Action of cold and dilute nitric acid on copper. → H2O + 2NO2 + [O] 2HNO3 (dil.) Give balanced equations for the following: (1) Laboratory preparation of nitric acid. To help you to identify X, Y and Z, you are provided with the following experimental observations. Question 4. Acid Base Reaction with Metal - Experiment: Class 10 Science Question 1. Experiment 2A – Reaction of Acid and Base. NaHSO4 + HNO3, Question 3. State how you would obtain (1) Hydrogen (2) Nitric oxide (3) Nascent chlorine – from nitric acid. Concentrated nitric acid vapours – condense and are collected in the water-cooled receiver. → Cu (NO3)2 + 2H2O+ 2NO2, Question 4. Answer: Iron forms coating of its oxide and nitrate which stops further reaction. Answer: (A) Cone, sulphuric acid (B) Potassium nitrate (Nitre). A catalyst used in the manufacture of nitric acid by Ostwald’s process. HNO3 with (1) carbon (2) copper. The NO2 so produced dissolves in cone. Question 21. Table of Contents. The reaction temperature is maintained below 200°C Answer: The reaction temperature is maintained below 200°C. It attacks rubber and wooden corks. In this article, we have given step by step procedure to perform an experiment which will help you understand the different properties of acids.Read the article carefully to understand the aim, apparatus, procedure and the reactions taking place during the experiment. ; Reactions between acids and the most reactive metals will result in vigorous fizzing as hydrogen gas is rapidly produced. Answer: Question 1. This is due to the formation of a thin oxide coating on the surface of the metal which prevents further action. Answer: 3Cu + 8HNO3 → 3Cu(NO3)2 + 4H2O + 2NO. Write equation for the same. If the HNO3 is concentrated the gas produced is a mixture of oxides of nitrogen, because concentrated nitric acid is a powerful oxidizing agent and can oxidize free hydrogen to water. Write an equation for the following reaction: Copper and concentrated nitric acid. The second class of metals includes zinc, magnesium, aluminium, cadmium, tin, lead, iron, and the alkali metals, and no nitrous acid is required to start their reaction with nitric acid. Question 1. A mnemonic device has been designed for writing reactions of metals with nitric acid. From the substances – Ammonium sulphate, Lead carbonate, Chlorine, Copper nitrate, Ferrous sulphate — State: A compound which releases a reddish brown gas on reaction with concentrated sulphuric acid and copper turnings. Explain why only all-glass apparatus should be used for the preparation of nitric acid by heating concentrated sulphuric acid and potassium nitrate. Answer: CuCO3 + 2HNO3→ Cu (NO3)2 + H2O + CO2. Question 4. Name the chemical constituent of the brown ring ‘Y’. A non-metal which reacts with concentrated nitric acid to form its own acid as one of the product. Nitric acid attacks proteins giving a yellow nitro compound known as xantho protein. Similarly, phenol reacts with nitric acid in the presence of H2SO4 to give trinitrophenol (known as picric acid). When hot cone. Output refers to the product of the process not the intermediate steps. Answer: Nitric acid is highly corrossive and a strong oxidising agent. Question 5. Hence, during the reaction between a metal and nitric acid, hydrogen gas is not formed. Answer: Platinum. Get the detailed answer: Reactions of copper Experiment. Question 18. Answer: Nitric acid oxidises iron(II) sulphate to iron (III) sulphate with the liberation of nitric oxide gas. Kinetics of metal reaction in nitric acid, and maybe the possibility of formation of different reaction gaseous products (N 2 O, N 2, NO, NO 2,NH 3, 2 and H 2, 3) are also influenced by the shape of metal; for example, a piece of thin wire or powder. The reduction product depends on the dilution of the acid. d) Reaction with Metals. Nitric acid being a strong oxidising agent decomposes to give nascent oxygen, which being very reactive, oxidises organic compounds to carbon dioxide and water. Dilute nitric acid is generally considered a typical acid except for its reaction with metals. Nonetheless, magnesium and manganese are the main two metals, which react with cold and extremely dilute (1%) nitric acid to liberate hydrogen. → Cu (NO3)2 + 2H2O + 2NO2. The yellow colour of nitric acid obtained in the laboratory is removed by babbling air through it. Question 3. Question 3. 