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ChemistryClass 10ICSE

One of the following does not happen during a chemical reaction This is : (a) Breaking of old chemical bonds and formation of new chemical bonds (b) Formation of new substances with entirely different properties (c) Atoms of one element change into those of another element to form new products A rearrangement of atoms takes place to form new products

Option (c) is the answer. Atoms of one element does not change into another element to form products but the bonds between these atom will break and form products and atoms are rearrange also

ChemistryClass 10ICSE

What do you understand by exothermic and endothermic reactions? (b) Give one example of an exothermic reaction and one of an endothermic reaction. (c) Which of the following are endothermic reactions and which are exothermic reactions? (i) Burning of natural gas (ii) Photosynthesis (iii) Electrolysis of water Solution: (iv) Respiration (v) Decomposition of calcium carbonate

Exothermic reaction is a reaction takes place when energy is released from the system into the surroundings Endothermic reaction is a reaction takes place when energy is absorbed from surroundings in the form of heat The thermal decomposition of Limestone CaCO3(s)→CaO (s)+CO2(g) This is an example for endothermic reaction Burning of fuel is an example for exothermic reaction C8H18(l)+25O2(g)→16CO2(g)+18H2O (g)+heat (i) and (iv) are exothermic (ii),(iii),(v) are endothermic reactions

ChemistryClass 10ICSE

State the various characteristics of chemical reactions. (b) State one characteristics each of the chemical reaction which takes place when: (i) Dilute hydrochloric acid is added to sodium carbonate (ii) Lemon juice is added gradually to potassium permanganate solution (iii) Dilute sulphuric acid is added to barium chloride solution (iv) Quicklime is treated with water Wax is burned in the form of a candle

A chemical reaction is a reaction that takes place to form new substance by reacting with It is characterised by Evolution of a gas, Change in colour, Formation of a precipitate, Change in temperature, Change in state. (i) Evolution of Carbon dioxide gas Change in colour from purple to colourless Formation of a white precipitate of Barium sulphate Change in temperature, an exothermic reaction Change in state from solid to liquid and gas

ChemistryClass 10ICSE

What is meant by a chemical reaction? Explain with the help of an example. (b) Give one example each of a chemical reaction characterised by: (i) Evolution of a gas (ii) Change in colour (iii) Formation of a precipitate (iv) Change in temperature Change in state.

A chemical reaction results in new substances by undergoing certain reactions and There will be reactants on the left hand side and products on the right hand side. An example of combustion is methane + oxygen forms carbon dioxide and water. This can be written as a balanced symbol equation: CH4 + 2O2 →CO2 + 2H2O (i) Evolution of gas Reaction of Zinc and Hydrochloric acid Zn + 2HCl → ZnCl2 + H2(g) Hydrogen gas is released in the form of diatomic molecule Change in colour Cu(s) + O2(g) + H2O → Cu(OH)2(s) + O2(g) Copper is in reddish brown colour and when reacts with oxygen and water it forms hydrated copper carbonate which is green in colour Formation of precipitate AgNO3(aq) + KCl(aq) →AgCl(s) + KNO3 When silver nitrate and potassium chloride in its aqueous form reacts a precipitate of potassium nitrate is obtained Change in temperature CaO + H20 →Ca(OH)2 When Quick lime is added to water to form slaked lime a change in temperature is obtained as it reacts vigorously and produce heat which is an exothermic reaction Change in state NH3(g) + HCl(g) → NH4Cl(s) Ammonia and Hydrogen chloride gas reacts to form Ammonium chloride which is a solid

ChemistryClass 10ICSE

• When potassium nitrate is heated, it decomposes into potassium nitrite and oxygen. Write a balanced equation for this reaction and add the state symbols of the reactants and products.

2KNO3 (s)→ 2KNO2 (s) + O2 (g)

ChemistryClass 10ICSE

Translate the following statement into chemical equation and then balance it: ‘Barium chloride solution reacts with aluminium sulphate solution to form a precipitate of barium sulphate and aluminium chloride solution’.

