Q: Question 6State which reaction of ammonia forms the first step of Ostwald's process.

Catalytic oxidation of ammonia to nitric oxide and water is the first step of Ostwald's process.4NH3+5O2→700−800°CPt4NO+6H2O+21.5K cals4\text{NH}_3 + 5\text{O}_2 \xrightarrow[700-800 \degree\text{C}]{\text{Pt}} \text{4NO} + \text{6H}_\text{2}\text{O} + 21.5 \text{K cals}4NH3+5O2Pt700−800°C4NO+6H2O+21.5K cals

Q: Question 7Convert ammonia to nitric acid by Ostwald's process giving all conditions.

Step I : 4NH3+5O2→700−800°CPt4NO+6H2O+21.5K cals4\text{NH}_3 + 5\text{O}_2 \xrightarrow[700-800 \degree\text{C}]{\text{Pt}} \text{4NO} + \text{6H}_\text{2}\text{O} + 21.5 \text{K cals}4NH3+5O2Pt700−800°C4NO+6H2O+21.5K calsStep II : 2NO+O2→50°C2NO22\text{NO} + \text{O}_2 \xrightarrow{50 \degree\text{C}} \text{2NO}_\text{2}2NO+O250°C2NO2Step III : 4NO2+2H2O+O2⟶4HNO34\text{NO}_\text{2} + 2\text{H}_\text{2}\text{O} + \text{O}_2 \longrightarrow 4\text{HNO}_34NO2+2H2O+O2⟶4HNO3

Q: Question 12State the cation responsible for turning moist neutral litmus red on reaction with dil. HNO3.

The high concentration of H+ ions imparts acidic nature to dilute Nitric Acid (HNO3), hence it turns moist neutral litmus red.HNO3 + H2O ⇌ H3O1+ + NO31-HNO3⇌H2OH1++NO31−\text{HNO}_3 \xrightleftharpoons {\text{H}_2\text{O}} \text{H}^{1+} + \text{NO}_3^{1-}HNO3H2OH1++NO31−H+ + H2O ⇌ H3O1+

Q: Question 19State your observation when:(i) nitric acid is added to saw dust(ii) conc. nitric acid is heated (a) in absence of copper (b) in presence of copper.

(i) Saw dust bursts into flames when hot conc. nitric acid is poured on it. The reason is that Nitric acid is a strong oxidising agent. It decomposes to give nascent oxygen which oxidises organic compounds to carbon dioxide and water.Saw dust [C6H10O5]n + Nitric acid [hot conc.] ⟶ carbon dioxide + water + nitrogen dioxide.(ii) (a) When conc. nitric acid is heated in absence of copper, reddish brown fumes of nitrogen dioxide are evolved.4HNO3→Δ4NO2+2H2O+O24\text{HNO}_3 \xrightarrow{\Delta} \text{4NO}_2 + \text{2H}_\text{2}\text{O} + \text{O}_24HNO3Δ4NO2+2H2O+O2(ii) (b) Cu reacts with conc. nitric acid liberating reddish brown fumes of nitrogen dioxide along with blue coloured solution of copper nitrate.Cu + 4HNO3 [conc.] ⟶ Cu(NO3)2 + 2H2O + 2NO2

Q: Question 21Name three chemical products manufactured from nitric acid. Give two general uses of HNO3.

Three chemical products manufactured from nitric acid are:Tri-nitro toluene [C7H5(NO2)3]Tri-nitro cellulose [C6H7O2(NO2)3]nTri-nitro glycerine [C3H5O3(NO2)3]Two general uses of nitric acid are:For etching designs on copper and brasswareIn purification of gold.

Q: Question 15Assertion (A): KNO3 and conc. H2SO4 are the reactants for the preparation of nitric acid.Reason (R): Conc. H2SO4 being a non volatile acid is required to prepare volatile acids.Both A and R are true and R is the correct explanation of A.Both A and R are true but R is not the correct explanation of A.A is true but R is false.A is false but R is true.