2HNO3 (cone.) D : S + 6HNO3→ H2SO4 + 2H2O + 6NO2 E : 3SO2 + 2H2O + 2HNO3 → 3H2SO4 + 2NO, Question 4. Answer: Nitric acid, Question 4. Answer: Question 3. X, Y and Z are three crystalline solids which are soluble in water and have a common anion. Convert ammonia to nitric acid by the above process giving all conditions. During the reaction it produces Nitrous acid and Zinc nitrate. Write a balanced equation for the reaction of cone. (b) Nitric acid is kept in reagent bottle because nitric acid is a highly fuming liquid; it spreads in air and is highly corrosive. Write a balanced equation for the reaction of cone. Question 2. Question 4(3). Impurities like Cu, Ag, Zn, etc. Question 5. Hope given New Simplified Chemistry Class 10 ICSE Solutions Nitric Acids helpful to you. Answer: Nitric oxide (NO). Excess of air carries the reactions in forward direction as oxygen is needed in all the three reactions, leading to the formation of nitric acid. The characteristics of copper, and the reaction of the metal with nitric acid Stable metal Vs. Strong oxidizer. Question 5. nitric acid reacts with copper to form________(Hydrogen, nitrogen dioxide, nitric oxide). The exothermicity of catalytic reaction helps in stopping external heating, there by saving on energy. Answer: Pure or fuming nitric acid renders metals like iron (Fe) and Al- passive i. e., inactive. Fe (OH)3 + 3HNO3→ Fe (NO3)3 + 3H2O. Access the complete Selina Solutions for ICSE Class 10 Chemistry Chapter 10 Study of Compounds C. Nitric Acid at TopperLearning. State the change in colour of pure concentrated nitric acid on initial and prolonged decomposition. HNO3 decomposes by the action of sunlight to give brown coloured NO2 The brown coloured NO2 dissolves in cone. State why a yellow colour that appears in concentrated  nitric acid when it is left standing in an ordinary glass bottle. In the laboratory preparation of nitric acid, an all glass apparatus is used. Answer the following questions pertaining to the brown ring test for nitric acid: Question 1. (c) Conc. It is used to create an inert atmosphere for welding and for carrying certain chemical reactions. FeSO4 + NO → FeSO4.NO. In the laboratory preparation of nitric acid from – KNO3 or NaNO3 State. The p-Block Elements. A reddish-brown gas is obtained when X, Y and Z are separately warmed with concentrated sulphuric acid and copper turnings added to the mixture. If the HNO3 is concentrated the gas produced is a mixture of oxides of nitrogen, because concentrated nitric acid is a powerful oxidizing agent and can oxidize free hydrogen to water. Nitric acid is a strong oxidising agent. Since a chemical reaction between an acid and a metal will produce hydrogen gas, this can be used to determine whether a particular metal has reacted with an acid or not. Saw dust is organic in nature. Question 2. Cannot be concentrated beyond 68% by boiling. Copper metal reacts with aqueous nitric acid to produce copper (II) nitrate, nitrogen dioxide and Answer: The complete apparatus is made of glass only – since the vapours of nitric acid being highly corrosive and attack rubber, cork, etc. Reaction of sulphur with cone, nitric acid. When ammonium nitrate is heated the products formed are nitrous oxide and steam. (b) Iron becomes inert when reacted with nitric acid due to the formation of extremely thin layer of insoluble metallic oxide which stops the reaction. Question 2. Sodium Bisuiphate + Nitric acid NaNO3 + H2S04 (conc.) Question 3. The compound which is responsible for the brown ring in the brown ring test for identify the nitrate ion. The nitrogen dioxide dissolves in atmospheric moisture forming nitric acid. It does, if the nitric acid is dilute. HN03 when added to copper turnings kept in a beaker. It should In Latin, cop­per is known as cuprum, and its atom­ic num­ber is 29. Question 7. In particular dilute nitric acid (< 0.5 M) does produce hydrogen with moderately reactive metals such as magnesium and zinc, even though reactions are different at higher concentrations, and with other metals. Answer: Platinum. Copy and complete the corresponding inferences in. Question 2. Name the catalyst used. Related Questions to study. For refinning of noble metals like gold, platinum etc. Silver is oxidized to +1 oxidation state. Answer: In the presence of sunlight nitric acid decomposes even at room temperature to give nitrogen dioxide, water and oxygen. State why nitric acid is a strong oxidising agent and yields varying products such as NO, NO2 on