Increasing temperature in system of dynamic equilibrium

According to the article Summary of Le Chatelier's Principle on dynamicscience.com.au, for the process

$$\ce{N2(g) + 3 H2(g) <=> 2 NH3(g)}\quad ΔH = \pu{-92 kJ/mol}$$

the forward reaction is exothermic, while the reverse reaction is endothermic.

If the forward reaction is exothermic, increasing temperature decreases $$K,$$ because it drives the equilibrium backwards, in order to absorb the heat energy.

However, in the graph, there is an abrupt change in the reaction rate of forward and reverse reactions. Why does the forward (exothermic) reaction rate rise up so abruptly, while the reverse (endothermic) reaction does not go up so high?

Shouldn't it clearly be the opposite, as increasing temperature favors the reverse reaction?

• Dont try to learn chemistry off dodgy websites ;) – Karl Nov 26 '19 at 21:14