3BaCl2 (aq) + Al2(SO4)3 (aq) → 3BaSO4 (s) + 2AlCl3 (aq)

ChemistryClass 10ICSE

Write a balanced chemical equation for the process of photosynthesis giving the physical states of all the substances involved and the conditions of the reaction.

6CO2 (g) + 6H2O (l) → C6H12O6 (aq.) + 6O2 (g) in the presence of sunlight

ChemistryClass 10ICSE

Ammonia reacts with oxygen to form nitrogen and water. Write a balanced chemical equation for this reaction. Add the state symbols for all the reactants and products.

4NH3 (g) + 3O2 (g) → 2N2 (g) + 6H2O (l)

ChemistryClass 10ICSE

(a) Substitute formulae for names and balance the following equations: Calcium carbonate reacts with hydrochloric acid to produce calcium chloride, water and carbon dioxide gas. (b) Write balanced chemical equation with state symbols for the following reaction: Sodium hydroxide solution reacts with hydrochloric acid solution to produce sodium chloride solution and water.

(a) CaCO3 + 2HCl → CaCl2 + H2O + CO2 (b) NaOH (aq) + HCl (aq) → NaCl (aq) + H2O (l)

ChemistryClass 10ICSE

(a) Potassium chlorate (KClO3) on heating forms potassium chloride and oxygen. Write a balanced equation for this reaction and indicate the evolution of gas. (b) Rewrite the following information in the form of a balanced chemical equation: Magnesium burns in carbon dioxide to form magnesium oxide and carbon.

(a) 2KClO3 (s) → 2KCl (s) + 3O2 (g) (b) 2Mg + CO2 → 2MgO + C

ChemistryClass 10ICSE

Carbon monoxide reacts with hydrogen under certain conditions to form methanol (CH3OH). Write a balanced chemical equation for this reaction indicating the physical states of reactants and product as well as the conditions under which this reaction takes place.

CO(g) + 2H2(g) → CH3OH Pressure: 300atm Temperature: 300℃ Catalyst: zinc oxide and chromium oxide

ChemistryClass 10ICSE

Write the balanced chemical equations for the following reactions, and add the state symbols: (a) Magnesium carbonate reacts with hydrochloric acid to produce magnesium chloride, carbon dioxide and water. Sodium hydroxide reacts with sulphuric acid to produce sodium sulphate and water.

MgCO3 (s) + 2HCl (aq) →MgCl2 (aq) + CO2 (g) + H2O (l) 2NaOH (aq) + H2SO4 (aq) →Na2SO4 (aq) + 2H2O (l)

ChemistryClass 10ICSE

Aluminium hydroxide reacts with sulphuric acid to form aluminium sulphate and water. Write a balanced equation for this reaction. (b) Balance the following chemical equation: MnO2 + HCl → MnCl2 + Cl2 + H2O

(a) 2Al(OH)3 + 3H2SO4 → Al2(SO4)3 + 6H2O (b) MnO2 + 4HCl → MnCl2 + Cl2 + 2H2O

ChemistryClass 10ICSE

Write any two observations in an activity which may suggest that a chemical reaction has taken place. Give an example in support of your answer

Change in temperature When calcium oxide reacts vigorously with water to produce calcium hydroxide a large amount of heat is evolved and thus temperature of the system increases hence it confirms that a chemical reaction has been taken place. Gas evolution When calcium carbonate is heated it decomposes into calcium oxide and carbon dioxide. Here carbon dioxide is a gas and thus confirms a chemical reaction

ChemistryClass 10ICSE

(a) Explain, with example, how the physical states of the reactants and products can be shown in a chemical equation. (a) Balance the following equation and add state symbols: Zn + HCl → ZnCl2 + H2 (b) Convey the following information in the form of a balanced chemical equation: "An aqueous solution of ferrous sulphate reacts with an aqueous solution of sodium hydroxide to form a precipitate of ferrous hydroxide and sodium sulphate remains in solution."

