It's easy to confuse changes in Keq, an expression of equilibrium ratios, with changes in reaction rates and vice versa. An easy way to always get these questions write is to jot down the Keq and rate law for a given reaction.

Octane(g) + Oxygen(gas) ----> Water(l) + Carbon Dioxide(g) + Heat

Keq = CO2 / ( [octane] * [oxygen] )

What will happen to the rate if theirs an increase in temperature? Rate always increases with temperature. An increase in T will cause reaction molecules to have kinetic energy, making them move faster. If they move faster, they collide much more, and so the rate will increase.

bonus- What direction will the rate increase be seen? (at bottom)

What will happen to Keq? Heat will cause the equilibrium to shift lift (For more practice look up LeChateliers principle). Heat is on the right side of the equation, and so creating more heat would unbalance the equation by putting "too much" on the right side. This would cause the reaction rate to INCREASE in the REVERSE direction (otherwise known as a leftward shift).

bonus answer: BOTH directions!

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