of Acid Reaction of acids with metal: Acids give hydrogen gas along with respective salt when they react with a metal. Example:- Hydrogen gas and zinc chloride are formed when hydrochloric acid reacts with zinc metal. Hydrogen gas and sodium chloride are formed when hydrochloric acid reacts with sodium metal. Hydrogen gas and iron chloride are formed when hydrochloric acid reacts with iron. Hydrogen gas and zinc sulphate are formed when zinc metal reacts with sulphuric acid
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Title: Enzyme Activity Aim: To investigate the activity of the enzyme catalase in liver and potatoes‚ and to investigate the effect of temperature‚ surface area‚ pH and certain chemicals on the activity of catalase. Equipment: Dilute hydrochloric acid solution x 1ml 10 volume hydrogen peroxide x 100ml Copper sulphate solution x 1ml Aluminum nitrate solution x 1ml Zinc nitrate solution x 1ml dilute NaOH solution x 1ml Mortar and pestle x 1 25ml Beaker x 1 Hot plate x1
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NSS Chemistry Part 3 Metals HKCEE Past Paper Questions – Structural Questions 1. HKCEE 1995 Q1 Rubidium (Rb) and potassium belong to the same group in the Periodic Table. The relative atomic mass of rubidium is larger then that of potassium. (a) Explain whether rubidium is more reactive than potassium. (b) Write a chemical equation for the reaction between rubidium and water. (State symbols should be given.) (c) Suggest how rubidium can be stored safely in the laboratory.
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predict that galvanizing the nail with zinc and greasing the nail and painting the nail and electroplating the nail will inhibit rusting. I also predict that adding NaCl to the test tube with water and air will promote rusting of the iron nail. Background information: Rusting is the chemical reaction between a metal and oxygen in the presence of water. In this case‚ it is the corrosion of iron. Corrosion is defined as the loss of metallic properties of a metal due to oxidation and it results in them
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electric current/ 4. Define electrolysis. 5. What is decomposition reaction? Give an example 6. Calcium oxide react with water to form calcium oxide. What type of reaction is it? 7. What happen when ferrous sulphate is heated? 8. What happen when copper metal is dipped in silver nitrate solution/Give the balance chemical equation? 9. Write chemical formula for following. a. calcium fluoride.b.iron(II)bromide 10. Write chemical names of a. Ag2O3 b.CuS c. Na2ZnO2
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TOTAL AIM: Experimentally determine the enthalpy change of the displacement reaction between zinc and copper sulphate. Zn (s) + CuSO4 (aq) Cu (s) + ZnSO4 (aq) Materials Required: 1M of CuSO4 Zinc powder Beaker Measuring Cylinder Thermometer Electronic weighing balance Spatula Thermometer Stop watch PROCEDURE: Measure 25cm3 of 1M of CuSO4 in a beaker Using a spatula take out zinc powder from its container and weigh out 2.5g of it using an electronic weighing machine. Use the
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ethanonoic acid CH3COOH aqueous sulphurous acid H2SO3 aqueous carbonic acid H2CO3 aqueous sulphuric acid H2SO4 aquous nitric acid HNO3 aquous hydrochloric acid HCl aqueous potassium hydroxide KOH aqueous sodium hydroxide NAOH copper(II) sulphate solution CuSO4 Electrolysis of Molten Compounds Molten/aqueous ionic
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very reactive metal. When stored it reacts with oxygen to form a layer magnesium oxide on its surface. This layer of magnesium oxide is quite stable and prevents further reaction of magnesium with oxygen. The magnesium ribbon is cleaned by sand paper to remove this layer so that the underlying metal can be exposed into air. Question 2: Write the balanced equation for the following chemical reactions. (i) Hydrogen + Chlorine → Hydrogen chloride (ii) Barium chloride + Aluminium sulphate → Barium sulphate
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divided into two types – Balanced Chemical Equation and Unbalanced Chemical Equation. Balanced Chemical Equation: A balanced chemical equation has number atoms of each element equal on both sides. Example: In this equation‚ numbers of zinc‚ hydrogen and sulphate are equal on both sides‚ so it is a balanced chemical equation. According to Law of Conservation of Mass‚ mass can neither be created nor
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rust and disintegrate. Surface rust is flaky and friable‚ and provides no protection to the underlying iron‚ unlike the formation of patina on copper surfaces. Rusting is the common term for corrosion of iron and its alloys‚ such as steel. Many other metals undergo equivalent corrosion‚ but the resulting oxides are not commonly called rust. Other forms of rust exist‚ like the result of reactions between iron and chloride in an environment deprived of oxygen – rebar used in underwater concrete pillars
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