Core 1 summary notes 1) Fossils fuels provide both energy & raw materials such as ethylene‚ for production of other substances Identify the industrial source of ethylene from the cracking of some of the fractions from the refining of petroleum Catalytic cracking is the process whereby high molecular weight fractions are broken down to low molecular weight ones. This process is used in petroleum refineries where crude oil is broken down to smaller alkenes and alkanes‚ until ethene‚ propene‚
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кислород и еден атом од друг хемиски елемент во својата формула. An oxide /ˈɒksaɪd/ is a chemical compound that contains at least one oxygenatom and one other element[1] in its chemical formula. Metal oxides typically contain an anion of oxygen in the oxidation state of −2. Most of the Earth’s crustconsists of solid oxides‚ the result of elements being oxidized by the oxygen in air or in water. Hydrocarbon combustion affords the two principal carbon oxides:carbon monoxide and carbon dioxide. Even materials
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Chemistry Final Study Guide Matter as anything that has mass and takes up space. Significant figures refers to digits that were measured. When rounding calculated numbers‚ we pay attention to significant figures so we do not overstate the accuracy of our answers. Rules: -All nonzero digits are significant. -Zeroes between two significant figures are themselves significant. -Zeroes at the beginning of a number are never significant. -Zeroes at the end of a number are significant if a decimal
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http://www.kewpid.com 1. Fossil fuels provide both energy and raw materials such as ethylene‚ for the production of other substances 1) Construct word and balanced chemical equations of chemical reactions as they are encountered • Methane + oxygen carbon dioxide + water • CH4(g) + 2O2(g) CO2(g) + 2H2O(l) 2) Identify the industrial source of ethylene from the cracking of some of the fractions from refining of petroleum Generally‚ demand for petrol exceeds supply produced from fractional distillation
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Assign Oxidation Numbers to the following: a. HNO3 b. PbSO4 c. (NH4)2Ce(SO4)3 Balance the following in acidic medium Al (s) + MnO4- (aq) Al3+ (aq) + Mn2+ (aq) Balance the following in a basic medium Mg (s) + OCl- (aq) Mg(OH)2 (s) + Cl- (aq) Balance the following Redox Reaction: The big nasty problem K4Fe(CN)6 + KMnO4 + H2SO4 KHSO4 + Fe2(SO4)3 + MnSO4 + HNO3 + CO2 +H2O 17.1: Galvanic Cells Review of Redox Reactions Oxidation: _______________________ Reduction: ___________________________
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reaction or process that releases energy in the form of heat. Sometimes the term is applied to processes that release other forms of energy‚ such as electrical energy‚ sound‚ or light. An Example –The example would be combustion of wood. Oxidation - Oxidation is the loss of electrons during a reaction by a molecule‚ atom or ion. An Example - The example is iron combines with oxygen to form iron oxide or rust. The iron is said to have oxidized into rust. Heating natural gas - Natural gas is a
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Biology Key Questions – Lesson #1 1. How many electrons does Mg2+ have? Answer: Mg2+ has 10 electrons. A Magnesium atom has 12 electrons‚ 2 of which are valence electrons. The atom will lose the 2 outermost electrons in order to stabilize its electron shell. The nucleus maintains its 12 protons and becomes a Mg2+ ion. 2. Given that the half-life of the radioisotope carbon-14 is 5730 years‚ how useful do you think this isotope would be for dating bones that are over a million years
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respiration consumes organic molecules and oxygen and yields ATP. 2. Diagram for photosynthesis and respiration 3. What are redox reactions? What is the difference between reduction and oxidation reactions? Redox reactions are chemical reactions that transfer between reactants. In oxidation‚ a substance loses electrons. In reduction‚ a substance gains electrons. The electron donor is the reducing agent. The electron receptor is the oxidizing agent. 4. What electron carrier temporarily holds
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Chemical Reactions Lab Objectives: 1. To examine a variety of reactions including precipitation‚ acid-base‚ gas forming‚ and oxidation-reduction reactions. 2. To identify the products formed in these reactions and summarize the chemical changes in terms of balanced chemical equations and net ionic equations. 3. To identify the species being oxidized and reduced in oxidation-reduction reactions and determine which species is the oxidizing agent and the reducing agent. Chemical equations represent what occurs
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anode was either Zn‚ Sn‚ Fe‚ Mg or Pb. The electrode with the most positive reduction potential in its half reaction had acted as the best oxidizing agent‚ or was the most likely to be reduced. For this experiment‚ copper was the best oxidizing agent‚ with a reduction potential of +.337 V. Copper was reduced in every reaction‚ also proving that it was the strongest oxidizing agent. The electrode with the most positive oxidation potential in its half reaction had reacted as the best reducing agent‚ or
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