Chemical properties of ammonia. Complete and balance the equations. Combustibility. Burning of ammonia in oxygen NH3 + O2 ⟶ ............... + ...............

As a reducing agent [ammonia gas]. Complete and balance the equations. Heated copper oxide CuO + NH3 ⟶ ............... + H2O + ............... [g]

From NH3, HCl, H2S, SO2 - Select : (i) The gas which when bubbled through CuSO4 soln., a deep blue coloured soln. is formed. (ii) This gas burns in oxygen with a green flame.

Write the equation for the reaction in the Haber's process that forms ammonia.

State the purpose of liquefying the ammonia produced in the Haber's process.

Write an equation for the reaction of chlorine with excess of ammonia.

Name the ion other than ammonium ion formed when ammonia dissolves in water.

Write equations for the formation of ammonia. (i) NH4Cl and slaked lime are heated. (ii) Aluminium nitride and water.

Select from the list - Ammonia, Copper oxide, Copper sulphate, Hydrogen chloride, Hydrogen sulphide, Lead bromide : The compound which is not a metal hydroxide but it's aqueous solution is alkaline in nature.

From the substances - Ammonium sulphate, Lead carbonate, Chlorine, Copper nitrate, Iron [II] sulphate - State : A compound which on heating with NaOH produces a gas which forms dense white fumes with HCl.

Compound which on heating with NaOH produces a gas which forms dense white fumes with HCl.

State what is observed when excess of ammonia is passed through an aq. solution of lead nitrate.

Name the substance used for drying ammonia.

Write a balanced chemical equation to illustrate the reducing nature of ammonia.

With reference to Haber's process, write the equation and the conditions required.

Give an equation for formation of ammonium sulphate from ammonia and dilute sulphuric acid.

Give equation for - reaction in which NH3 is oxidized by : (i) a metal oxide (ii) a gas which is not oxygen

You enter a laboratory after a class has completed the Fountain Experiment. How will you be able to tell whether the gas used in the experiment was hydrogen chloride or ammonia.

Name : An alkaline gas 'A' which gives dense white fumes with hydrogen chloride.

Write the equation for the following reaction : Aluminium nitride and water.

Complete the table relating to an important industrial processes. [Output refers to the product of the process].

Name the gas - that burns in oxygen with a green flame.

Write a fully balanced equation for - Magnesium nitride is treated with warm water.

Identity the substances 'Q' based on the information given - The white crystalline solid 'Q' is soluble in water. It liberates a pungent smelling gas when heated with sodium hydroxide solution.

Complete the blanks (a) to (e) in the passage given, using the following words. [Ammonium, reddish brown, hydroxyl, nitrogen dioxide, ammonia, dirty green, alkaline, acidic]. In the presence of a catalyst, nitrogen and hydrogen combine to give (a) .............. gas. When the same gas is passed through water, it forms a soln. which will be (b).............. in nature, and will contain the ions (c) .............. and (d) .............. .(e) A .............. coloured ppt. of iron [II] hydroxide is formed when the above solution is added to iron [II] sulphate solution.

State your observation when - in the absence of catalyst, ammonia is burnt in an atmosphere of oxygen.

Give the equation for the reaction - ammonium chloride is heated with sodium hydroxide.

In the manufacture of ammonia: (i) Name the process. (ii) State the ratio of the reactants taken? (iii) State the catalyst used. (iv) Give the equation for the manufacture of the gas ammonia.

Write a relevant equation, to show that ammonia can act as a reducing agent

Name two gases which can be used to study the fountain experiment. State the common property demonstrated by the fountain experiment ?

State what is observed when - Ammonium hydroxide is first added in a small quantity and then in excess to a solution of copper sulphate.

The diagram shows set up for the lab. preparation of a pungent alkaline gas. (i) Name the gas collected in the jar. (ii) Give a balanced equation for the above preparation (iii) State how the above gas is collected? (iv) Name the drying agent used. (v) State how you will find out that the jar is full of the pungent gas?