Both A and R are true and R is the correct explanation of A.Explanation— In the laboratory preparation of Nitric acid, nitric acid is obtained by distilling the reactants, conc. sulphuric acid (H2SO4) and potassium nitrate (KNO3). Hence, the assertion (A) is true.Sulphuric acid is a non-volatile acid and produces volatile nitric acid on reacting with potassium nitrate or sodium nitrate. Hence, the reason (R) is true.Reason (R) explains why conc. sulphuric acid (H2SO4) and potassium nitrate (KNO3) are used as reactants for the preparation of nitric acid. Hence, reason (R) is a correct explanation of assertion (A).

Question 1

Question 2Give a word equation and balanced molecular equation for the laboratory preparation of nitric acid from :(i) KNO3(ii) NaNO3.

Accepted Answer

(i) Potassium Nitrate [Nitre] + Sulphuric acid [conc.] ⟶ Potassium bisulphate + Nitric acid [vapours]KNO3[conc.]+H2SO4[conc.]→<200°CKHSO4+HNO3	ext{KNO}_3 [	ext{conc.}] + 	ext{H}_2	ext{SO}_4 [	ext{conc.}]\xrightarrow{\lt 200 \degree	ext{C}} 	ext{KHSO}_	ext{4} + 	ext{HNO}_	ext{3}KNO3​[conc.]+H2​SO4​[conc.]<200°C​KHSO4​+HNO3​(ii) Sodium Nitrate [Chile salt petre]+ Sulphuric acid [conc.] ⟶ Sodium bisulphate + Nitric acid [vapours]NaNO3[conc.]+H2SO4[conc.]→<200°CNaHSO4+HNO3	ext{NaNO}_3 [	ext{conc.}] + 	ext{H}_2	ext{SO}_4 [	ext{conc.}]\xrightarrow{\lt 200 \degree	ext{C}} 	ext{NaHSO}_	ext{4} + 	ext{HNO}_	ext{3}NaNO3​[conc.]+H2​SO4​[conc.]<200°C​NaHSO4​+HNO3​

Question 2

Question 6State which reaction of ammonia forms the first step of Ostwald's process.

Accepted Answer

Catalytic oxidation of ammonia to nitric oxide and water is the first step of Ostwald's process.4NH3+5O2→700−800°CPt4NO+6H2O+21.5K cals4	ext{NH}_3 + 5	ext{O}_2 \xrightarrow[700-800 \degree	ext{C}]{	ext{Pt}} 	ext{4NO} + 	ext{6H}_	ext{2}	ext{O} + 21.5 	ext{K cals}4NH3​+5O2​Pt700−800°C​4NO+6H2​O+21.5K cals

Question 3

Question 7Convert ammonia to nitric acid by Ostwald's process giving all conditions.

Accepted Answer

Step I : 4NH3+5O2→700−800°CPt4NO+6H2O+21.5K cals4	ext{NH}_3 + 5	ext{O}_2 \xrightarrow[700-800 \degree	ext{C}]{	ext{Pt}} 	ext{4NO} + 	ext{6H}_	ext{2}	ext{O} + 21.5 	ext{K cals}4NH3​+5O2​Pt700−800°C​4NO+6H2​O+21.5K calsStep II : 2NO+O2→50°C2NO22	ext{NO} + 	ext{O}_2 \xrightarrow{50 \degree	ext{C}} 	ext{2NO}_	ext{2}2NO+O2​50°C​2NO2​Step III : 4NO2+2H2O+O2⟶4HNO34	ext{NO}_	ext{2} + 2	ext{H}_	ext{2}	ext{O} + 	ext{O}_2 \longrightarrow 4	ext{HNO}_34NO2​+2H2​O+O2​⟶4HNO3​

Question 4

Question 12State the cation responsible for turning moist neutral litmus red on reaction with dil. HNO3.

