The kinetics and equilibrium of the decomposition of hy-drogen iodide have been studied extensively:2HI(g)⇌ H₂(g)+I₂(g) (a) At 298 K, K꜀=1.26X10⁻³ for this reaction. Calculate Kₚ.(b) Calculate K꜀ for the formationof HI at 298 K.(c) Calculate ΔH°ᵣₓₙ for HI decomposition from H°f values. (d) At 729 K, K꜀ =2.0X10⁻² for HI decomposition. Calculate ΔHᵣₓₙ for this reaction from the van’t Hoff equation.

10. Use data from your textbook’s appendix to determine ΔG° for the following reaction at 549 K and standard conditions:CH2O(g) + 2 H2(g) ⇌ CH4(g) + H2O(g).(a) 193.7 kJ (b) ‒193.7 kJ (c) 5.749×104 kJ (d) ‒150.1 kJ 11. Determine the equilibrium constant (K) for the reaction in the problem above. CH2O(g) + 2 H2(g) ⇌ CH4(g) + H2O(g).(a) 481 (b) 1.07×109 (c) 2.08×10‒3 (d) 1.87×1014                        CH2O(g) + 2 H2(g) ⇌ CH4(g) + H2O(g). H(kJ/mol)       -108.6        0             -74.6         -241.8 S (J.mol k)       218.8         130.7       186.3          188.8

The equilibrium constant, K,, for the following reaction is 0.160 at 298 K. 2NOBr(g) 2NO(g) + Br2(g) If AH° for this reaction is 16.1 kJ, what is the value of K, at 420 K? Kp =

Consider the following reaction: PBCO3(s) = PbO(s) + CO2(g) Part A Using data in Appendix C in the textbook, calculate the equilibrium pressure of CO2 in the system at 380 ° C. Express your answer using two significant figures.