C. No change D. Cannot be determined Which statement is TRUE about the reaction? C6H12O6 + O2(g) H2O OH = -2805 kJ/mol A. The reaction is exothermic. B. The Hproducts is less than Hreactants. C. One mole of glucose produces one mole of water. D. None of these --> CO2(g)

Consider the following reaction where K. = 1.29×102 at 600 K. COCI2(g) CO(g) + Cl2(g) A reaction mixture was found to contain 0.109 moles of COC1,(g), 2.19x10 2 moles of CO(g), and 3.88x102 moles of Cl,(g), in a 1.00 liter container. Is the reaction at equilibrium? If not, what direction must it run in order to reach equilibrium? The reaction quotient, Qe, equals The reaction A. must run in the forward direction to reach equilibrium. B. must run in the reverse direction to reach equilibrium. C. is at equilibrium.

Consider the following reaction: 4PC13(g) P4(g) + 6C12(g) If the initial concentration of PC13(g) is 1.5 mol/L, and "x" is the equilibrium concentration of Pa(g), what is the correct equilibrium relation а. Кс-бх7 O b. Kc=6x7/(1.0-4x)4 O c. Kc=(x)(6x)6/(1.0-4x)4 O d. Kc=(x)(6x)°/(1.5-4x)4 O e. Kc=x'/(1.0-x)4

This is the problem from the textbook (at the end of bioenergenic chapter) but has no explanation.. can you please explain this problem?