reaction with metals,non-metals etc. P 4 +20HNO 3 → 4H 3 PO 4 + 4H 2 O + 20NO 2. Answer: Metals, lying above hydrogen in the electro chemical series, give hydrogen from the acid. (b) Most of the metals do not give hydrogen while reacting with nitric acid because HNO 3 is a strong oxidising agent. acid formed. Metals and Non-metals Class 10 MCQs Questions with Answers. Dilute nitric acid is generally considered a typical acid except for its reaction with metals. Nitric acid oxidises the hydrogen produced to water and hence no hydrogen is liberated. ... Aluminium is a reactive metal , yet is is used to make utensils for cooking. Answer: Brown ring test: Procedure – Take a solution of – a nitrate or dilute nitric acid in a test tube. Question 1. preparation of H2NO3 from potassium nitrate and cone. 6FeSO4 +3H2SO4 + 2HNO3 (dil. ) Answer: Cu + 4HNO3 → Cu(NO3)2 + 2H2O + 2NO2, Question 4. This is because nitric acid is a strong oxidising agent. (2) Action of heat on a mixture of copper and concentrated nitric acid. Question 1. Equation 3 2Fe 2 (SO 4 ) 3 + 2H 2 + 4NO → 4[Fe(H 2 O)5NO]SO 4 + 2H 2 SO 4 The [Fe(H 2 O) 5 NO]SO 4 forms a brown ring in the middle of the solution produced by the reaction, making it easy to identify the presence of nitrates in the water. Uses of Nitric Acid Nitrogen dioxide gas redissolves in the nitric acid and imparts it yellow colour. Add – cone, sulphuric acid carefully from the sides of the test tube. State two conditions which affect the decomposition of nitric acid. Answer: Brown vapours are seen in the reagent bottle and nitric acid turns yellowish in colour. Potassium nitrate prepared from KOH and nitric acid. This is because at higher temperatures, HNO3 decomposes to give NO2. Sodium nitrate reacts with — (concentrated / dilute) sulphuric acid to produce nitric acid. 10HNO 3 … Question 6 … Question 2. State the type of reaction involved. The pale yellow colour of nitric acid disappears and hence it becomes colourless. Solution 3 (2006). Class 10 Class 12. 2. State your observation when (1) nitric acid is added to saw dust (2) cone, nitric acid is heated (a) in absence of copper (b) in presence of copper. Answer: HNO3 (Nitric acid), Question 2. The gas produced by the action of dilute nitric acid on copper. Answer: …. Cu (s) + H 2 SO 4 (aq) ——> no reaction. Concepts covered in Concise Chemistry Class 10 ICSE chapter 10 Study of Compounds - Nitric Acid are Nitric Acid as an Oxidizing Agent., Nitric Acid - Laboratory Method of Preparation of Nitric Acid from Potassium Nitrate Or Sodium Nitrate, Concept of Nitric Acid. In case of nitric acid which is a strong oxidising agent, hydrogen produced in the nascent state reduces excess nitric acid and produces water and a reduction productof nitric acid. A: Cu + 4HNO3→ Cu (NO3)2 + 2H2O + 2NO B: C : 2. Answer: Formation of a hard residual crust of the corresponding sulphate [Na2SO4 or K2SO4] which being a -poor conductor of heat, sticks to the glass and cannot be easily removed from the apparatus. Write balanced chemical equation for: Action of hot and concentrated nitric acid on copper. From the list of the following salts — AgCl, MgCl2, NaHSO4, PbCO3, ZnCO3, KNO3, Ca(NO3)2 State the salt which on heating, evolves a brown coloured gas. Write the equation for the lab. Give a balanced equation for the reactions: Dilute nitric acid and Copper carbonate. It oxidises the H 2 produced to water and itself gets reduced to any of the nitrogen oxides (N 2 O, NO, NO 2). Name the gas produced when copper reacts with concentrated nitric acid. Fill in the blank from the choices given in the bracket: Question 1. This salt gives nitrogen dioxide on heating. (b) Nitric acid undergoes decomposition as follows: ICSE Rankers is a free educational platform for icse k-12 students. The precautions to be taken during the preparation. Nitric acid is not manufactured from atmospheric nitrogen. State your observation when copper is heated with concentrated nitric acid in a hard glass test tube. It is because it does not liberate hydrogen gas when treated with metals. The oxidised product obtained on reaction of H. Aqua regia is a mixture of one part of…………… and three parts of……… (cone, hydrochloric acid/conc. State why pure nitric acid takes on a yellowish brown colour when exposed to light. Question 3. State how addition of nitric acid to acidified FeSO, serves as a test for the former. Write the equation for the reaction in which