction, assuming that all gases have a pressure of 20.46 mm Hg.2NO(g) + O2(g)2NO2(g)  G =  ______kJ/mol

A chemical engineer is studying the two reactions shown in the table below. In each case, he fills a reaction vessel with some mixture of the reactants and products at a constant temperature of 63.0 °C and constant total pressure. Then, he measures the reaction enthalpy AH and reaction entropy AS of the first reaction, and the reaction enthalpy AH and reaction free energy AG of the second reaction. The results of his measurements are shown in the table. Complete the table. That is, calculate AG for the first reaction and AS for the second. (Round your answer to zero decimal places.) Then, decide whether, under the conditions the engineer has set up, the reaction is spontaneous, the reverse reaction is spontaneous, or neither forward nor reverse reaction is spontaneous because the system is at equilibrium.

Given the dissociation of methane to graphite (C) and hydrogen gas. For the methane at 298K, Given the following data: kJ = -74.85- mol = -80.67 mol · K A,GE.graphite = A,Gån = 0 %3D Solve the following: a. Calculate the equilibrium constant (K) of the dissociation of methane at 298K with the appropriate units. b. Assuming that enthalpy is independent of temperature, Calculate the equilibrium constant (K) of methane dissociation at 1000 K. C. Calculate the ratio between the amounts of methane and hydrogen gas at 298 K and 0.2 bar.

What is true about the following reaction at 25°C? H₂(g) + 2BrF(g) = 2HBr(g) + F₂(g) \Delta Hr\ deg = 115 kJ mol-¹ \Delta Sr\deg = 11.55 J mol-¹ K-¹ \Delta Gr\deg = 111 kJ mol-¹ i. The reaction is endothermic. ii. As the reaction proceeds heat is transferred from the surroundings to the system.

1.Provide an explanation for  why  B2H6(g) /BH3(g) spontaneously reacts and ignites in air , but  CH4 (g) persists in the presence of air indefinitely. 2.The standard state for elementary antimony is the tetrameric  molecular solid ( Sb4(s)) .    The standard enthalpies of vaporization and atomization for one gram atom (121.76g)  of elemental antimony   are 68 kj and 264 kj  per mole of antimony atoms respectively . What is the average effective   Sb-Sb bond dissociation enthalpy  for the standard state of antimony .