Accepted Answer

The high concentration of H+ ions imparts acidic nature to dilute Nitric Acid (HNO3), hence it turns moist neutral litmus red.HNO3 + H2O ⇌ H3O1+ + NO31-HNO3⇌H2OH1++NO31−	ext{HNO}_3 \xrightleftharpoons {	ext{H}_2	ext{O}} 	ext{H}^{1+} + 	ext{NO}_3^{1-}HNO3​H2​O​H1++NO31−​H+ + H2O ⇌ H3O1+

Question 5

Question 19State your observation when:(i) nitric acid is added to saw dust(ii) conc. nitric acid is heated (a) in absence of copper (b) in presence of copper.

Accepted Answer

(i) Saw dust bursts into flames when hot conc. nitric acid is poured on it. The reason is that Nitric acid is a strong oxidising agent. It decomposes to give nascent oxygen which oxidises organic compounds to carbon dioxide and water.Saw dust [C6H10O5]n + Nitric acid [hot conc.] ⟶ carbon dioxide + water + nitrogen dioxide.(ii) (a) When conc. nitric acid is heated in absence of copper, reddish brown fumes of nitrogen dioxide are evolved.4HNO3→Δ4NO2+2H2O+O24	ext{HNO}_3 \xrightarrow{\Delta} 	ext{4NO}_2 + 	ext{2H}_	ext{2}	ext{O} + 	ext{O}_24HNO3​Δ​4NO2​+2H2​O+O2​(ii) (b) Cu reacts with conc. nitric acid liberating reddish brown fumes of nitrogen dioxide along with blue coloured solution of copper nitrate.Cu + 4HNO3 [conc.] ⟶ Cu(NO3)2 + 2H2O + 2NO2

Question 6

Question 21Name three chemical products manufactured from nitric acid. Give two general uses of HNO3.

Accepted Answer

Three chemical products manufactured from nitric acid are:Tri-nitro toluene [C7H5(NO2)3]Tri-nitro cellulose [C6H7O2(NO2)3]nTri-nitro glycerine [C3H5O3(NO2)3]Two general uses of nitric acid are:For etching designs on copper and brasswareIn purification of gold.

Question 7

Question 1Preparation of nitric acidNitric acidComplete and balance the equationsLaboratory preparation from nitrates 1. Potassium nitrate [nitre]KNO3+H2SO4[conc.]→<200°C...............+............... ext{KNO}_3 + ext{H}_2 ext{SO}_4 [ ext{conc.}]\xrightarrow{\lt 200 \degree ext{C}} ............... + ...............KNO3+H2SO4[conc.]<200°C...............+...............2. Sodium nitrate [chile salt petre]NaNO3+H2SO4[conc.]→<200°C...............+............... ext{NaNO}_3 + ext{H}_2 ext{SO}_4 [ ext{conc.}]\xrightarrow{\lt 200 \degree ext{C}} ............... + ...............NaNO3+H2SO4[conc.]<200°C...............+...............[NaNO3+NaHSO4[conc.]→>200°C...............+...............][ ext{NaNO}_3 + ext{NaHSO}_4 [ ext{conc.}]\xrightarrow{\gt 200 \degree ext{C}} ............... + ...............][NaNO3+NaHSO4[conc.]>200°C...............+...............]Atmospheric nitrogen to nitric acid 3. Nitrogen to nitric oxideN2 + ............... ⟶ ...............4. Nitric oxide to nitrogen dioxide............... + ............... ⟶ NO25. Nitrogen dioxide to nitric acid[Nitric acid to soluble nitrates]NO2 + ............... + ............... ⟶ HNO3[HNO3 + ............... ⟶ Ca(NO3)2 + ............... + ...............]Manufacture of nitric acid Ostwald's process 6. Step 1 [Catalytic chamber]NH3+O2→700−800°CPt...............+............... ext{NH}_3 + ext{O}_2 \xrightarrow[700-800 \degree ext{C}]{ ext{Pt}} ............... + ...............NH3+O2Pt700−800°C...............+...............7. Step 2 [Oxidation chamber]NO+O2→50°C............... ext{NO} + ext{O}_2 \xrightarrow{50 \degree ext{C}} ...............NO+O250°C...............8. Step 3 [Absorption tower]NO2 + H2O + O2 ⟶ ...............

