The oxidation of glucose (C6H12O6) in body tissue producesCO2 and H2O. In contrast, anaerobic decomposition,which occurs during fermentation, produces ethanol(C2H5OH) and CO2. (a) Compare the equilibrium constants for the following reactions: C6H12O6(s) + 6 O2(g)   ⇌ 6 CO2(g)  + 6 H2O(l) C6H12O6(s)  ⇌ 2 C2H5OH(l) + 2 CO2(g)  (b) Compare the maximum work that can be obtained fromthese processes under standard conditions.

The equilibrium constant for the following reaction is 20.9 at 907 °C. 2 SO2(g) + O2(g) 2 SO3(g) K= 20.9 at 907 °C Calculate the equilibrium constant for the following reactions at 907 °C. (a) 2 SO3(g) 2 SO2(g) + 02(g) K= (b) SO3(g) SO (g) + 1/2 O2(g) K=

An important step in the industrial production of hydro- gen is the reaction of carbon monoxide with water: CO(g) + H2O(g) = CO2(g) + H2(g) (a) Use the law of mass action to write the equilibrium expression for this reaction. (b) At 500°C, the equilibrium constant for this reaction is 3.9. Suppose that the equilibrium partial pressures of CO and H,O are both 0.10 atm and that of CO, is 0.70 atm. Calculate the equilibrium partial pressure of H2(g).

Do not give handwriting solution. Given the following equilibrium reaction and equilibrium constant at 300 K: 2 SO3 (g) ⇌ O2 (g) + 2 SO2 (g) Kp = 0.049 calculate the equilibrium constant (Kp) for the following reaction at the same temperature. Enter your answer with no units. 3 O2 (g) + 6 SO2 (g) ⇌ 6 SO3 (g) Kp = ?

The equilibrium constant expression for the reaction, 2CO (g) + 02 (g) = 2C02 (g) is given by Kp =

For the reaction below, the thermodynamic equilibrium constant is K= 1.92x103 at 35 °C. NHẠCO2NH2(s) → 2 NH3(g) + CO2(g) Suppose that 0.0046 moles of NHẠCO2NH2, 0.0092 moles of NH3, and 0.0046 moles of CO2 are added to a 3.00 L container at 35 °C. (a) What are Q and A,G for the initial reaction mixture? Your answers must be accurate to 3 significant figures. Q = Number A,G= Number kJ mol-1 (b) Is the spontaneous reaction to the left or to the right? Click for List

5) At 25 °C the equilibrium constant of the reaction is Kel for the respective reactions and N₂(g) +3H₂(g) 2NH₂(g) (reaction 1) 3.5 x 108. What are the values Ke2 and Ke3 of the equilibrium constants = N2(g) +H₂(g) = NH₂(g) H₂(g) NH3(g), (reaction 2) 2NH3(9) N₂(g) + 3 H₂(g) 1 3 (reaction 3)?

In an experiment, gaseous C2H4 and H2O, at 25 mmol each, were mixed in a 50-mL flask that contains 2.5 mmol of C2H6. (a) Determine the equilibrium constant if, at equilibrium, 16 mmol of C2H6 was present. C2H4(g) + H2O(g) ⇋ C2H6(g) + O2(g) At one point of the experiment, it was found that 9.7 mmol C2H4, 7.5 mmol H2O, 21.9 mmol C2H6 and 16.4 mmol O2 were present in the flask. (b) At what direction should the reaction proceed to achieve equilibrium? Support your answer with calculations and explain your answer in not more than 3 sentences.

The value of the equilibrium constant is Ke = 0.052 at 600 °C for the reaction: 2 S03 (g) = 2 S02 (g) + 02 (g). Now we mix 0.72-mol SO3, 0.31-mol SO2 (g) and 0.11-mol 02 (g) in a 1-L container. Which of the following statements is (or are) true? a) The reaction will proceed to left (shift to the reactant side) to reach equilibrium. b) The concentration of SO3 will increase during the reaction course. c) The concentration of SO2 will increase during the reaction course. %3! a) only bi only Og only Oa and b) O b) and c) O and a) O a), b) and c) Neither of the 3 statements is true.

The reaction HCO₂H(g) CO(g) + H₂O(g) has Kp = 1.6 × 106 at 400 °C. What is the value of Kc for this reaction at this temperature? Kc = H