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The Equilibrium Constant of the Coupled Reaction will be :
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How would the equilibrium constant change if the reaction X with AGⓇ = +12.2 kJ moll...
please help! thanks TABLE 12-4 Standard Free Energy Change for Phosphate Hydrolysis Compound AGⓇ' (kJ. mol-')...
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TABLE 12-4 Standard Free Energy Change for Phosphate Hydrolysis Compound AGⓇ' (kJ. mol-') Phosphoenolpyruvate -61.9 1,3-Bisphosphoglycerate -49.4 ATP → AMP + PP, -45.6 Phosphocreatine -43.1 ATP ADP + P -30.5 Glucose-1-phosphate -20.9 PP, 2P, -19.2 Glucose-6-phosphate -13.8 Glycerol-3-phosphate -9.2 thioester bond AGⓇ' = -31.5 kJ•mol-1 H20 O CH3 -C-s-CoA I CH3 -C-0- + COA-SH Acetyl-CoA The formation of acetyl CoA from acetate is an ATP driven reaction: Acetate + ATP + COA <--> acetyl COA + AMP...
5.The following reaction has a ΔG°'--61.9 kJ/mol at 25°C, Phosphoenolpyruvate (PEP) +H2O Pyruvate + Inorganic Phosphate...
5.The following reaction has a ΔG°'--61.9 kJ/mol at 25°C, Phosphoenolpyruvate (PEP) +H2O Pyruvate + Inorganic Phosphate (Pi) (a) Is the reaction favorable under standard biochemical conditions? Explain your answer. (b) What is the equilibrium constant (K) of this reaction at 25°C? In cells the direct hydrolysis of PEP rarely occurs. Rather, the hydrolysis of PEP and the reverse hydrolysis of ATP are coupled (c) w rite out the coupled reaction and determine its ΔG at 25°C The hydrolysis of ATP...
State the answer and show your work. State units in the answer. 10 points total [F...
State the answer and show your work. State units in the answer. 10 points total [F = 96.485 kJ/V-mole; R = 8.314 J/mole-K] 1. The standard state free energy change (AG°') of hydrolysis for phosphoenolpyruvate (PEP) is -62.2 kJ/mole. The standard state free energy change of hydrolysis for ATP is -30.5 kJ/mole. What is the standard state free energy change for the following coupled reaction? PEP + ADP ---------> Pyruvate + ATP 2. In glycolysis, the standard state free energy...
Consider these hypothetical chemical reactions: A⇌B,ΔG= 13.7 kJ/mol B⇌C,ΔG= -27.2 kJ/mol C⇌D,ΔG= 6.20 kJ/mol What is...
Consider these hypothetical chemical reactions: A⇌B,ΔG= 13.7 kJ/mol B⇌C,ΔG= -27.2 kJ/mol C⇌D,ΔG= 6.20 kJ/mol What is the free energy, ΔG, for the overall reaction, A⇌D? Express your answer with the appropriate units. ΔG = Firefly luciferase is the enzyme that allows fireflies to illuminate their abdomens. Because this light generation is an ATP-requiring reaction, firefly luciferase can be used to test for the presence of ATP. In this way, luciferase can test for the presence of life. The coupled reactions...
er at initial change (AG The standard free energy change (AG) for ATP hydrolysis is -30.5 kJ/ mol ATP, ADP, and I a...
er at initial change (AG The standard free energy change (AG) for ATP hydrolysis is -30.5 kJ/ mol ATP, ADP, and I are mixed together at initial concentrations of 1 M each then left alone until the reaction below has come to equilibrium. For each species (ie. ATP. ADP and P.) indicate whether the concentration will be equal to 1 M, less than 1 M, or greater than 1 M after the reaction had reached equilibrium. Explain why. ATP +...
Consider a general reaction enzyme A(aq) = B(aq) The AGⓇ of the reaction is -8.070 kJ....
Consider a general reaction enzyme A(aq) = B(aq) The AGⓇ of the reaction is -8.070 kJ. mol-. Calculate the equilibrium constant for the reaction at 25 °C. Kéq= What is AG for the reaction at body temperature (37.0 °C) if the concentration of A is 1.7 M and the concentration of B is 0.70 M? AG = kJ. mol-1
Determine AGⓇ for a reaction at 298 Kelvin, If the equilibrium constant is 7.38 x 102?...
