If the concentration of C6H12O6 (glucose) is increased, the equilibrium will shift to the left. This is based on Le Chatelier’s Principle, which states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium moves to counteract the change.
The given chemical equation is:
6H2O (l) + 6CO2 (g) ⇌ C6H12O6 (s) + 6O2 (g) ΔH = 2801.69 kJ/mol
When the concentration of C6H12O6 is increased, the system will try to reduce this concentration by shifting the equilibrium to the left. This means that more C6H12O6 will react to form 6H2O and 6CO2, thereby reducing the concentration of C6H12O6 and restoring equilibrium.
In summary, increasing the concentration of C6H12O6 will cause the equilibrium to shift to the left, favoring the formation of reactants (6H2O and 6CO2).