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reactants."},{"text":"The reversible arrow: $\\rightarrow$","correct":false,"explanation":"A single right-pointing arrow represents a reaction proceeding only from reactants to products. A reversible reaction is shown by the opposing arrows $\\rightleftharpoons$."},{"text":"The reversible arrow: $\\leftarrow$","correct":false,"explanation":"A single left-pointing arrow shows only one direction, even though that direction is reversed. The symbol $\\rightleftharpoons$ shows that both reactions can occur."},{"text":"The reversible arrow: $=$","correct":false,"explanation":"An equals sign expresses equality and is not a chemical reaction arrow. Reversible reactions use $\\rightleftharpoons$ to show possible changes in both directions."}]},{"id":"2b447153-7290-4dac-9fbb-2c7e5689b734","cardType":"basic","points":1,"front":"What can the products of a reversible reaction do?","back":"They can react to form the original reactants.","mcqOptions":[{"text":"They can react to form the original reactants.","correct":true,"explanation":"In a reversible reaction, the products of the forward reaction can react together in the reverse reaction, reforming the substances that were originally present."},{"text":"They can react to form completely new reactants.","correct":false,"explanation":"Reversibility does not produce a different set of starting substances. The products undergo the reverse reaction to form the original reactants again."},{"text":"They can remain unchanged under all conditions.","correct":false,"explanation":"Products are not necessarily permanently unchanged because suitable conditions can favour the reverse reaction. They can then react to form the original reactants."},{"text":"They can react without forming any substances.","correct":false,"explanation":"Chemical reactions rearrange atoms into substances rather than making matter disappear. In the reverse reaction, the products form the original reactants."}]},{"id":"abaa03b1-b748-4b74-8b14-da4d9ece5536","cardType":"basic","points":1,"front":"What is the forward reaction?","back":"The change from left to right.","mcqOptions":[{"text":"The change from left to right.","correct":true,"explanation":"Chemical equations conventionally place reactants on the left and products on the right, so the forward reaction changes reactants into products from left to right."},{"text":"The change from right to left.","correct":false,"explanation":"Confusing the two arrow directions makes this tempting, but right to left is the reverse reaction. The forward reaction proceeds from left to right."},{"text":"The change from products to reactants.","correct":false,"explanation":"Changing products back into reactants describes the reverse reaction. The forward reaction changes the left-hand reactants into the right-hand products."},{"text":"The change from equilibrium to completion.","correct":false,"explanation":"The forward reaction is defined by its direction, not by whether equilibrium or completion is reached. It is the change from left to right."}]},{"id":"832ccd52-ac84-491e-8ef0-789dd0a102eb","cardType":"basic","points":1,"front":"What is the reverse reaction?","back":"The change from right to left.","mcqOptions":[{"text":"The change from right to left.","correct":true,"explanation":"The reverse reaction converts the products shown on the right of the equation back into the reactants shown on the left."},{"text":"The change from left to right.","correct":false,"explanation":"Reversing the definitions is a common mistake: left to right is the forward reaction. The reverse reaction proceeds from right to left."},{"text":"The change from reactants to products.","correct":false,"explanation":"Reactants changing into products describes the forward reaction. In the reverse reaction, the right-hand products change back into the left-hand reactants."},{"text":"The change from equilibrium to completion.","correct":false,"explanation":"A reverse reaction is identified by its direction rather than by reaching completion. It is the chemical change proceeding from right to left."}]},{"id":"7f111a73-b68e-4875-a3b1-30df89c5ad44","cardType":"basic","points":2,"front":"How can changing reaction conditions affect a reversible reaction?","back":"It can change which direction happens.","mcqOptions":[{"text":"It can change which direction happens.","correct":true,"explanation":"Changing conditions can favour either the forward or reverse reaction, affecting whether reactants form products or products change back into reactants."},{"text":"It can change which atoms are conserved.","correct":false,"explanation":"Reaction conditions do not alter the conservation of atoms; every element remains conserved. They can instead change which direction of the reversible reaction is favoured."},{"text":"It can change which elements are created.","correct":false,"explanation":"Ordinary chemical conditions cannot create new elements because chemical reactions only rearrange existing atoms. Conditions can change which direction of a reversible reaction occurs."