Consider this cell: Al(s) | Al3+(aq) || Br2(l) | Br-(aq)1/3Al(s) + 1/2Br2(l) -> 1/3Al3+(Aq) + Br-(aq) Delta H^{0} rxn = -299 kJ/molBr2(l) + 2e - -> 2Br-(aq) : 1.09 VAl3+(aq) + 3e - -> Al(s) : -1.66 V1. What is the standard potential for this cell at 25 degrees C? 2. What is the potential of the cell at room temperature if the concentration of bromide ion is 0.691 M and the concentration of aluminum ions is 31 μM? 3. What is the equilibrium constant for the reaction?4. Without doing any calculations, decide if the standard potential for the cell will increase or decrease if the temperature is increased. Write down your reasoning. What is the standard potential of this cell at 88 °C?