Q1) State what is a chemical reaction. A chemical reaction is often accompanied by external indications or characteristics which include - (a) Colour change (b) Effervescence or gas evolved © Evolution or absorption of heat (d) Formation of a precipitate. With reference to each of the above indications, state the external indication seen during - (i) addition of dilute acid to active metal (ii) Addition of dilute hydrochloric acid to silver nitrate (iii) Addition of water to quicklime (iv) Thermal decomposition of mercury oxide.
Q3) Differentiate between -
Q4) Classify the following reactions into - (a) Direct combination (b) Decomposition (c) Displacement (d) Double displacement. The reactions are - (i) Zinc Hydroxide on heating gives zinc oxide & water (ii) Zinc reacts with copper sulphate to give zinc sulphate & copper (iii) Zinc sulphate reacts with ammonium hydroxide to give ammonium sulphate & zinc hydroxide (iv) Molten zinc at high temperatures, burns in air to give zinc oxide.
Q5) Give balance equations for -
Q6) State what is meant by ‘reactivity series of metals’. With reference to - (a) Water (b) Acids, Explain with suitable examples of how the reactivity of the metals could be differentiated.
Q8) State which type of chemical reactions proceed with - (a) Evolution of heat energy (b) Absorption of heat energy. State in each of the following reactions whether heat is evolved or absorbed - (i) water is added to quicklime (ii) two neutral gases on passage through an electric arc give nitric oxide (iii) two neutral gases combine to give - a basic gas
Q7) A chemical reaction may be ‘reversible’ in nature. State the meaning of the term in italics. Give a reason why a catalyst is used in certain chemical reactions. Give a balanced equation for the following - (a) A reversible catalytic reaction involving -
Q9) Certain thermal decomposition reactions result in the formation of oxides. Give balanced equations for the thermal decomposition of the following which results in the formation of a metallic oxide:
Q10) State the meaning of the term ‘oxide’. Give a balanced equation for the formation of the following oxides:
Q11) Give two examples each of the following oxides - (a) Acidic oxides (b) Basic oxides (c) Amphoteric oxides (d) Neutral oxides. State which of the following oxides i.e. (a) to (d) (i) React with water to give a base (ii) React with a base to give salt & water (iii) React with acids & bases to give salt & water.
Select the correct answer from A, B, C, D and E for each statement given below:
B: Carbonic Acid
E: Carbon monoxide
Q2) Complete the statements by filling in the blank with the correct word/words:
Q3) Give a balanced equation for each of the following types of reactions:
Q4) Differentiate between the following:
Q5) Match the chemical reactions in List I with the appropriate answer in List II
|List I||List II|
|1. XY ⇌ X + Y||A: Displacement reaction|
|2. XY → X + Y||B: Double decomposition|
|3. X+Y- + A+B- → X+B- + A+Y-||C: Endothermic reaction|
|4. X + YZ → XZ + Y||D: Thermal dissociation|
|5. X + Y → XY - △||E: Decomposition reaction|
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