Determine AGⓇ for a reaction at 298 Kelvin, If the equilibrium constant is 7.38 x 102? a.-11.4 Kj b. 16.4 kJ C. - 9.11 ) d.-16.4 Kj e. - 9.64K)
The change in enthalpy (ΔHorxn) for a reaction is -36.6 kJ/mol . The equilibrium constant for...
The change in enthalpy (ΔHorxn) for a reaction is -36.6 kJ/mol . The equilibrium constant for the reaction is 2.0×103 at 298 K. What is the equilibrium constant for the reaction at 621 K ?
The change in enthalpy (ΔHorxn) for a reaction is -27.3 kJ/mol . The equilibrium constant for...
The change in enthalpy (ΔHorxn) for a reaction is -27.3 kJ/mol . The equilibrium constant for the reaction is 1.1×103 at 298 K. What is the equilibrium constant for the reaction at 666 K ?
The change in enthalpy (ΔHorxn) for a reaction is -23.1 kJ/mol . The equilibrium constant for...
The change in enthalpy (ΔHorxn) for a reaction is -23.1 kJ/mol . The equilibrium constant for the reaction is 2.9×103 at 298 K. Part A What is the equilibrium constant for the reaction at 632 K ?
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TABLE 12-4 Standard Free Energy Change for Phosphate Hydrolysis Compound AGⓇ' (kJ. mol-') Phosphoenolpyruvate -61.9 1,3-Bisphosphoglycerate -49.4 ATP → AMP + PP, -45.6 Phosphocreatine -43.1 ATP ADP + P -30.5 Glucose-1-phosphate -20.9 PP, 2P, -19.2 Glucose-6-phosphate -13.8 Glycerol-3-phosphate -9.2 thioester bond AGⓇ' = -31.5 kJ•mol-1 H20 O CH3 -C-s-CoA I CH3 -C-0- + COA-SH Acetyl-CoA The formation of acetyl CoA from acetate is an ATP driven reaction: Acetate + ATP + COA <--> acetyl COA + AMP...
5.The following reaction has a ΔG°'--61.9 kJ/mol at 25°C, Phosphoenolpyruvate (PEP) +H2O Pyruvate + Inorganic Phosphate (Pi) (a) Is the reaction favorable under standard biochemical conditions? Explain your answer. (b) What is the equilibrium constant (K) of this reaction at 25°C? In cells the direct hydrolysis of PEP rarely occurs. Rather, the hydrolysis of PEP and the reverse hydrolysis of ATP are coupled (c) w rite out the coupled reaction and determine its ΔG at 25°C The hydrolysis of ATP...
State the answer and show your work. State units in the answer. 10 points total [F = 96.485 kJ/V-mole; R = 8.314 J/mole-K] 1. The standard state free energy change (AG°') of hydrolysis for phosphoenolpyruvate (PEP) is -62.2 kJ/mole. The standard state free energy change of hydrolysis for ATP is -30.5 kJ/mole. What is the standard state free energy change for the following coupled reaction? PEP + ADP ---------> Pyruvate + ATP 2. In glycolysis, the standard state free energy...
er at initial change (AG The standard free energy change (AG) for ATP hydrolysis is -30.5 kJ/ mol ATP, ADP, and I are mixed together at initial concentrations of 1 M each then left alone until the reaction below has come to equilibrium. For each species (ie. ATP. ADP and P.) indicate whether the concentration will be equal to 1 M, less than 1 M, or greater than 1 M after the reaction had reached equilibrium. Explain why. ATP +...
Consider a general reaction enzyme A(aq) = B(aq) The AGⓇ of the reaction is -8.070 kJ. mol-. Calculate the equilibrium constant for the reaction at 25 °C. Kéq= What is AG for the reaction at body temperature (37.0 °C) if the concentration of A is 1.7 M and the concentration of B is 0.70 M? AG = kJ. mol-1
Determine AGⓇ for a reaction at 298 Kelvin, If the equilibrium constant is 7.38 x 102? a.-11.4 Kj b. 16.4 kJ C. - 9.11 ) d.-16.4 Kj e. - 9.64K)
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