Introduction: The lesson “Reduction-Oxidation Reaction” really challenged my comprehension and computation skills in many ways. The first one is the complexity of instructions that are needed to be followed in order to arrive at the corresponding answer for a particular reaction. I basically confused the oxidation and reduction half reaction wherein I don’t know what elements will be reduced and oxidized. One of the things that I’ve confused is that I’ve mistaken the monoatomic charges for the oxidation numbers, wherein I put the monoatomic charges of their corresponding element, causing all of my answers in one of my quiz to fail horribly. Although I was able to get the concept of the oxidation reaction, I am still confused by the reduction Oxidation is defined as the loss of electrons of an atom due to the transfer of electrons to another atom. Reduction is defined as the gain of electrons of an atom due to the transferred electrons which came from the oxidation of another atom. In other words, oxidation is the opposite of reduction. Redox is considered to be one of the ways in balancing an equation. Half-reaction is obtained by considering the change in oxidation number of substances in the equation. There are also some rules to be followed in balancing equations using redox: 1. The oxidation number of hydrogen is always +1, except for hydride (-1) 2. The oxidation number of oxygen is always -2, except for peroxide (-1) 3. Free elements have an oxidation number of 0. 4. The sum of the oxidation numbers in a compound is 0 5. Polyatomic ions have a sum of oxidation numbers equal to the valence of the ion itself. Steps in solving equations using Redox: 1. Assign the oxidation numbers for the corresponding elements 2. Find the elements that undergone a change in oxidation numbers at the other side of the equation. Take note of which element’s oxidation number was reduced and which one was
The question I was trying to answer is Which balanced chemical equation best represents the thermal decomposition of sodium bicarbonate. Using that question to guide us we were trying to determine which of the four chemical equations show how atoms are rearranged during thermal decomposition. We concluded it was the second chemical equation, we know that because:
Determine the reaction order for Na2S2O3 using calculations described in the Background. Show your work. Note that your answer will probably not be an even whole number as it is in the examples.
Enzymes are biomolecules that catalyze or assist chemical reactions. ("Enzyme Information - Disabled World", n.d.,) Without enzymes it would be impossible for an organism to carry out chemical reactions. Enzymes are proteins that carry a chemical reaction for a specific substance or nutrient. For example, the digestive enzymes help food to be broken down so it can be absorbed. Enzymes can either initiate the reaction or speed it up. Substrates are the chemicals that are transformed by enzymes. (Gunsch & Foster, 2014) Reactants are the chemicals in the absence of enzymes. Metabolic pathways that occur in a cell are determined by a set of enzymes which are selective for their substrates and catalyze only a few reactions among the many possibilities.
Ionic Equation: H+(aq) + NO3(aq) + Na+(aq) + OH-(aq) → Na+(aq) + NO3(aq) + H2O(l)
The equation shows how 1 mol of Na2CO3 reacts with 1 mol of H2SO4, so
Introduction: The purpose of this lab was to cycle solid copper through a series of chemical forms and return it to its original form. A specific quantity of copper undergoes many types of reactions and goes through its whole cycle, then returns to its solid copper to be weighted. We observed 5 chemical reactions involving copper which are: Redox reaction (which includes all chemical reactions in which atoms have their oxidation state changed), double displacement reaction, precipitation reaction, decomposition reaction, and single displacement reaction. 4HNO3(aq) + Cu(s) --> Cu (NO3)2(aq) + 2H2O (l) + 2NO2(g) Oxidation reduction reaction Cu (NO3)2(aq) + 2 NaOH (aq) --> Cu (OH)2(s) + 2 NaNO3(aq) Precipitation Reaction Cu (OH)2(s) + heat --> CuO (s) + H2O (l) Decomposition reaction CuO (s) + H2SO Data Results: (mass of copper recovered / initial mass of copper) x 100 Mass of copper recovered: 0.21 Initial mass of copper: 0.52 (0.21/0.52)x100 =40.38%.
Ionic compounds are normally a combination of a metal, along with one or more non-metals. If you recognize the two ions, you have the name of the compound. For example, the familiar calcium ion, Ca2+ must combine with two iodides, I–, to afford calcium iodide, CaI2. For ionic compounds this means that the formula unit must have an equal number of positive and negative charges because ionic
== == I completed a table to show my results, here is the table: Table 1. Results of different changes of substances Part A Copper (II) Sulfate and Water Reactant description Water (reactant): Color: Colorless Transparency:
Atoms are electrically neutral; the electrons that bear the negative charge are equal in number to the protons in the nucleus
x2 (x + 12) +(−9) (x −12)=0 Factor out the common term in each group. x2 and (−9)
Oxygen is an essential component for cellular metabolic processes. As a result of normal cellular metabolism, oxidative products i.e. oxygen free radicals or reactive oxygen species are produced. In eukaryotic cells energy is generated in mitochondria as a result of aerobic respiration and this oxidative metabolism is responsible for formation of various compounds. Nearly all of these compounds are advantageous but a small proportion could be lethal if produced in higher concentration. During normal conditions small quantities of oxidative products are necessary for certain sub cellular events, including enzyme activation, formation of disulfide bond during the folding of new proteins, signal transduction and gene expression etc. (Yu etal., 2002; Droge, 2002). Oxidative stress can be defined as the excessive production of ROS which are not adequately removed from the body, because of reduced antioxidant defense system or the ROS increases beyond the capacity of antioxidants. The balance between oxidants and antioxidants is vital because oxidative stress can cause oxidative damages to N.A, lipids and proteins. The most important ROS are superoxide anion (O2−), singlet oxygen (O2), hydrogen peroxide (H2O2) and highly reactive hydroxyl radical (OH-). Whereas, antioxidant defense system is responsible to give protection against ROS. These antioxidants can scavenge and destroy ROS. The major antioxidant enzymes are catalase (CAT), superoxide dismutase (SOD) PON ….. and glutathione system (Sies, 1985; Valko et al., 2007; Halliwell and Gutteridge, 1990).
Copper Oxide + Carbon Dioxide (CuCO3 = CuO + CO2) The reactivity series determines how fast this reaction occurs. The reactivity series is the order of metals in the periodic table. The most reactive metals are placed at the top of the reactivity series.
Reactions occur when the particles of reactants collide together continuously. If they collide with sufficient energy, then they will react. The minimum amount of kinetic energy required for particles at the time of collision is called the activation energy and this theory is known as the ?collision theory?.
... the reaction to shift to the right would be to remove products. A third way is to change the temperature. Since this is an endothermic reaction, +∆H, we can imagine that “heat” is a reactant. Thus, if we add heat, it will shift to the right. To be classified as a redox reaction, we need at least two elements to change oxidation states. The easiest way to look at a reaction and determine this is if you have an element by itself on one side of the reaction and it is in a compound on the other side. Most of the time, the oxidation number of each element in a compound is their common charge. The sum of oxidation numbers must equal the compounds overall charge. Elements in the natural state (by themselves) have an oxidation number of 0. The reducing agent is the species responsible for reducing the other chemical. Therefore, the reducing agent is oxidized itself.
Smith, Roland. Conquering Chemsitry: HSC course. 4th ed. Vol. 1. N/A: Cengage Learning Australia, 2010. 74-90. 1 vols. Print.