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- Another step in the metabolism of glucose, which occurs after the formation of glucose6-phosphate, is the conversion of fructose6-phosphate to fructose1,6-bisphosphate(bis meanstwo): Fructose6-phosphate(aq) + H2PO4(aq) fructose l,6-bisphosphate(aq) + H2O() + H+(aq) (a) This reaction has a Gibbs free energy change of +16.7 kJ/mol of fructose6-phosphate. Is it endergonic or exergonic? (b) Write the equation for the formation of 1 mol ADP fromATR for which rG = 30.5 kJ/mol. (c) Couple these two reactions to get an exergonic process;write its overall chemical equation, and calculate theGibbs free energy change.Plants synthesize carbohydrates from CO2 and H2O by the process of photosynthesis. For example, 6CO2(g)+6H2O(l)C6H12O6(aq)+6O2(g) G=2.87103 kJ at pH 7.0 and 25°C. What is K for the reaction at 25°C?3. Compute the equilibrium constant (Keq) for the synthesis of glucose-1-phosphate at 37\deg C, based on the reaction: Glucose + HPO4^2- Glucose-1-phosphate + H2O,
- For the triose phosphate catalyzed reaction: dihydroxyacetone phosphate <--> glyceraldehyde-3-phosphate the standard change in Gibbs free energy is ΔG'º=7.53 kJ/mol. Calculate the ΔG for this reaction at 298K when the concentration of dihydroxyacetone phosphate is 0.161 M and the concentration of glyceraldehyde-3-phosphate is 0.00163 M.Consider The Following Reaction: CaCO3(S) + 2HCl(Aq) = CaCl2(Aq) + H2O(L) + CO2(G) Write down the quation of the equilibrium constant kc for this reactionCalculate the equilibrium constant for the phosphorylation of glucose to glucose 6-phosphate at 37.0 °C. 4.74 x10¬3 M-1 eq In the rat hepatocyte, the physiological concentrations of glucose and P; are maintained at approximately 4.8 mM. What is the equilibrium concentration of glucose 6-phosphate (G6P) obtained by the direct phosphorylation of glucose by P;? 8.75 x10-8 [G6P] = M Incorrect
- The conversion of glucose (C&H1206) into lactic acid (2CH3CH(OH)COOH) drives the phosphorylation of 2 moles of ADP to ATP and has a AG -135 kJ/mol. CH1,06laq) +2HPO (aq) + 2ADP (aq) + 2H* (aq) → 2CH,CH(OH)COOH (aq) + 2ATP (aq) + 2H,0(1) The conversion of ATP to ADP has a AG° = -30.5 kJ/mol. ATP (aq) +H,0(1) ADP (aq) +HPO (aq) +H*(aq) 1st attempt See Periodic Table See Hint What is AG° for the conversion of glucose into lactic acid? CH1206(aq) 2CH,CH(OH)COOH(aq)In biological cells, the energy released by the oxidation of foods is stored in adenosine triphosphate (ATP or ATP4). The essence of ATP's action is its ability to lose its terminal phosphate group by hydrolysis and to form adenosine diphosphate (ADP or ADP³-) ATP+ (aq) + H₂0 (1)→ ADP³- (aq) + HPO¯(aq) + H₂O+ (aq) At physiological conditions, pH = 7 and T = 310K (blood temperature), the enthalpy and Gibbs energy of hydrolysis are A, H = -20 and AG = -31, respectively. The hydrolysis of 1.00 mol of ATP, at these conditions, results in the extraction of 31 kJ of energy that can be used to do non-expansion work such as the synthesis of proteins or activation of neurons. mol Calculate the entropy of hydrolysis at pH = 7 and T = 310K5. One of the key steps in the tricarboxylic acid (TCA) cycle is the hydration of fumarate to malate: Fumarate-² + H₂O = Malate-2 The standard reaction Gibbs free energy and enthalpy for this reactions are -880 cal/mol and 3560 cal/mol, respectively. (a) What is the equilibrium constant for this reaction (25 °C)? (b) Is the reaction favorable (spontaneous) at 25 °C? (c) What is the equilibrium constant of this reaction under physiological conditions (37 °C)? (d) Is this reaction favorable at 37 °C?
- Calculate the equilibrium constant of the reaction in which glutamine is formed -O2CCH (NH3 +) CH2CH2CONH2 (hereinafter G) from glutamic acid -O2CCH (NH3 +) CH2CH2COOH (G ') in cells, under the action of the synthetase enzyme glutamine. This reaction is used to carry ammonia from the cells to the kidneys, where it is re-released and excreted. Use the value of the standard free reaction enthalpy G '(aq) + NH3 (aq) → G (aq) equal to +15.7 kJ / mol at 37 ° C. The reaction is driven by the feed-back of the ATP (aq) → reaction ADP (aq) + Pi (aq). the standard free enthalpy of which is -31 kJ / mol. What is constant equilibrium joint reaction: G '(aq) + NH3 (aq) + ATP (aq) → G (aq) + ADP (aq) + Pi (aq)?For the aqueous reaction CH2OH H C-OH of ČH2-O P-O ČH2- dihydroxyacetone phosphate glyceraldehyde-3-phosphate the standard change in Gibbs free energy is AG" 7.53 kJ/mol. Calculate AG for this reaction at 298 K when [dihydroxyacetone phosphate] = 0.100 M and [glyceraldehyde-3-phosphate] = 0.00300 M. AG = %3D kJ/molCalcium ions bind to a Ca2+-ATPase which has two identical calcium sites, in two stages with apparent equilibrium constants of K, = 3.5 x 105 and K2 = 2 x 106. Determinet for this binding.