},{"text":"It can change which catalyst is consumed.","correct":false,"explanation":"A catalyst is not consumed and does not determine the favoured direction of a reversible reaction. Changing conditions can instead favour the forward or reverse direction."}]},{"id":"5d6263ff-b31c-47e9-9f2d-4dd2217bd0d4","cardType":"basic","points":1,"front":"Give one reaction condition that can change the direction of a reversible reaction.","back":"Temperature or the amount of a substance present.","mcqOptions":[{"text":"Temperature or the amount of a substance present.","correct":true,"explanation":"Changing temperature or changing how much of a reactant or product is present can favour one direction of a reversible reaction over the other."},{"text":"A catalyst or the surface area of a solid present.","correct":false,"explanation":"Catalysts and surface area can alter reaction rates, but they do not favour the forward direction over the reverse. Temperature or substance amount can change the favoured direction."},{"text":"Stirring or the shape of the reaction vessel used.","correct":false,"explanation":"Stirring can improve mixing, while vessel shape normally does not determine reaction direction. Temperature or the amount of a substance can favour one direction."},{"text":"Particle colour or the material of the thermometer used.","correct":false,"explanation":"Colour and thermometer material do not control the direction of a reversible reaction. Temperature or the amount of a reactant or product can do so."}]},{"id":"cf94dbef-a652-4273-b8fe-486c4480c263","cardType":"basic","points":2,"front":"What happens when solid ammonium chloride is heated?","back":"It breaks down into ammonia and hydrogen chloride gases.","mcqOptions":[{"text":"It breaks down into ammonia and hydrogen chloride gases.","correct":true,"explanation":"Heating ammonium chloride causes thermal decomposition, producing ammonia gas and hydrogen chloride gas in the forward direction of this reversible reaction."},{"text":"It breaks down into nitrogen and chlorine gases.","correct":false,"explanation":"This incorrectly assumes ammonium chloride separates into its elements. Heating it produces the compounds ammonia and hydrogen chloride as gases."},{"text":"It breaks down into hydrogen and ammonium gases.","correct":false,"explanation":"Ammonium is an ion rather than a gas produced in this decomposition. Heated ammonium chloride forms ammonia gas and hydrogen chloride gas."},{"text":"It breaks down into ammonia and chlorine gases.","correct":false,"explanation":"The chloride combines with hydrogen to form hydrogen chloride, not chlorine gas. The two products are ammonia and hydrogen chloride gases."}]},{"id":"ef640914-9634-40fd-9972-a09653c2f79d","cardType":"basic","points":1,"front":"What happens when ammonia and hydrogen chloride gases are cooled?","back":"They react to form solid ammonium chloride.","mcqOptions":[{"text":"They react to form solid ammonium chloride.","correct":true,"explanation":"On cooling, ammonia and hydrogen chloride undergo the reverse reaction and combine, producing solid ammonium chloride as a white deposit."},{"text":"They react to form liquid ammonium chloride.","correct":false,"explanation":"Cooling does not produce liquid ammonium chloride under these conditions. The gases combine in the reverse reaction to form solid ammonium chloride."},{"text":"They react to form solid ammonium hydroxide.","correct":false,"explanation":"Ammonium hydroxide would require water, which is not one of the two reacting gases. Ammonia and hydrogen chloride combine to form solid ammonium chloride."},{"text":"They react to form solid ammonia chloride.","correct":false,"explanation":"The ionic compound is named ammonium chloride, not ammonia chloride. Cooling ammonia and hydrogen chloride gases produces solid ammonium chloride."}]},{"id":"83aa136d-075d-40b5-866c-37d6055a5b59","cardType":"basic","points":1,"front":"What does blue hydrated copper(II) sulfate contain?","back":"Water joined to the copper sulfate.","mcqOptions":[{"text":"Water joined to the copper sulfate.","correct":true,"explanation":"Hydrated copper(II) sulfate contains water of crystallisation incorporated into its crystal structure, which gives the hydrated compound its characteristic blue colour."},{"text":"Hydrogen joined to the copper sulfate.","correct":false,"explanation":"Hydration means that water, not hydrogen alone, is incorporated into the crystal structure. Hydrated copper(II) sulfate therefore contains water joined to the copper sulfate."},{"text":"Oxygen joined to the copper sulfate.","correct":false,"explanation":"Although sulfate already contains oxygen, hydration specifically refers to water in the crystal structure. Blue hydrated copper(II) sulfate contains water joined to the copper sulfate."},{"text":"Ammonia joined to the copper sulfate.","correct":false,"explanation":"This confuses hydration with the formation of an ammonia complex. Hydrated copper(II) sulfate contains water joined within the copper sulfate crystal structure."