We’re being asked to determine the ΔH° using the provided data in the graph
This means we need to use the two-point form of the Arrhenius Equation:
K1 = equilibrium constant at T1
K2 = equilibrium constant T2
ΔH° = standard enthalpy
R = gas constant (8.314 J/mol•K)
T1 and T2 = temperature (in K).
The temperature dependence of the equilibrium constant (Kp) is illustrated for the following reaction:
NH4ClO4(s) → NH3(g) + HClO4(g)
Note: the points are labeled as (1/T • 103, lnKp).
Answer the following questions relating to the plot shown above:
Calculate ΔH° (in kJ/mol) for the reaction given above. You may assume that ΔH° and ΔS° are temperature independent. Show all work and circle your final answer.
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