Accepted Answer

Nitric acidComplete and balance the equationsPreparation of nitric acid Laboratory preparation from nitrates 1. Potassium nitrate [nitre]KNO3+H2SO4[conc.]→<200°CKHSO4+HNO3 ext{KNO}_3 + ext{H}_2 ext{SO}_4 [ ext{conc.}]\xrightarrow{\lt 200 \degree ext{C}} \bold{KHSO}_\bold{4} + \bold{HNO}_\bold{3}KNO3+H2SO4[conc.]<200°CKHSO4+HNO32. Sodium nitrate [chile salt petre]NaNO3+H2SO4[conc.]→<200°CNaHSO4+HNO3 ext{NaNO}_3 + ext{H}_2 ext{SO}_4 [ ext{conc.}]\xrightarrow{\lt 200 \degree ext{C}} \bold{NaHSO}_\bold{4} + \bold{HNO}_\bold{3}NaNO3+H2SO4[conc.]<200°CNaHSO4+HNO3NaNO3+NaHSO4[conc.]→>200°CNa2SO4+HNO3 ext{NaNO}_3 + ext{NaHSO}_4 [ ext{conc.}]\xrightarrow{\gt 200 \degree ext{C}} \bold{Na}_\bold{2}\bold{SO}_\bold{4} + \bold{HNO}_\bold{3}NaNO3+NaHSO4[conc.]>200°CNa2SO4+HNO3Atmospheric nitrogen to nitric acid 3. Nitrogen to nitric oxideN2+O2→dischargelightning2NO ext{N}_2 + \bold{O}_\bold{2} \xrightarrow[ ext{discharge}]{ ext{lightning}} \bold{2NO}N2+O2lightningdischarge2NO4. Nitric oxide to nitrogen dioxide2NO + O2 ⟶ 2NO25. Nitrogen dioxide to nitric acid[Nitric acid to soluble nitrates]4NO2 + 2H2O + O2 ⟶ 4HNO3[2HNO3 + CaCO3 ⟶ Ca(NO3)2 + H2O + CO2]Manufacture of nitric acid Ostwald's process 6. Step 1 [Catalytic chamber]4NH3+5O2→700−800°CPt4NO+6H2O4 ext{NH}_3 + 5 ext{O}_2 \xrightarrow[700-800 \degree ext{C}]{ ext{Pt}} \bold{4NO} + \bold{6H}_\bold{2}\bold{O}4NH3+5O2Pt700−800°C4NO+6H2O7. Step 2 [Oxidation chamber]2NO+O2→50°C2NO22 ext{NO} + ext{O}_2 \xrightarrow{50 \degree ext{C}} \bold{2NO}_\bold{2}2NO+O250°C2NO28. Step 3 [Absorption tower]4NO2 + 2H2O + O2 ⟶ 4HNO3

Question 8

Question 3Tests for nitric acidNitric acidComplete and balance the equations32. Heat on nitric acidHNO3 ⟶ H2O + ............... [g]+ ............... [g][reddish brown fumes evolved]33. Heat on copper and conc. HNO3Cu + HNO3 ⟶ ............... + ............... + ............... [g][dense reddish brown fumes evolved - blue solution remains]34. Brown ring testFeSO4 + H2SO4 + ............... ⟶ ............... + ............... + NO[FeSO4 + NO ⟶ ...............][A brown ring of nitroso ferrous sulphate is formed at the junction of the two liquids]

