So there is a voltage cell that is based on copper ions and copper and brome and brome ions. So the first task is what is the standard EMF of the cell. For this you have the standard EMF of the cathode, it's the brome and the anal that's the copper and you just have to subtract the from the anal from the cathode and so there is 0.72 volts as the standard EMF of the cell. That's the first. The second one is which reaction occurs at the cathode and which one at the end of the cell. Just simple, at the end of the copper is oxidized and at the cathode the brome is reduced. The third task is a little bit more difficult. I add to use S values and appendix C and the relationship between cell potential and free energy to change to predict whether the cell potential increases or decreases when the temperature is raised above 25 degrees. So what happens when you increase the temperature of the reaction? With this you need Gibbs-Antelope and you have two electrons for N, for F, the third-day constant and E is the standard EMF 0.72. You put it together all the numbers together, the two for the two electrons, then the ferridae constant and the EMF and you get minus 138.9 kilojoule per mole. That's the Gibbs constant. The whole entropy, delta S, you need the entropy of the products minus the entropy of the adults. Then you put it all together, the unit is every time joule per Kelvin and mole and you get to minus 123.78 joule per Kelvin and mole. With this you can see the cell potential will decrease as temperature increases. This is because delta S is negative and so delta G will become more positive with rising temperature. With the big at delta G so comes smaller E.