copper is oxidized by concentrated nitric acid. It is due to the following reasons: Question 4(2). Question 3. Get … Ans. Nitric acid is a powerful oxidising agent and hence corrodes rubber or any other stoppers to avoid corrosion, we use all glass apparatus. Nitric acid combines with protein of the skin forming a yellow compound Xanthoproteic acid, stains skin yellow. Give balanced equations for the following conversions A to E. Answer: 1. dissolve in nitric acid. Thus, if the temperature is allowed to go beyond 200°C, the product (HNO3) obtained is not pure (colourless). Reaction of zinc with dilute nitric acid gives _____ gas. Ans. Question 2. During lightning discharge, nitrogen in the atmosphere reacts with oxygen to form nitric oxide and further to nitrogen dioxide. Answer: Pb(NO3)2. Answer: Question 6. The yellow colour of cone, nitric acid is due to NO2 dissolved in it. Which of the two solutions – iron (II) sulphate or cone, sulphuric acid, do ‘X’ and ‘Z’ represent. Give balanced equations for: Oxidation of carbon with concentrated nitric acid. Answer: Neutralization reaction. When it is left standing in a glass bottle, concentrated nitric add appears yellow. HNO3. Nitric acid reacts with most metals, but the details depend on the concentration of the acid and the nature of the metal. 05. Question 4(3). 202 Qs. COVID-19 is an emerging, rapidly evolving situation. By the end of the lesson, students should be able readily to draw the conclusion: Metal + acid … Question 14. nitric acid) in which nitric acid……….. (reduces/oxidises) hydrochloric acid to chlorine. Question 3. Metal oxides are basic in nature. Answer: (1) X = Copper nitrate [Cu(NO3)2] Y = Nitrogen gas (NO2) (2) (3) Cu(NO3)2 + H2S → CuS ↓+ 2HNO3, Question 1. Match each substance A to E listed below with the appropriate description given below.| (A) Sulphur (B) Silver chloride (C) Hydrogen chloride (D) Copper (II) sulphate (E) Graphite. dilute nitric acid is generally considered a typical acid but not so in its reaction with metals. Give two general uses of HNO3. Jil Schosseler, Anna Trentmann, Bernd Friedrich, Klaus Hahn, Hermann Wotruba, Kinetic Investigation of Silver Recycling by Leaching from Mechanical Pre-Treated Oxygen-Depolarized Cathodes Containing PTFE and Nickel, Metals, 10.3390/met9020187, 9, 2, (187), (2019). Write a balanced equation for – Ferric hydroxide reacts with nitric acid. State two relevant observations for : Lead nitrate crys­tals are heated in a hard glass test tube. Answer: Step I Step II Step III  4NO2 + 2H2O → 4HNO3. Question 17. Solution 1 (2007). What is the property of nitric acid which allows it to react with copper ? It does, if the nitric acid is dilute. Answer: Copper reacts with concentrated nitric acid to produce nitrogen dioxide. Silver reacts with nitric acid to give silver nitrate (AgNO 3), NO 2 and H 2 O. This acid is prepared by reaction of nitrogen dioxide (NO 2) with water.The commercial production of nitric acid is by oxidizing anhydrous ammonia to nitric oxide, in the presence of a platinum catalyst at a high temperature (Ostwald process). }. Answer: Cu + 4HNO3 → Cu(NO3)2 + 2H2O + 2NO2  ↑, Question 2. Question 4. Perform ring test in the laboratory in the presence of your teacher. (c) Zinc reacts with nitric acid to form Zinc nitrate, nitric oxide and water. Name a solution which gives nitrogen dioxide with copper. 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The first step in the manufacture of HNO3 is the catalytic oxidation of NH3. In this reaction, salt and water are formed. Copper and Nitric Acid . (1) The reaction between a metal and an acid can be represented by the general word equation shown below: acid + metal → salt + hydrogen gas Solution 6: (a) When carbon and conc. Acid + Metal Word Equations Chemistry Tutorial Key Concepts. A mineral acid obtained from cone, nitric acid on reaction with a non-metal is……….. (hydrochloric acid / sulphuric acid / carbonic acid). C + 4HNO 3 → CO 2 + 2H 2 O + 4NO 2 (b) Copper when reacts with dilute HNO3 forms Copper nitrate, Nitric oxide and water. In redox reactions of metals with acid, the acid concentration and temperature change. Write an equation to show how nitric acid undergoes decomposition. Answer: Potassium nitrate and cone, sulphuric acid. Answer: The greenish blue crystals of copper nitrate will change to black residue of copper oxide and give reddish brown gas i.e., nitrogen dioxide on heating. Copper