At 298 K a cell reaction has a standard cell potential of +0.17 V. The equilibrium constant for the reaction is 5.5 × 10⁵. What is the value of n for the reaction?

Video transcript

Welcome back everyone. To another video. A cell reaction has a reading of 2.1 volts at 298. Kelvin. What is the value of N if the reaction has an equilibrium constant of 3.289 multiplied by 10 to the power of 35th. First of all, we have to recall that the relationship between the cell potential in the equilibrium constant is E not cell equals RT divided by NF multiplied by the natural log of the equilibrium constant. Specifically, we're looking for the number of moles of electrons transferred. So we're looking for the value of N and if we rearrange the equation, we get N equals the universal gap constant R multiplied by the absolute temperature T divided by the cell potential Y not sell multiplied by the far days constant F and also multiplied by the natural logarithm of the equilibrium constant keq. So essentially what we want to do is just substitute the data. And we know that the universal gas constant is 8.314 jules per mole per Kelvin. The given temperature is 298 Kelvin. Now we're given 2.1 volts for the E knot cell value. What about the Faraday constant? That would be 96485 cool arm mode. And now we're going to multiply by the natural logarithm of the equilibrium constant, which is 3.289 multiplied by 10 to the power of 35th. And when we evaluate the result, we get one mole of electrons specifically, if we use our units correctly, that'd be cool on per mole of electrons. So we can get one mole of electrons transferred in this reaction. And that's our final answer. Thank you for watching.