# structuralism vs functionalism

i) Silver metal does not react with dilute HCI because it is located below hydrogen not be able to displace hydrogen from acid. (ii) The temperature of the reaction mixture rises when aluminium is added because it is an exothermic reaction. (i) Silver metal does not show any change. This activity is related to single displacement reaction. Metal + dil. General equation. Temperature influences the rates of reaction through kinetic energy, such that high temperatures increase the kinetic energy of reacting molecules therefore causing frequent collisions, which form products faster. Acetic acid forms acetate salts. Hydrochloric acid forms chloride salts. When added to hydrochloric acid, the metals that lose electrons are able to produce hydrogen gas and a chloride solution. Based from the activity the copper and silver are the ones did not react with hydrochloric acid this is because both copper and silver are below in position that H element, meaning they are less active than H. Do all metals react with acid in same way? Now you can throw small pieces of different metals into it carefully to see how it reacts with different metals. Second option. Reaction of some metals with hydrochoric acid (HCl) - YouTube Write balanced equations for the reaction of dilute hydrochloric acid with each of the following : Name the gas evolved when sodium hydrogen carbonate is made to react with dilute hydrochloric acid. For example, the combination of magnesium with hydrochloric acid creates magnesium chloride and hydrogen. Magnesium + hydrochloric acid → magnesium chloride + hydrogen. The chemical reaction between hydrochloric acid and magnesium produces magnesium chloride and hydrogen gas. Reactions with dilute sulfuric acid Many, but not all, metals react with acids. Examples of acid metal reactions. (iii) The reaction of sodium metal is found to be highly explosive. When magnesium reacts with hydrochloric acid, hydrogen gas is released. Mg (s) + + 2 HCl (aq) —–> MgCl2 (aq) + H2 (g) 2)Al,Fe and Zn metals also react with dilute hydrochloric acid to form corresponding metal chlorides and hydrogen gas. What's chemistry without combining a bunch of stuff together, right? The reactions of acids with metals are redox reactions. Activity series of metals is used to predict whether reaction will occur or not in single replacement reaction depending on the activity of the metal. However, there are some exceptions to this rule, including platinum, gold, silver and copper. Hydrogen gas forms as the metals react with the acid to form salts. Why ? For example, zinc metal reacts with hydrochloric acid, producing zinc chloride and hydrogen gas. The reaction is similar to the reaction with water, Magnesium reacts with hydrochloric acid according to the equation: Mg (s) + 2 HCl (aq) --> MgCl2(aq) + H2(g) This demonstration can be used to illustrate the characteristic reaction of metals with acid, a single replacement reaction, or to demonstrate the generation of hydrogen gas. The salt of the metal is named following the rules you learned in Unit 1 of the course. These include the presence or absence of catalyst, temperature, concentration, and surface area of reactants. Zinc + sulfuric acid zinc sulfate + hydrogen gas. The higher the position of metal in the activity series means more active than the metal below it. (iv) Some bubbles of a gas are seen when lead (Pb) is reacted with the acid. Metal compound A reacts with dilute hydrochloric acid to produce effervescence. Clearly, in this reaction sulfuric acid acts as the "acid", while nitric acid acts as the "base", hence sulfuric acid is indeed a stronger acid. For example, the ionic equation for the reaction of magnesium with hydrochloric acid is: 2H + (aq) + Mg(s) → Mg 2+ (aq) + H 2 (g) Name the gas evolved when sodium hydrogen carbonate is made to read with dilute hydrochloric acid. You need to employ caution while handling acids, especially if you use strong ones. The gas evolved extinguishes a burning candle. How will you test the gas ? The result is hydrogen and sodium chloride. Metals like magnesium, zinc and iron are common active metals. When metals react with acids, a salt of the metal and hydrogen gas are formed. 6. The reactions between metals and acids. 1)Magnesium metal react with dilute hydrochloric acid to form magnesium chloride and hydrogen gas. (ii) The temperature of the reaction mixture rises when aluminium (Al) is added. The balanced chemical equation for this reaction is Mg (s) + 2 HCl (aq) produces MgCl 2 (aq) + H 2 (g), where the letter "s" stands for solid, "g" is gas and "aq" represents an aqueous solution. This page shows how the position of a metal in the reactivity series affects its reactions with common dilute acids such as hydrochloric acid or sulfuric acid. During the reaction of some metals with dilute hydrochloric acid, following observations were made. Magnesium + Sulfuric Acid 3. Explain why ? Copper, silver and gold are not active enough to react with these acids. Write balanced equation for the reaction of