Electrochemistry

Proposed Mechanisms for the Direct Oxidation of Methane to Methanol The oxidation of CH4 usually progresses to C02 and H20 because the intermediates are a series of highly reactive radical reactions and this makes partial oxidation of CH3 into CH3OH very hard. In addition, CH3OH oxidizes faster than CH4 and requires less energy for its oxidation. Industrial attempts to synthesize methanol from methane is usually done indirectly since the direct methods have low methanol specificity and yield. Current

Unit P4 Electro-Chemical Cells. Redox reaction. The procedure for producing EMF in an electrochemical cell is due to an internal chemical reaction which is the redox reaction this is a reaction that involves electrons being transferred from the reducing agent to the oxidizing agent. The reaction is between the electrolyte and negative electrode which will create a buildup of free electrons, each of which has a negative charge at the anode of the battery which is the negative terminal. The chemical

a. O3: The O has an oxidation number of 0, because the oxidation number of an element is always 0 regardless of its subscript. b. H3PO4: (+1)3+P+(-2)4=0 P-5=0 P=+5 For the compound to have an overall charge of 0, phosphorus must have an oxidation number of +5 c. MnO3- : Mn+(-2)3=-1 Mn-6=-1 Mn=-1+6 Mn=+5 For the compound to have an overall charge of 0, manganese must have an oxidation number of +5. d. C2O42- C(2)+(-2)4=-2 C(2)-8=-2 C(2)=+6 C=+3 For the compound to have

Properties of Solutions: Electrolytes and Non-Electrolytes The objective of this lab the type of compounds formed in many different solutions dissolved in water based on the conductivity of each. Procedure: Refer to handout entitled “Properties of Solutions: Electrolytes and Non-Electrolytes” Materials: Refer to handout entitled “Properties of Solutions: Electrolytes and Non-Electrolytes” Data & Observations: Solution Conductivity (μS/cm) A – CaCl2 9100 μS/cm A – AlCl3 11920 μS/cm A – NaCl

Chem Speech – Daniel George From the roots of the HSC Chemistry course, we are conditioned to the concept of a Galvanic Cell. It is essentially a circuit containing a Positive Cathode where reduction reactions occur and a Negative Anode, where oxidation reactions occur. Galvanic Cells operate with the basic principles of converting chemical energy into electrical energy via spontaneous reactions at the Anode and Cathode. However, today we are looking Electrolytic cells. These operate with the function

A H2/O2 proton−exchange membrane fuel cell (PEMFC) is a clean, sustainable energy source and suitable for the operation of small electronic device [1]. Among many problems that still exist for PEMFC, the sluggish reactions at the cathode electrode and poor mass transport of protons and electron decrease the fuel cell performance by increasing the activation overvoltage, or activation loss [2]. This problem can, however, be solved by raising the fuel-cell operating temperature [3], but only up to

It is typical when analyzing technology for the presence of chemistry to be hardly noticed or failed to be seen at all. This is a false assessment, and is caused by simply not looking close enough. Chemistry’s presence is not always blatantly obvious, even though it is truly at the root of most all technology we use on a daily basis. One of the fields of technology that we do in fact use on a daily basis that chemistry impacts, and therefore impacts whole other genres of technology, is the battery

Lithium-ion batteries are made from lithium; hence the name. Since lithium is an unstable metal, lithium ions must be made through chemicals. Lithium is used because it is the lightest metal with the highest electrochemical potential. Inside these batteries are a positive electrode called the cathode, an anode or the negative electrode and lithium ions. Theses lithium ions move from the negative electrode to the positive when it’s being used and vice versa when it’s being charged. For the electrodes

Redox reaction: Redox reactions involve transfer of electrons from one reactant to another Anode: The anode is the electrode which oxidation occurs Cathode: The cathode is the electrode at which reduction occurs Oxidation: Oxidation is loss of electrons Reduction: Reduction is gain of electrons Oxidation state: The oxidation state of an element is the charge on the ion Salt bridge: The salt bridge allows the migration of ions to occur Electrolyte: An electrolyte is a substance which in solution

The EPA estimates Americans purchase nearly 3 billion batteries each year (D., 2009). A battery is also known as a voltaic cell, and the energy generated and stored by a battery is actually a result of chemical reactions and not mechanical motion. Batteries are contained in nearly every common electronic device, ranging from small devices like smartphones to larger scale products like automobiles, and chemistry is the driving force behind the function of these batteries.Batteries consist of galvanic