Accepted Answer

Nitric acidComplete and balance the equations32. Heat on nitric acid4HNO3→Δ2H2O+4NO2[g]+O2[g]4	ext{HNO}_3 \xrightarrow{\Delta} 2	ext{H}_2	ext{O} + \bold{4NO}_\bold{2}[g] + \bold{O}_\bold{2} [g]4HNO3​Δ​2H2​O+4NO2​[g]+O2​[g][reddish brown fumes evolved]33. Heat on copper and conc. HNO3Cu+4HNO3→ΔCu(NO3)2+2H2O+2NO2[g]	ext{Cu} + 4	ext{HNO}_3 \xrightarrow{\Delta} \bold{Cu(NO}_3)_2 + \bold{2H}_2\bold{O} + \bold{2NO}_2[g]Cu+4HNO3​Δ​Cu(NO3​)2​+2H2​O+2NO2​[g][dense reddish brown fumes evolved - blue solution remains]34. Brown ring test6FeSO4 + 3H2SO4 + 2HNO3 ⟶ 3Fe2(SO4)3 + 4H2O +2NO[FeSO4 + NO ⟶ FeSO4.NO][A brown ring of nitroso ferrous sulphate is formed at the junction of the two liquids]

Question 9

Question 4In the laboratory preparation of nitric acid, nitre is heated with :conc. HClconc. H2SO4dil. H2SO4conc. H3PO4

Accepted Answer

conc. H2SO4Reason — In the laboratory preparation of Nitric acid by distillation process, potassium nitrate (nitre) is heated with conc. sulphuric acid (H2SO4).KNO3[conc.]+H2SO4[conc.]→<200°CKHSO4[acid salt]+HNO3\underset{[	ext{conc.}]}{	ext{KNO}_3} + \underset{[	ext{conc.}]}{	ext{H}_2	ext{SO}_4} \xrightarrow{\lt 200 \degree	ext{C}} \underset{[	ext{acid salt}]}{	ext{KHSO}_4} + 	ext{HNO}_3[conc.]KNO3​​+[conc.]H2​SO4​​<200°C​[acid salt]KHSO4​​+HNO3​

Question 10

Question 15Assertion (A): KNO3 and conc. H2SO4 are the reactants for the preparation of nitric acid.Reason (R): Conc. H2SO4 being a non volatile acid is required to prepare volatile acids.Both A and R are true and R is the correct explanation of A.Both A and R are true but R is not the correct explanation of A.A is true but R is false.A is false but R is true.

Accepted Answer

Both A and R are true and R is the correct explanation of A.Explanation— In the laboratory preparation of Nitric acid, nitric acid is obtained by distilling the reactants, conc. sulphuric acid (H2SO4) and potassium nitrate (KNO3). Hence, the assertion (A) is true.Sulphuric acid is a non-volatile acid and produces volatile nitric acid on reacting with potassium nitrate or sodium nitrate. Hence, the reason (R) is true.Reason (R) explains why conc. sulphuric acid (H2SO4) and potassium nitrate (KNO3) are used as reactants for the preparation of nitric acid. Hence, reason (R) is a correct explanation of assertion (A).

Question 11

Question 18Assertion (A): The yellow colour of nitric acid is removed by using carbon dioxide gas or dry air.Reason (R): Carbon dioxide gas or dry air drives away NO2 gas from the warm nitric acid.Both A and R are true and R is the correct explanation of A.Both A and R are true but R is not the correct explanation of A.A is true but R is false.A is false but R is true.

Accepted Answer

Both A and R are true and R is the correct explanation of A.Explanation — The yellow colour of nitric acid is removed by bubbling carbon dioxide gas or dry air into it. Hence, the assertion (A) is true.The yellow colour will disappear because carbon dioxide gas or dry air drive out NO2 gas from the warm nitric acid. Hence, the reason (R) is true.Reason (R) explains how the use of carbon dioxide and dry air turn yellow colour nitric acid into a colourless compound. Hence, reason (R) is a correct explanation of assertion (A).