hydrochloric acid with each of the following : Explain why metals usually do not liberate hydrogen gas with dilute nitric acid. When magnesium reacts with hydrochloric acid, a gas is released. Testing the gas 4. About 5 mL of the HCl is added to a small piece of potassium metal. A substance X which is used as an antacid reacts with dilute hydrochloric acid to produce a gas Y which is used in one type of fire-extinguisher. We are working to restore a broken URL for this simulation. Active metal + acid salt + hydrogen gas 1. Potassium, sodium, lithium and calcium all react violently with dilute sulfuric acid and dilute hydrochloric acid. Tin will react with condensed acid but diluted acid the reaction will need to be sped up by heat, tin is the most nonreactive of group 2 metals GCSE ... Metal + acid = salt + hydrogen. Reactions of dilute nitric acid with some metals are typical of an acid, namely: $\ce{Mg + 2 HNO3 → Mg(NO3)2 + H2\uparrow}$ Other metals that react in this fashion are manganese and zinc. Nitric acid forms nitrate salts. Activity 4 in this program has an abbreviated set of metals with HCl(aq). The balanced formula for this is: Mg(s) + 2HCL(aq) MgCl2(aq) + H2(g) Magnesium + hydrochloric acid Magnesium Chloride + Hydrogen Magnesium will react with hydrochloric acid, because it is higher in the reactivity series than hydrogen. Sodium has a violent reaction when exposed to dilute hydrochloric acid. Al … Metals react with acid Bubbles of gas are Produced 3. Each metal reacts with dilute hydrochloric acid, producing bubbles of hydrogen gas and a colorless solution of the metal chloride: (1) X + 2 H C l → X C l 2 + H 2 These reactions become more vigorous down the group. This video shows some metals that react and do not react with hydrochloric acid. High concentrations imply that more reacting molecules are at high proximity to each o… The reactivity of six metals are qualitatively tested by adding 3M HCl. Students add powdered or finely-divided metals to hydrochloric acid and measure the temperature changes. As discussed previously, metals that are more active than acids can undergo a single displacement reaction. Reactions with dilute hydrochloric acid All the metals react with dilute hydrochloric acid to give bubbles of hydrogen and a colourless solution of the metal chloride. How will you test the gas ? Potassium metal reacts with hydrochloric acid in this video. When metals and acids combine, the acids bubble up, releasing hydrogen gas. (iii) Reaction of sodium metal is found to be highly explosive because it is an exothermic reaction, (iv) When lead is treated with hydrochloric acid, bubbles of hydrogen gas are evolved Pb + 2HCl → PbCl2 + H2. The negative ion of the salt produced in an acid-metal reaction is determined by the acid. The reaction of lead with acids is slow. Reaction of sodium metal with dilute acid: Sodium metal gives sodium chloride and hydrogen gas when it reacts with dilute hydrochloric acid. 2Na + 2HCl ⇨ 2NaCl + H 2. Sulfuric acid forms sulfate salts. This class experiment is often used in the introductory study of acids to establish that this behaviour is a characteristic property Nitric acid (another common acid) behaves differently with metals for reasons that are too complicated to talk about at this early stage of a course. Zinc liberates hydrogen gas when reacted with dilute hydrochloric acid, whereas copper does not. With dilute acids, metals usually displace the hydrogen. Choose Activity 1, then choose Activity 4 to navigate to the metals + hydrochloric acid section. Metals form respective salts when react with dilute acid. acid ⇨ Metal salt + Hydrogen. Reaction of metal with Acid Metal + Hydrochloric → Salt + Hydrogen Acid 5. $\ce{Zn(s) + 2HCl(aq) → ZnCl2(aq) + H2(g)}\nonumber$ Bases also react with certain metals, like zinc or aluminum, to produce hydrogen gas. It is dangerous to put these metals into an acid. Mg(s) + 2HCl(aq) → MgCl 2 (aq) + H 2 (g) The more reactive the metal, the more rapid the reaction is. They are unable to displace the hydrogen when an anion is not metal. Metals that react with the acid dissolve and disappear in the acid; They form a salt with the acid; The word equation for these is: \text{metal + acid}\rightarrow\text{salt +hydrogen} If the metals react with sulphuric acid the salts are called sulphates; If hydrochloric acid reacts with metals to form salts known as chloride; For example: To try this out take 30 ml of concentrated hydrochloric acid in a beaker. When aluminum reacts with a strong acid (such as hydrochloric acid), hydrogen gas is formed. The experiment reinforces ideas about energy changes during reactions, the reactivity seriesof the metals, and the chemical behaviour of acids. The black colour of copper oxide changes to bluish-green if reacted with dilute hydrochloric acid. On adding dilute hydrochloric acid to copper oxide powder the solution formed is blue-green. In acid-base chemical reactions, there are four main variables, which influence the rate of reaction. 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