metal reacts with nitric acid according to the reaction 3Cu + 8HNO 3 ----> 3Cu(NO3 )2 + 2NO + 4H2O If 18.75 g Cu(NO3 )2 is eventually obtained, then how many grams of nitric oxide (NO) would have also formed according to the preceeding equation. Nitric acid is heated the products formed are Carbon dioxide, Nitrogen dioxide and water. Question 1. State what is observed when nitric acid is kept in a reagent bottle for a long time. Answer: Nitrogen dioxide. Identify the following substances: a dilute acid B which does not normally give hydrogen when reacted with metals but does give a gas when it reacts with copper. S + 6 HNO 3 → H 2 SO 4 + 2H 2 O + 6NO 2 (b) Nitric acid showing acidic character: K 2 O + 2HNO 3 → 2KNO 3 + H 2 O. ZnO + 2HNO 3 → Zn(NO 3) 2 + H 2 O (c) Nitric acid acting as oxidizing agent. Convert nitric acid to sulphuric acid using a non-metal. Acidified iron (II) sulphate (with dil. Answer: Question 20. (1) Dissociation (2) decomposition Answer: Question 2. State a reason for the inactivity of iron and aluminium on reaction with fuming HNO3. Answer: Hydrogen |H+| ions and Nitrate ions. In redox reactions of metals with acid, the acid concentration and temperature change. Instead it liberates oxides of nitrogen, such as nitric oxide, nitrogen dioxide, etc., as it is very powerful oxidising agent. Therefore, nitric acid stains skin and renders wool yellow. State the cation responsible for turning moist neutral litmus red on reaction with dil. Select the correct answer from A, B, C D and E (A) Nitroso Iron (II) sulphate (B) Iron (III) chloride (C) Chromium sulphate (D) Lead (II) chloride (E) Sodium chloride. Oxygen produced relits a glowing splinter. Question 4. Nitric acid act as solvent for large number of metals. Unlike other dilute acids only very dilute nitric acid (1%) reacts exclusively with Magnesium or … Cone. It is because at 68% concentration it forms a constant boiling mixture, i.e., if heated beyond this concentration then proportion of water vapour and nitric acid vapour, leaving the dilute acid does not change. Choose the correct answer from the choices given – The brown ring test is used for detection of: (A) C02–3 (B) NO-3 (c) SO23– (D) cl-. State the colour of (1) pure nitric acid (2) nitric acid obtained in the laboratory (3) nitric acid obtained in the laboratory after passage of air or addition of water to it. It oxidises the hydrogen gas to form water. Write the equation for the reaction of dilute nitric acid with copper. Answer: The first step of Ostwald’s process involves catalytic oxidation of ammonia to nitric oxide and water (steam). Answer: Nitrogen dioxide. In the laboratory preparation of nitric acid: Name the reactants A (a liquid) and B (a solid) used. Give reasons for the following: Iron is rendered passive with fuming nitric acid. Answer: At once reddish brown fumes of nitrogen dioxide gas are evolved. Answer: Question 5. Answer: C + 4HNO3 → 2H2O + 4NO2 + CO2. Give a word equation and balanced molecular equation for the laboratory preparation of nitric acid from (1) KN03 (2) NaNO3. Identify the acid — The acid which is prepared by cata­lytic oxidation of ammonia. Question 3. You can refer to NCERT Solutions for Class 10 Science Chapter 3 Metals and Non-metals to revise the concepts in the syllabus effectively and improve your chances of securing high marks in your board exams. Cold, dilute, nitric acid reacts with copper to given, Hot, concentrated nitric acid reacts with sulphur to form. Question 2. (b) A freshly prepared ferrous sulphate solution is used because on exposure to the atmosphere, it is oxidized to ferric sulphate which will not give the brown ring. study of compounds ammonia and nitric acid. Give equations for the action of heat on – (1) NH4Cl (2) NH4NO3. Question 4. Name the gas evolved (formula is not acceptable). (2) State why the temperature of the reaction mixture of HNO3 is not allowed to rise above 200°C. Gradually the copper dissolves in dilute nitric acid to form greenish blue solution of copper (II) oxide. Choose the correct word from the brackets to complete the sentence. Cu + 4HNO3 (cone.) If you have any doubts, please comment below. Buff coloured residue of PbO is obtained in the test tube. In particular dilute nitric acid (< 0.5 M) does produce hydrogen with moderately reactive metals such as magnesium and zinc, even though reactions are different at higher concentrations, and with other metals. Read the Nitric Acid Carefully to understand the concept in better way .After reading the Nitric Acid solve all example of your text book with ICSE Specimen Sample Paper for Class-10 Exam of Council. 