decreases. This causes the equilibrium system to shift to the left (reactant) side. This is why the solution becomes lighter yellow. Fe(OH)3 is also formed during the experiment. 3) If the hydrated cobalt (II) ion complex was refrigerated‚ the temperature would decrease. Since this is an endothermic reaction a decrease in temperature will actually cause the equilibrium system to move to the left‚ favouring the reactants. When the reactants are favoured‚ the color of the solution will get lighter and change
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burned and was glowing a bright white color when ignited. Reactants: Mg and O2 Products: MgO Balanced chemical equation 2Mg + O2 2MgO Table 8.2- Combustion of heptane Observations When holding test tube inverted over heptane flame‚ condensation formed against top walls of the test tube. When the burning splint was added the walls of the test tube became less foggy from the condensation formed from the heptane flame. Reactants: C7H16 and O2 Products: CO2 and H2O Balanced chemical
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SALTS AND THEIR PREPARATION SALTS A salt is a compound formed when the hydrogen ions in an acid are replaced by metal ions or by ammonium ions. Compounds in which the H+ ions in an acid have been replaced by ammonium ions (NH4+) are called ammonium salts. NOTE: •An anion is a negatively charged ion. Hence:•Hydrochloric acid gives chlorides. E.g. sodium chloride‚ ammonium chloride. •Nitric acid gives nitrates. E.g. barium nitrate‚ copper nitrate. •Sulphuric acid gives sulphates. E.g. silver sulphate
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through the Arrhenius equation and the Eyring equation. The main factors that influence the reaction rate include: the physical state of the reactants‚ the concentrations of the reactants‚ the temperature at which the reaction occurs‚ and whether or not any catalysts are present in the reaction. Factors affecting reaction rate[edit] Nature of the reactants[edit] Depending upon what substances are reacting‚ the reaction rate varies. Acid/base reactions‚ the formation of salts‚ and ion exchange are
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Unit 11: Kinetics and Equilibrium Activated complex: an intermediate state that is formed during the conversion of reactants into products‚ the structure that results at the maximum energy point along the reaction path. Activation energy: a chemical reaction is the difference between the energy of the activated complex and the energy of the reactants. Catalyst: substance that increases the rate of a chemical reaction by reducing the activation energy‚ but which is left unchanged by the reaction
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Factors Affecting Rates of Reaction Thanks to Michelle Craig Manitoba Curriculum Chemistry Grade 12; Kinetics‚ Topic 3-08 Objectives To design short experiments to investigate and explain qualitatively using collision theory the relationship between reaction rate and temperature‚ concentration‚ catalyst‚ and surface area. Apparatus and Materials Available 3 x 250 mL beakers magnesium ribbon (1 cm) 3 x test tubes magnesium powder test tube rack mossy zinc 10 mL graduated
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favourable reactions are so slow (ex: metamorphic transformation of rocks‚ corrosion of marble sculptures owing to weathering) that they can be considered not to happen! Derivation of equilibrium constant (gases) Consider the following reaction‚ where reactants (A‚ B) and products (C‚ D) are all gases: ?? ? + ?? ? → ?? ? + ?? ? (where ?‚ ?‚ ?‚ ? are stoichiometric coefficients) The change in molar Gibbs free energy of that reaction: ∆? = ??? + ??? − ??? + ??? Which can be rewritten as: ∆? = ∆? 0 + ?? ln
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produced from reactants equals the rate at which reactants are produced from products At equilibrium a particular ratio of concentration terms equals a constant The composition of an equilibrium mixture does not change with time Kc: equilibrium constant 15.2 Law of mass action: expresses the relationship between the concentrations of the reactants and products present at equilibrium 15.3 * * LARGE VALUE OF Kc: Equilibrium mixture contains more products than reactants = product
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of the reactions we will be studying + Chemical Equilibrium Occurs when opposing reactions are proceeding at equal rates Rate at which products form is equal to the rate at which reactants disappear Have the illusion that the reaction has stopped +At equilibrium‚ the concentrations of the reactants and products are constant‚ but are not necessarily equal the reaction of iron(III) ions with thiocyanate +Equilibrium and Rates The equilibrium below is two reactions: N2O4 Forward
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given concentration of the reactants. In other words‚ the relationship of the rate of a reaction is directly proportional to the concentration. While the reaction is taking place‚ the concentration of the reactants are decreased‚ as these reactants are formed into products. During the decrease of the reactants’ concentration‚ the rate of the forward reaction also decreases. As more and more products are being formed‚ they start to reform to their constituent reactants again. This causes the reverse
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