Use the standard half-cell potentials listed below to calculate the standard cell potential for the following reaction occurring in an electrochemical cell at 25°c. (the equation is balanced.) 3 cl2(g) + 2 fe(s) → 6 cl⁻(aq) + 2 fe3+(aq) cl2(g) + 2 e⁻ → 2 cl⁻(aq) e° = +1.36 v fe3+(aq) + 3 e⁻ → fe(s) e° = -0.04 v

According to the diagram; a) identify the anode of the cell and write the half-reaction that occurs there b) write the overall equation for the reaction that occurs as the cell operates c) calculate the value of the standard cell potential ,e cell. d)write the shorthand notation of the cell above e)indicate the flow of the electrons on the diagram

Place the elements below in order of decreasing ionization energy. aluminum(al) chlorine(cl) magnesium (mg) sulfur(s)

Chemistry worksheet - i am not sure what they are asking for exactly?