This reaction is exothermic. C6H12O6(s) + 6 O2(g) ⇌ 6 CO2(g) + 6 H2O(g). Predict the effect (shift right, shift left, or no effect) of increasing and decreasing the reaction temperature. How does the value of the equilibrium constant depend on temperature?

Verified step by step guidance

1. Identify that the reaction is exothermic, meaning it releases heat as a product.
2. Apply Le Chatelier's Principle, which states that if a system at equilibrium is disturbed, it will shift in a direction that counteracts the disturbance.
3. Consider the effect of increasing temperature: Since heat is a product in an exothermic reaction, increasing temperature adds more 'product', causing the equilibrium to shift to the left to consume the excess heat.
4. Consider the effect of decreasing temperature: Removing heat from the system will cause the equilibrium to shift to the right to produce more heat.
5. Understand that the equilibrium constant (K) for an exothermic reaction decreases with an increase in temperature, as the reaction shifts to the left, and increases with a decrease in temperature, as the reaction shifts to the right.