Write the equation for the combustion of glucose with O2 to give CO2 and H2O.
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Write the equation for the combustion of glucose with O2 to give CO2 and H2O.
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- Plants convert carbon dioxide and water to glucose 1C6H12O62 and oxygen in the process of photosynthesis. Write a balanced equation for this reaction, and determine how many moles of CO2 are required to produce 15.0 mol of glucose.One step of the cycle that incorporates CO2 into glyceraldehyde in plants is the production of two 3-phosphoglycerates. ΔG = -3.5 kJ/mol for thisreaction. Is this process endergonic or exergonic?Write the chemical equation in which CO2 is converted to HCO3- and H+. What enzyme catalyzes this reaction, and where in the blood is it found?
- Complete the following reactions: NADH, H+ oxidoreductase O2 oxidoreductaseList the following substances in order of their increasing oxidizing power: (a) acetoacetate, (b) cytochrome b (Fe3+, (c) NAD+, (d) SO42− , and (e) pyruvate.Ozone in the lower atmosphere is a pollutant that can form by the following reaction involving the oxidation of unburned hydrocarbons:CH4(g) + 8 O2(g)-------->CO2(g) + 2 H2O(g) + 4 O3(g)Use the standard free energies of formation to determine ΔG°rxn for this reaction at 25 °C.
- Write an equation for the pyruvate dehydrogenase reaction.Refer to the figure shown here, and determine the value of E for the overall oxidation/reduction reaction (refer to the book/lecture slides if you need help with the overall reaction). 121/202 + 2H+ + 2e → H₂0 NAD + H* + 2e → NADH O-1.136 volts O 0.496 volts O+1.136 volts voltsm -0.496 volts EU (volts) +0.816 - 0.320The complete combustion of palmitate and glucose yields 9781 kJ ∙ mol−1 and 2850 kJ ∙ mol−1 of free energy, respectively. Compare these values to the free energy (as ATP) obtained though catabolism of palmitate and glucose under standard conditions. Which process is more efficient?
- Write a balanced equation showing the conversion of glucose and oxygen to carbon dioxide and water: (a) Indicate in your equation which molecule becomes reduced? (b) Indicate in your equation which molecule becomes oxidized? (c) What happens to the energy that is released in this redox reaction? (d) Name the oxidizing agent.explain in quantitative terms the circumstances under which the following reaction can porceed; L-malate + NAD+ (forward arrow) oxaloacetate + NADH + H+ delta G' standard = +29.7 KJ/molUsing the symbols X-H2 and Y, draw a coupled oxidation-reduction reaction. Designate the molecule that is reduced and the one that is oxidized and state which one is the reducing agent and which is the oxidizing agent.