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2 cards from this section. Quick, good the night before a test.
What happens to the value of K when temperature increases for an endothermic reaction?
Remember the heat absorption in endothermic processes.
Define the term equilibrium constant.
Think about the relationship of products and reactants.
What does an increase in temperature do to the equilibrium constant K for an endothermic reaction?
Think about heat absorption.
True or False: The equilibrium constant K is constant across all temperatures.
Remember the relationship between temperature and equilibrium.
Consider the equilibrium N2(g) + 3H2(g) ⇌ 2NH3(g) with ΔH = -92 kJ. Predict how K changes as temperature is raised from 400°C to 600°C.
Review how exothermic reactions behave with increasing temperatures.
Given ΔG° = -10.2 kJ for the reaction CO(g) + 2H2(g) ⇌ CH3OH(g) at 298 K, calculate the predicted value of K.
Use the connection of ΔG with K.
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