The physical state of the reactants and products in a chemical reaction can be shown by using the letters in the round brackets if it is solid then (s) liquid (l) gas (g) and aqueous (aq) Example: Ca(OH)2 (aq) + CO2 (g) → CaCO3 (s) + H2O (l) Zn (s) + 2HCl (aq) → ZnCl2 (aq) + H2 (g) FeSO4(aq) + 2NaOH (aq) → Fe(OH)2 (s) + Na2SO4 (aq)

ChemistryClass 10ICSE

What is a balanced chemical equation? Why should chemical equations be balanced? b) Aluminium burns in chlorine to form aluminium chloride (AlCl3). Write a balanced chemical equation for this reaction. c) Potassium metal reacts with water to give potassium hydroxide and hydrogen gas. Write a balanced chemical equation for this reaction.

A chemical equation can be written by balancing total number of atoms of each element in reactants and A chemical equation should be balanced so that it can follow Law of conservation of mass. 2Al + 3Cl2 → 2AlCl3 2K + 2H2O → 2KOH + H2

ChemistryClass 10ICSE

What are the various ways in which a chemical equation can be made more informative? Give examples to illustrate your answer. (b) Write balanced chemical equation from the following information: An aqueous calcium hydroxide solution (lime water) reacts with carbon dioxide gas to produce a solid calcium carbonate precipitate and water.

(a) Ca(OH)2 (aq)+ CO2 (g)---3000°C →CaCO3(s)+H2O(l) A chemical equation can be informative by 1) The chemical states is indicated by (s) for solids, (l) for liquids and (g) for gases and (aq) for aqueous solution 2) Temperature written on the above of arrow 3) Arrow upwards shows compound or any gas formed escaped or liberated 4) Arrow downwards shows precipitated 5) Heat is written on reactant side to indicate exothermic and when on written product side it will be endothermic b) Ca(OH)2 (aq) + CO2 (g) → CaCO3 (s) + H2O (l)

ChemistryClass 10ICSE

When hydrogen is passed over copper oxide, copper and steam are formed. Write a balanced equation for this reaction and state which of the chemicals are: (i) Elements (ii) Compounds (iii) Reactants (iv) Products (v) Metals Non-metals

Solutions: H2 + CuO→ Cu + H2O Elements : H2 and Cu Compounds : CuO and H2O Reactants: H2 and CuO Products: Cu and H2O Metal: Cu Non-metal: H2

ChemistryClass 10ICSE

What is a chemical equation? Explain with the help of an example. (b) Giving examples, state the difference between balanced and unbalanced chemical equations. (c) Balance the following chemical equations: (i) NH3 → N2 + H2 (ii) C +CO2→ CO

(a) Solutions: Chemical equations are the symbolic representation of chemical reactions in which the reactants and products are expressed in terms of chemical formulae. Reactant entities are given on the left side and product entities are given on the right side of a chemical equation Example: Zn + H2SO4→ZnSO4 + H2 A balanced chemical equation is always energy and mass conservative whereas unbalanced chemical equation is neither energy nor mass conservative. A chemical equation can be written by balancing total number of atoms of each element in reactants and products while in unbalanced chemical equations the total number of atoms of each element in reactants and products are not equal Example: KClO3→KCl + 3O2 Unbalanced equation 2KCl03→2KCl + 3O2 Balanced equation (i) 2NH3 → N2 + 3H2 (ii) C +CO2→ 2CO

ChemistryClass 10ICSE

(a) Give one example of a chemical reaction. (b) State two characteristics of the chemical reaction which takes place when dilute sulphuric acid is poured over zinc granules. (c) Give two characteristics of the chemical reaction which occurs on adding potassium iodide solution to lead nitrate solution.

A chemical reaction results in new substances by undergoing certain reactions and There will be reactants on the left hand side and products on the right hand side. An example for chemical reaction is An example of combustion is methane + oxygen forms carbon dioxide and water. This can be written as a balanced symbol equation: CH4 + 2O2 →CO2 + 2H2O When dilute sulphuric acid is poured over zinc granules heat will liberate thus the reaction becomes exothermic Hydrogen gas is evolved which burns with a sound 2KI (aq) + Pb(NO ) (aq) → PbI (↓) + 2 KNO (aq) When solutions of lead nitrate and potassium iodide are mixed together a yellow precipitate of lead iodide is formed. This is an example for Double Displacement Reaction.

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