Question 12

Question 20Assertion (A): Cold and dilute nitric acid oxidise metals to their nitrates and nitric oxide.Reason (R): Hot and concentrated nitric acid liberates nitrogen dioxide.Both A and R are true and R is the correct explanation of A.Both A and R are true but R is not the correct explanation of A.A is true but R is false.A is false but R is true.

Accepted Answer

Both A and R are true but R is not the correct explanation of A.Explanation — Cold and dilute nitric acid oxidises metals to their nitrates and nitric oxide. Hence, the assertion (A) is true.3Cu + 8HNO3 ⟶ 3Cu(NO3)2 + 4H2O + 2NOHot dilute nitric acid or concentrated nitric acid liberates nitrogen dioxide. Hence, the reason (R) is true.Cu + 4HNO3 ⟶ Cu(NO3)2 + 2H2O + 2NO2However, reason (R) doesn't explain the action of Cold and dilute nitric acid on metals. So, it is not the correct explanation of assertion (A).

Question 13

Question 5Give balanced equation for the following :(a) dilute nitric acid and copper carbonate.(b) oxidation of carbon with conc. HNO3.(c) Laboratory preparation of nitric acid.(d) Action of heat on a mixture of copper and concentrated nitric acid.

Accepted Answer

(a) CuCO3 + 2HNO3 [dil.] ⟶ Cu(NO3)2 + H2O + CO2(b) C + 4HNO3 ⟶ CO2 + 2H2O + 4NO2(c) Balanced equation for laboratory preparation of nitric acid:KNO3[conc.]+H2SO4[conc.]→<200°CKHSO4[acid salt]+HNO3\underset{[	ext{conc.}]}{	ext{KNO}_3} + \underset{[	ext{conc.}]}{	ext{H}_2	ext{SO}_4} \xrightarrow{\lt 200 \degree	ext{C}} \underset{[	ext{acid salt}]}{	ext{KHSO}_4} + 	ext{HNO}_3[conc.]KNO3​​+[conc.]H2​SO4​​<200°C​[acid salt]KHSO4​​+HNO3​(d) Balanced equation for action of heat on a mixture of copper and concentrated nitric acid:Cu+4HNO3[conc.]⟶Cu(NO3)2+2H2O+2NO2	ext{Cu} + 4\underset{[	ext{conc.}]}{	ext{HNO}_3} \longrightarrow 	ext{Cu(NO}_3 	ext{)}_2 + 2	ext{H}_2 	ext{O} + 2	ext{NO}_2Cu+4[conc.]HNO3​​⟶Cu(NO3​)2​+2H2​O+2NO2​

Question 14

Question 5cConc. nitric acid prepared in the laboratory is yellow in colour. Why? How is this colour removed?

Accepted Answer

Concentrated nitric acid prepared in the laboratory is yellow in color due to dissolution of reddish brown nitrogen dioxide gas in the acid. This gas is produced due to the thermal decomposition of a portion of nitric acid.4HNO3 ⟶ 2H2O + 4NO2 + O2The yellow color of the acid is removed :If dry air or CO2 is bubbled through the yellow acid, the latter turns colourless because it drives out NO2 gas from warm acid, which is further oxidised to nitric acid.By adding excess water, nitrogen dioxide gas dissolves in water and thus yellow color of acid is removed.

Question 15

Question 5dGive reasons for the following:In the laboratory preparation of nitric acid, the mixture of concentrated sulphuric acid and sodium nitrate should not be heated very strongly above 200°C.

Accepted Answer

The temperature of the reaction should not increase above 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, although the yield of nitric acid is higher.2NaNO3 + H2SO4 →>200°C\xrightarrow{\gt 200 \degree	ext{C}}>200°C​ Na2SO4 + 2HNO3The higher temperaturemay damage the glass apparatus.decomposition of nitric acid can also occur.wastage of fuel.

Question 16

Question 6(a) Nitric acid cannot be concentrated beyond 68% by the distillation of a dilute solution of HNO3. State the reason.(b) What is passive iron? How is passivity removed?

