Use the following information corresponding to 1 Molar concentrations of reactants and products for Questions 7-12. Glycerol + ATP → ADP+ 3-Phosphoglycerate: AH = -63.39 kJ/mol and AS = -0.1255 kJ/molk. At what temperature is this reaction at equilibrium? Report your answer in Kelvin. Type your answer...

For the ammonia synthesis reaction ⇌ Does the entropy effect favor products? Explain your answer. Does the energy effect favor products? Explain your answer. Is the equilibrium concentration of NH3(g) greater at high or low temperature? Explain.

Use the same fat described in Question 27. (a) Write a thermochemical equation for the metabolism of fat. (b) A dieter reduces his food intake by 425 nutritional calories a day (1 nutritional calorie=1000calories). How many kJ can he lose in one day? (c) How many pounds of fat are lost in one week with this diet?

The AGo' of a reaction is -250 kcal/mol. Which of the following can be deduced about this reaction? At equilibrium, [products] > [reactants]. Keq < 1 The reaction will proceed spontaneously under cellular conditions. None of the above can be deduced

Calculate the equilibrium constant for the following reaction at 37 oC. Fumarate +  H2O  → Malate          ΔGo’ = -3.13 kJ/mol

Fill in the missing intermediates and products in each of the following reactions.

Many metabolites are maintained at steady-state concentrations that are far from equilibrium. A comparison of K, and Q, the mass-action ratio, can determine whether a metabolic reaction is far from equilibrium. The equation for this equilibrium is, fructose 6-phosphate + ATP = fructose 1,6-bisphosphate + ADP Calculate K, for this reaction at T = 25.0 °C. AG' = -14.2 kJ/mol Calculate the mass-action ratio, Q, from the approximate physiological concentrations for rat heart tissue shown in the table. Metabolite Concentration (µM) Q = fructose 6-phosphate fructose 1,6-bisphosphate 84.0 29.0 ATP 11,800 ADP 1,310 Select the true statements about the PFK-1 reaction. In heart tissue, the PFK-1 products are more abundant than reactants. The PFK-1 reaction in heart tissue does not reach equilibrium. In heart tissue, the PFK-1 reaction will be driven toward product formation. Under standard conditions, the PFK-1 reaction reaches equilibrium when the concentrations of all products and reactants…

Consider the following system at equilibrium where ΔΗ° - 111 kJ, and == Kc = 0.159, at 7.23 × 10² K: N₂(g) + 3H₂ (g) — 2NH3 (g) If the temperature on the equilibrium system is suddenly decreased: The value of Kc Oincreases Odecreases Oremains the same The value of Qc is less than Ke Ois greater than Kc Ois equal to Ke The reaction must Orun in the forward direction to reestablish equilibrium Orun in the reverse direction to reestablish equilibrium Oremain in the current position, since it is already at equilibrium The concentration of H₂ will Oincrease Odecrease Oremain the same

Please answer this with work shown! Thanks!

Consider the following equilibrium: N₂(g) + 3H₂(g) → 2NH3 (g) Now suppose a reaction vessel is filled with 7.18 atm of nitrogen (N₂) and 0.0762 atm of ammonia (NH3) at 359. °C. Answer the following questions about this system: AGO= = -34. kJ Under these conditions, will the pressure of NH3 tend to rise or fall? H₂? Is it possible to reverse this tendency by adding In other words, if you said the pressure of NH3 will tend to rise, can that be changed to a tendency to fall by adding H₂? Similarly, if you said the pressure of NH3 will tend to fall, can that be changed to a tendency to rise by adding H₂? If you said the tendency can be reversed in the second question, calculate the minimum pressure of H₂ needed to reverse it. Round your answer to 2 significant digits. rise fall 0 yes O no atm x10 X