Cytochrome, a complicated molecule that we will represent as CyFe2+, reacts with the air we breathe to supply energy required to synthesize adenosine triphosphate (ATP). The body uses ATP as an energy source to drive other reactions (Section 19.7). At pH 7.0 the following reduction potentials pertain to this oxidation of CyFe2+: O21g2 + 4 H+1aq2 + 4 e- ¡ 2 H2O1l2 Ered ° = +0.8 (b) If the synthesis of 1.00 mol of ATP from adenosine diphosphate (ADP) requires a ∆G of 37.7 kJ, how many moles of ATP are synthesized per mole of O2?

Video transcript

hey everyone in this example, we're told that the energy from a reaction of nitric acid shown below is used to create nitrogen dioxide. We need to figure out how many moles of nitrogen dioxide can be created. Permal of nitric acid. And we're told that the energy needed to create one mole of nitrogen dioxide is 1 22.92 kg joules. So we're given our reaction here below as well as its electrode potential being 0.98 volts. So for the first part of the solution, we're going to calculate our change in gibbs free energy and we should recall that. This is calculated by taking negative one times our electrons transferred in our reduction N. This is then multiplied by Faraday's constant. And then multiplied by our energy where the value for energy is going to be our electrode potential degree. So what we should have plugging in what we know is negative one times our moles of electrons transferred. And we can see that according to our given reaction, we just have one mole of electrons transferred because we have a coefficient of one here. So we have one. And sorry about that wrong pen, we have one mole of electrons that is transferred in our reaction. This is multiplied by Faraday's constant. Which we should recall is 96,485 kg jewels. Which is then multiplied by our electoral potential given in our prompt as 0.98V. And so to simplify this, we would get that our change in Gibbs free energy is equal to - 555.3 kayla jewels per mole of our nitric acid. So moving on to Part two of the solution, now that we have this information according to the prompt, we're going to use the info where they tell us that the energy needed to create one mole of nitrogen dioxide is 1 22.92 kg jewels. So we're going to take that value 1 22 0.92 kg jewels. And this is the energy per hour nitrogen dioxide molecule. We're going to multiply this by what we just calculated above for gibbs. Free energy where for one mole of our nitric acid, We have 94, 0.5553 kg jewels. So just to make a correction here, this should be the point or the decimal here should be between the four and the five. So we would have 94.5553 kg joules here. So canceling out our units, we can cancel out Kayla jewels were left with moles of nitric acid, per molecule of nitrogen dioxide. And this is going to give us our final results equal to 1. moles of nitrogen dioxide per mole of nitric acid. That can be created according to our reaction. So this would be our final answer here. To complete this example. I hope that everything I reviewed was clear. But if you have any questions, just leave them down below and I will see everyone in the next practice video.