}]},{"id":"08ff59d5-b831-4ebb-87cb-66182c54392f","cardType":"basic","points":1,"front":"What colour is hydrated copper(II) sulfate?","back":"Blue.","mcqOptions":[{"text":"Blue.","correct":true,"explanation":"Water of crystallisation gives hydrated copper(II) sulfate its blue appearance, distinguishing it from white anhydrous copper(II) sulfate."},{"text":"White.","correct":false,"explanation":"White is the colour of anhydrous copper(II) sulfate after its water has been removed. Hydrated copper(II) sulfate is blue."},{"text":"Green.","correct":false,"explanation":"Green may be associated with some other copper compounds, but hydrated copper(II) sulfate has a characteristic blue colour because it contains water of crystallisation."},{"text":"Pink.","correct":false,"explanation":"Pink is associated with hydrated cobalt chloride rather than hydrated copper(II) sulfate. Hydrated copper(II) sulfate is characteristically blue."}]},{"id":"9bf759d9-4ae3-4808-844b-e071bf1a5d3d","cardType":"basic","points":2,"front":"What happens when hydrated copper(II) sulfate is heated?","back":"It loses water and leaves white anhydrous copper(II) sulfate.","mcqOptions":[{"text":"It loses water and leaves white anhydrous copper(II) sulfate.","correct":true,"explanation":"Heating removes water of crystallisation from blue hydrated copper(II) sulfate, leaving white anhydrous copper(II) sulfate behind."},{"text":"It loses oxygen and leaves blue anhydrous copper(II) sulfate.","correct":false,"explanation":"Heating removes water, not oxygen, from the hydrated salt. The product is white anhydrous copper(II) sulfate rather than a blue anhydrous solid."},{"text":"It loses sulfate and leaves white hydrated copper(II) oxide.","correct":false,"explanation":"Normal heating in this reversible change removes water of crystallisation rather than sulfate. It leaves white anhydrous copper(II) sulfate."},{"text":"It loses copper and leaves blue hydrated sulfuric acid.","correct":false,"explanation":"Copper atoms are not removed during dehydration, and sulfuric acid is not formed. Heating removes water and leaves white anhydrous copper(II) sulfate."}]},{"id":"1265ce8b-193b-4841-84d1-329b3b906410","cardType":"basic","points":1,"front":"What happens when water is added to anhydrous copper(II) sulfate?","back":"The white solid turns blue.","mcqOptions":[{"text":"The white solid turns blue.","correct":true,"explanation":"Anhydrous copper(II) sulfate takes up the added water and becomes hydrated copper(II) sulfate, causing the colour change from white to blue."},{"text":"The white solid turns green.","correct":false,"explanation":"Green is not the colour of hydrated copper(II) sulfate. Adding water rehydrates the white anhydrous salt, so it turns blue."},{"text":"The white solid turns pink.","correct":false,"explanation":"Pink is commonly linked to hydrated cobalt chloride, which is a different chemical test. Anhydrous copper(II) sulfate turns blue when water is added."},{"text":"The white solid turns black.","correct":false,"explanation":"Black copper oxide is not formed by simply adding water. The white anhydrous copper(II) sulfate becomes blue hydrated copper(II) sulfate."}]},{"id":"d701e5cd-39b7-4cb0-be54-fa35532a0fb4","cardType":"basic","points":1,"front":"Why is the copper sulfate colour change useful?","back":"It tests for the presence of water.","mcqOptions":[{"text":"It tests for the presence of water.","correct":true,"explanation":"White anhydrous copper(II) sulfate turns blue when it becomes hydrated, so this colour change provides a chemical test for water."},{"text":"It tests for the presence of oxygen.","correct":false,"explanation":"The colour change occurs through hydration, not oxidation. White anhydrous copper(II) sulfate turns blue specifically when water is present."},{"text":"It tests for the presence of chlorine.","correct":false,"explanation":"Chlorine does not cause this hydration colour change. Anhydrous copper(II) sulfate changes from white to blue in the presence of water."},{"text":"It tests for the presence of ammonia.","correct":false,"explanation":"Although ammonia can interact with copper compounds, this white-to-blue test depends on hydration. It is used to detect the presence of water."}]},{"id":"712bdcae-8b5e-4ba1-b294-7ac2b84c8663","cardType":"cloze","points":null,"front":"A reversible reaction can go both ways, shown by the $\\text{[...]}$ symbol.","back":"A reversible reaction can go both ways, shown by the $\\boxed{\\rightleftharpoons}$ symbol.","mcqOptions":[{"text":"$$\\rightleftharpoons$","correct":true,"explanation":"The pair of arrows pointing in opposite directions indicates that both the forward and reverse reactions can occur, making the reaction reversible."},{"text":"$$\\rightarrow$","correct":false,"explanation":"A single right-pointing arrow only shows reactants changing into products. The opposing-arrow symbol $\\rightleftharpoons$ is required to show that a reaction can go both ways."},{"text":"$$\\leftarrow$","correct":false,"explanation":"A single left-pointing arrow shows only one reaction direction rather than both. Reversibility is represented by the opposing arrows $\\rightleftharpoons$."