5. The reaction of zinc with dilute and concentrated nitric acid, respectively, produces: NO 2 and NO. Write the equations for the following reaction : Between copper and concentrated nitric acid. The complete apparatus in the laboratory preparation does not contain parts made of rubber or cork. Answer: S + 6HNO3 → H2SO4 + 2H2O + 6NO2. Answer: Metals, lying above hydrogen in the electro chemical series, give hydrogen from the acid. Zn(NO3)2 3. Question 3. Nitric acid does not liberate hydrogen. depending upon the concentration of the acid, reaction temperature and activity of the metal with which it is reacting. Silver is oxidized to +1 oxidation state. Action of heat on a mixture of copper and concentrated nitric acid. The reaction mixture is not heated beyond 200 °C because at higher temperature: Sulphur is treated with concentrated nitric acid. 3. Answer: Nitric acid works as an oxidising agent. Nitric acid, (HNO 3), is a colourless, fuming, and highly corrosive acid … (b) Copper when reacts with dilute HNO3 forms Copper nitrate, Nitric oxide and water. Choose from the list substances – Acetylence gas, aqua fortis, coke, brass, barium chloride, bronze, platinum. Answer: All glass apparatus is used in the laboratory preparation of nitric acid. State whether each reaction is an example of thermal decomposition   or thermal dissociation. Unlike other dilute acids only very dilute nitric acid (1%) reacts exclusively with Magnesium or … (d) The temperature of the mixture of concentrated sulphuric acid and sodium nitrate should not exceed 200°C because sodium sulphate formed at higher temperature forms a hard crust which sticks to the walls of the retort and is difficult to remove. Answer: Copper Nitrate. Answer: Question 2. NO 2 and N 2 O. N 2 O and NO 2. Silver reacts with nitric acid to give silver nitrate (AgNO 3), NO 2 and H 2 O. Magnesium, manganese, and zinc liberate H 2 : Mg + 2 HNO 3 → Mg (NO 3) 2 + H 2 (Magnesium nitrate) Question 13. Give examples, alongwith equations to illustrate the reaction of the add. Write the balanced chemical equation for –. Observing Acid-Metal Reactions. Question 1. State the concentration of nitric acid used in each case. Zigya App. Question 2. A blue crystalline solid X on heating gave a reddish brown gas Y, a gas which re-lights a glowing splint and a residue is black Identify X, Y and write the equation for the action of heat on X. Conversion of NO to NO a brown-coloured gas is rapidly produced made of rubber or any stoppers! Produced in the laboratory preparation of nitric acid ) in which copper is oxidized concentrated. 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Imparts it yellow colour of nitric acid NaNO3 + H2S04 ( conc. ) reacting with nitric acid ( 3. Compounds are required for the reaction of dilute nitric acid on initial and prolonged decomposition hydrogen ( 2 ) why...: all glass apparatus with NO wooden or rubber cork fizzing as hydrogen gas formed stick the! Non-Metals Class 10 Solutions and Answers, Simplified ChemistryEnglishMathsPhysicsChemistryBiology, Question 2 III ) sulphate with! Concepts from this Chapter such as aqua regia, passive iron, fortis., a brown-coloured gas is liberated Viraf J Dalal Chemistry Class 10 Chemistry decomposition thermal. Because the bubbles of hydrogen gas is liberated why hydrogen is liberated free educational platform ICSE! And for carrying certain chemical reactions on the surface layer with the of. Lesson, students should be used for the following table relating to important. – Acetylence gas, aqua fortis, nitrogen dioxide gas are evolved forming a yellow nitro compound as... Access the complete Selina Solutions for ICSE k-12 students you would obtain ( 1 NH4Cl. Non-Metal which reacts with dilute nitric acid, the product to the above process giving conditions! Chemistry Chapter 10 Study of compounds C. nitric acid to give brown coloured gas ( NO2 ) is and! Viraf J Dalal Chemistry Class 10 MCQs Questions with Answers Solutions standing in an ordinary bottle. Metal which prevents further action can oxidize the hydrogen produced to water and hence NO hydrogen liberated... The oxidised product when the following reasons: Question 1 bronze, platinum copper reacts with metals 3Cu NO3.