Accepted Answer

(a) An aqueous solution of nitric acid (68% concentration) forms a constant boiling mixture at 121°C. A constant boiling mixture is one which boils without change in composition.Hence on boiling further, the mixture evolves out the vapours of both acid and water in the same proportion as in the liquid.Therefore, dilute HNO3 cannot be concentrated beyond 68% by boiling.(b) Iron becomes passive or inert when treated with pure concentrated nitric acid due to the formation of the extremely thin layer of insoluble iron oxide (passivity) which stops the reaction.Fe + 6HNO3 ⟶ Fe(NO3)3 + 3H2O + 3NO2This inert iron is known as passive iron.Passivity can be removed by rubbing the surface layer with sandpaper or by treating with strong reducing agent.

Question 17

Question 8Give two chemical equations for each of the following:(a) Reactions of nitric acid with non-metals.(b) Nitric acid showing as acidic character.(c) Nitric acid acting as oxidising agent.

Accepted Answer

(a) Action on non-metals:C + 4HNO3 ⟶ CO2 + 2H2O + 4NO2S + 6HNO3 ⟶ H2SO4 + 2H2O + 6NO2(b) Reaction with alkalis:K2O + 2HNO3 ⟶ 2KNO3 + H2OCuO + 2HNO3 ⟶ Cu(NO3)2 + H2O(c) Nitric acid acting as oxidising agent:C + 4HNO3 ⟶ CO2 + 2H2O + 4NO23Cu + 8HNO3 [cold and dil.] ⟶ 3Cu(NO3)2 + 4H2O + 2NO

Question 18

Question 9Write balanced equations and name the products formed when:(a) Sodium hydrogen carbonate is added to nitric acid.(b) Cupric oxide reacts with nitric acid(c) Zinc reacts with dilute nitric acid(d) Concentrated nitric acid is heated

Accepted Answer

(a) Sodium hydrogen carbonate when treated with nitric acid forms sodium nitrate, carbon dioxide and water.NaHCO3 + HNO3 ⟶ NaNO3 + H2O + CO2 ↑(b) Cupric oxide reacts with dilute nitric acid, it forms copper nitrate and water.CuO + 2HNO3 ⟶ Cu(NO3)2 + H2O(c) Zinc reacts with dil. nitric acid to form zinc nitrate, nitric oxide and water3Zn + 8HNO3 ⟶ 3Zn(NO3)2 + 4H2O + 2NO(d) When concentrated nitric acid is heated it forms nitrogen dioxide gas, water and oxygen gas4HNO3 →Δ\xrightarrow{\Delta}Δ​ 4NO2 + 2H2O + O2

Question 19

Question 11Write equation for the following conversions A, B, C and D.

Accepted Answer

A : 3Cu + 8HNO3 [cold and dil.] ⟶ 3Cu(NO3)2 + 4H2O + 2NOB : 2Cu(NO3)2 →Δ\xrightarrow{\Delta}Δ​ 2CuO + 4NO2 + O2C : 2Cu + O2 ⟶ 2CuOD : CuO + H2 →Δ\xrightarrow{\Delta}Δ​ Cu + H2O

Question 20

Question 12Correct the following, if required:(a) HNO3 is a strong reducing agent.(b) NaNO3 gives NO2 and O2 on heating.(c) Constant boiling nitric acid contains 80% nitric acid by weight.(d) Nitric acid remains colourless even when exposed to light.(e) Magnesium reacts with nitric acid to liberate hydrogen gas.

Accepted Answer

(a) HNO3 is a strong oxidizing agent(b) NaNO3 gives NaNO2 and O2 on heating.(c) Constant boiling nitric acid contains 68% nitric acid by weight(d) Nitric acid turns yellow when exposed to light.(e) Magnesium reacts with very dilute (about 1%) nitric acid to liberate hydrogen gas.

Study of Compounds — Nitric Acid

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