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Cells use the hydrolysis of adenosine triphosphate, abbreviated as ATP, as a source of energy. Symbolically, this reaction can be represented as
ATP(aq) + H2O(l) ? ADP(aq) + H2PO4-(aq)
where ADP represents adenosine diphosphate. For this reaction
G° = ?30.5 kJ/mol.
(a) Calculate K at 25°C.
(b) If all the free energy from the metabolism of glucose
C6H12O6(s) + 6 O2(g) ? 6 CO2(g) + 6 H2O(l)
goes into the production of ATP, how many ATP molecules can be produced for every molecule of glucose? molecules
Calculate the enthalpy change associated with the conversion of 25.0 grams of ice at -4.00°C to water vapor at 110.0°C. The specific heats of ice, water, and steam are 2.09 J/g-K, 4.18 J/g-K, and 1.84 J/g-K
Consider the situation in which 1.60 mL of an aqueous CuSO4 solution of unknown concentration is diluted to a volume of 10.00mL.
Explain why water boils at a lower temperature (
Consider two solutions. One solution is 0.1115 M Ca(OH)(2). The other is 0.1050 M HClO(4). a) Write a balanced equation for the reaction between the two solutions.
Calculate the number of moles in each of the following quantities.a) atoms of each element in 3.35 moles of aspirin(C9H8O4)
What is the normality of sulfuric acid solution which contains 6.64 g of H2SO4 in 837 mL of solution provided that the reaction involved
Draw the Lewis structure for the PO4-3 ion, indicating any resonance forms. On the basis of electron configurations, predict the formula of the Type I ionic compound formed from the elements Z=49 and Z=51.
If a gas held at constant pressure had an initial volume of 5.00 L and the temperature changed from 35°C to 578 K what would be the final volume of this gas?
calculate the heat released when 176g of water at 23.0 degrees celsius are converted to ice at -10.0 degrees celsius?
how many kilojoules and kilocalories of heat are required to raise 40.0 g of water from -12 degrees Celsius to 130 degrees Celsius?
In a titration of HNO3, you add a few drops of phenolphthalein indicator to 50.00 mL of acid in a flask. You quickly add 26.50 mL of 0.0502 M NaOH but overshoot the end point, and the solution turns deep pink.
which produce no significant response to interfering ions. It is then used to measure the pH of 0.0100 M NaOH in 0.50 M NaCl at 25 degrees C. What is the observed pH under these conditions if the true pH is 1.13?
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