1 for the reaction 2nas 2h2ol2naohaq h2g h 369 kj and s 153 jk the equilibrium constant k would

Step 1: Calculate the temperature in Kelvin using the formula: T = (-ΔH° / ΔS°) * 10^3

Question

1. For the reaction 2Na(s) + 2H2O(l) → 2NaOH(aq) + H2(g) ΔH° = -369 kJ and ΔS° = -15.3 J/K The equilibrium constant, K, would be greater than 1 at temperatures _ above/below Kelvin. Select above or below in the first box and enter the temperature in the second box. Assume that ΔH° and ΔS° are constant. 2. For the reaction CO(g) + Cl2(g) → COCl2(g) ΔH° = -108 kJ and ΔS° = -137 J/K The equilibrium constant, K, would be greater than 1 at temperatures _ above/below Kelvin. Select above or below in the first box and enter the temperature in the second box. Assume that ΔH° and ΔS° are constant.

          1. For the reaction
2Na(s) + 2H2O(l) → 2NaOH(aq) + H2(g)
ΔH° = -369 kJ and ΔS° = -15.3 J/K
The equilibrium constant, K, would be greater than 1 at temperatures _______ above/below Kelvin.
Select above or below in the first box and enter the temperature in the second box. Assume that ΔH° and ΔS° are constant.

2. For the reaction
CO(g) + Cl2(g) → COCl2(g)
ΔH° = -108 kJ and ΔS° = -137 J/K
The equilibrium constant, K, would be greater than 1 at temperatures _______ above/below Kelvin.
Select above or below in the first box and enter the temperature in the second box. Assume that ΔH° and ΔS° are constant.

Added by Connie H.

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