},{"text":"$$=$","correct":false,"explanation":"An equals sign represents equality, not a chemical process occurring in two directions. Reversible reactions are shown using the symbol $\\rightleftharpoons$."}]},{"id":"b407f45b-1bee-43c0-abba-4e7db876768e","cardType":"cloze","points":null,"front":"Heating solid ammonium chloride produces [ ] and hydrogen chloride gas.","back":"Heating solid ammonium chloride produces ammonia and hydrogen chloride gas.","mcqOptions":[{"text":"ammonia","correct":true,"explanation":"Heating ammonium chloride causes it to decompose into ammonia gas and hydrogen chloride gas; the products can recombine when cooled."},{"text":"nitrogen","correct":false,"explanation":"This assumes the compound decomposes into simpler elements, but nitrogen gas is not formed. Heated ammonium chloride produces ammonia and hydrogen chloride gases."},{"text":"chlorine","correct":false,"explanation":"Chlorine gas is not released because the chloride forms hydrogen chloride. The other gaseous product formed from heated ammonium chloride is ammonia."},{"text":"oxygen","correct":false,"explanation":"Ammonium chloride contains no oxygen atoms, so oxygen gas cannot be produced. Heating it forms ammonia gas together with hydrogen chloride gas."}]},{"id":"fb7417bf-f229-4149-a531-fa2268dc6f3b","cardType":"cloze","points":null,"front":"Heating solid ammonium chloride produces ammonia and [ ] gas.","back":"Heating solid ammonium chloride produces ammonia and hydrogen chloride gas.","mcqOptions":[{"text":"hydrogen chloride","correct":true,"explanation":"Thermal decomposition of ammonium chloride produces ammonia gas and hydrogen chloride gas, which can recombine to form solid ammonium chloride when cooled."},{"text":"hydrogen peroxide","correct":false,"explanation":"Hydrogen peroxide contains oxygen, but ammonium chloride supplies no oxygen atoms. Its gaseous decomposition products are ammonia and hydrogen chloride."},{"text":"chlorine","correct":false,"explanation":"The chloride does not form elemental chlorine during this reversible decomposition. It combines with hydrogen, producing hydrogen chloride gas alongside ammonia."},{"text":"carbon dioxide","correct":false,"explanation":"Ammonium chloride contains no carbon or oxygen, so carbon dioxide cannot form. Heating produces ammonia and hydrogen chloride gases."}]},{"id":"d0747f65-add7-4294-ab1c-78d52027fc71","cardType":"cloze","points":null,"front":"On cooling, ammonia and hydrogen chloride gases form solid [ ].","back":"On cooling, ammonia and hydrogen chloride gases form solid ammonium chloride.","mcqOptions":[{"text":"ammonium chloride","correct":true,"explanation":"Ammonia reacts reversibly with hydrogen chloride to produce solid ammonium chloride. Cooling favours the forward reaction, so the two colourless gases combine to form a white solid."},{"text":"ammonium hydroxide","correct":false,"explanation":"Ammonium hydroxide is associated with ammonia dissolved in water, not the reaction between ammonia and hydrogen chloride. These gases combine on cooling to form solid ammonium chloride."},{"text":"hydrogen chloride","correct":false,"explanation":"Hydrogen chloride is one of the gaseous reactants, so it is not the solid product formed when the mixture cools. The product is solid ammonium chloride."},{"text":"ammonium nitrate","correct":false,"explanation":"Ammonium nitrate contains nitrate ions and would require a source of nitric acid or nitrate ions. Ammonia and hydrogen chloride instead combine to form ammonium chloride."}]},{"id":"8345b5a7-454e-46dc-8359-ec98fb26f5f4","cardType":"cloze","points":null,"front":"Heating hydrated copper(II) sulfate leaves white [ ].","back":"Heating hydrated copper(II) sulfate leaves white anhydrous copper(II) sulfate.","mcqOptions":[{"text":"anhydrous copper(II) sulfate","correct":true,"explanation":"Heating hydrated copper(II) sulfate removes its water of crystallisation. The blue hydrated crystals therefore become white anhydrous copper(II) sulfate, and adding water reverses the change."},{"text":"hydrated copper(II) sulfate","correct":false,"explanation":"Hydrated copper(II) sulfate is the blue starting material because it still contains water of crystallisation. Heating removes this water and leaves white anhydrous copper(II) sulfate."},{"text":"anhydrous copper(II) oxide","correct":false,"explanation":"Confusing sulfate with oxide gives the wrong copper compound; copper(II) oxide is black rather than white. Gentle heating removes water and leaves anhydrous copper(II) sulfate."},{"text":"anhydrous copper(I) sulfate","correct":false,"explanation":"Heating off water does not change copper’s oxidation state from +2 to +1. It only removes water of crystallisation, producing white anhydrous copper(II) sulfate."}]}]}],"examCountdown":{"examDate":"2027-05-17","paperLabel":"Paper 1"},"heading":"6.2.1 Reversible reactions","title":"6.2.1 Reversible reactions Flashcards","topbar":{"backHref":"/gcse/chemistry/aqa/flashcards"},"topicSidebar":"$L36"}]}],"topicId":"862ae474-da90-5882-857d-9dbd7b59e50f","walled":"$L37"}],"$L38","$L39"]