Ammonia is prepared industrially by the following reaction: N2(g) + 3H2(g) ⇌ 2NH3(g)    ΔH° = –92.2 kJ/mol For this reaction, K = 4.0×108 at 25°C. When the temperature of the reaction is increased to 500°C, which of the following statements is true? Select one: No shift will occur since heat is not included in the equilibrium expression. The equilibrium constant will increase. The partial pressure of N2 will increase. Product formation is favoured. The value of K will not change.

Consider the following chemical equilibrium: A(s) +  B(g) ⇄ 3 C(s) + 4 D(g) If the initial pressure of B is 4.26 bar, the total pressure at equilibrium is 7.15 bar. Use these pressures to calculate Keq.

Phosphorous pentachloride decomposes according to the reaction PCl5(g)↽−−⇀PCl3(g)+Cl2(g)PCl5⁢(g)⁢↽−−⇀⁢PCl3⁢(g)+Cl2⁢(g) A 13.1 gsample of PCl5 is added to a sealed 1.25 L flask and the reaction is allowed to come to equilibrium at a constant temperature. At equilibrium, 48.4% of the PCl5 remains. What is the equilibrium constant, Kc , for the reaction?

Nitrosyl bromide decomposes to NO and Br2 in an endothermic process (A,H° = 16.3 kJ/mol-rxn). 2 NOBr(g) ⇒ 2 NO(g) + Br2 (g) Predict the effect of the following changes on the position of the equilibrium; that is, state which way the equilibrium will shift (left, right, or no change) when each of the following changes is made. a. adding more NOBr(g) shift left shift right O no change b. adding more Br₂(g) shift left shift right O no change c. increasing the volume of the reaction flask shift left shift right O no change d. lowering the temperature shift left shift right O no change

Calculate AGO at 600. K for using the following data: AGO = H₂O(g) + 1/2O₂(g) → H₂O2(g) H₂(g) + O₂(g) → H₂O2(g) K = 1.8 × 10³7 at 600. K 2H2(g) + O₂(g) → 2H₂O(g) K = 2.3 × 106 at 600. K kJ/mol

A mixture of gaseous CO and H2, called synthesis gas, is used commercially to prepare methanol (CH3OH), a compound considered an alternative fuel to gasoline. Under equilibrium conditions at 565.3 K,[H2] = 0.07911 mol/L, [CO] = 0.03125 mol/L, and [CH3OH] = 0.0401 mol/L. What is the value of K. for this reaction at 565.3 K?

demonstrate an understanding of the concept of dynamic equilibrium and the variables that cause shifts in the equilibrium of chemical systems.

The steam reforming reaction of methane follows this chemical equation: CHA(g) + H50(g) - CO(g) + 3 H2(g) A H° = +193 kJ/mol At 298 K the reaction lies far to the reactant side with a very small equilibrium constant of 2.35 × 10-23. To obtain a significant amount of the desired hydrogen gas product, the reaction is operated at very high temperatures. What is the equilibrium constant at 1100 K?