Write a balanced chemical equation - Chlorine reacts with excess of ammonia.

State your observation - Water is added to the product formed, when Al is burnt in a jar of nitrogen gas.

Name the gas produced when excess ammonia reacts with chlorine.

Rewrite the correct statement with the missing word/s - Magnesium nitride reacts with water to liberate ammonia.

Give balanced equation for the reaction : Ammonia and Oxygen in the presence of a catalyst.

The following questions are based on the preparation of ammonia gas in the laboratory: (i) Explain why ammonium nitrate is not used in the preparation of ammonia. (ii) Name the compound normally used as a drying agent during the process. (iii) How is ammonia gas collected? Explain why it is not collected over water.

State one appropriate observation for : Excess of chlorine gas is reacted with ammonia gas.

Nitrogen gas can be obtained by heating : (a) Ammonium nitrate (b) Ammonium nitrite (c) Magnesium nitride (d) Ammonium chloride

State two observations for : NH4OH soln. is added to zinc nitrate soln. slowly and then in excess.

Give a balanced equation for : Reduction of hot Copper (II) oxide to copper using ammonia gas.

State the - (i) Temperature (ii) Catalyst used in the Haber's process for manufacture of ammonia. Give the equation for the catalyzed reaction.

Identify : An alkaline gas which produces dense white fumes when reacted with HCl gas.

Fill in the blank from the choices given in bracket : Ammonia gas is collected by .............. (upward displacement of air, downward displacement of water, downward displacement of air)

Write balanced equation for : Action of warm water on magnesium nitride.

Distinguish between the following pairs of compounds using the test given in bracket : (i) Iron [II] sulphate and iron [III] sulphate [using ammonium hydroxide] (ii) A lead salt and a zinc salt [using excess ammonium hydroxide]

State your observation : Calcium hydroxide is heated with ammonium chloride crystals.

Name the other ion formed when ammonia dissolves in water. Give one test that can be used to detect the presence of the ion produced.

State the conditions required for : Catalytic oxidation of ammonia to nitric oxide.

From the list of the gases - Ammonia, ethane, hydrogen chloride, hydrogen sulphide, ethyne - Select the gas which is used as a reducing agent in reducing copper oxide to copper.

State one relevant observation - Ammonia gas is burnt in an atmosphere of excess oxygen.

A metal 'X' has valency 2 and a non-metal 'Y' has a valency 3. If 'Y ' is a diatomic gas, write an equation for the direct combination of X and Y to from a compound.

Give balanced chemical equations for - (i) Lab. preparation of ammonia using an ammonium salt. (ii) Reaction of ammonia with excess chlorine. (iii) Reaction of ammonia with sulphuric acid.

Write balanced equations for : (i) Action of warm water on AlN. (ii) Excess of ammonia is treated with chlorine. (iii) An equation to illustrate the reducing nature of ammonia.

Name the gas evolved when the following mixtures are heated : (i) Calcium hydroxide and Ammonium chloride. (ii) Sodium nitrite and Ammonium chloride.

Write the balanced chemical equation for each of the following - (i) Reaction of ammonia with heated copper oxide. (ii) Laboratory preparation of ammonia from ammonium chloride.

Give a balanced chemical equation for each of the following - (i) Catalytic oxidation of ammonia. (ii) Reaction of ammonia with nitric acid.

State one observation for the following : Ammonia gas is passed over heated copper [II] oxide.

Identify the substance italicized : The catalyst used to oxidize ammonia.

Name the gas evolved when : Ammonia reacts with heated copper [II] oxide.

Study the flowchart given and give balanced equations to represent the reactions A, B and C Mg3N2→ANH3⇄CBNH4ClMg3​N2​A​NH3​BC​NH4​Cl

Copy and complete the following table which refers to the industrial method for preparation of ammonia. Name of the compound - Ammonia Name of the process - Haber's process Catalytic equation [with the catalyst] - N2+3H2⇌450-500 °CFe2NH3+ΔN2​+3H2​Fe450-500 °C​2NH3​+Δ

Write a balanced chemical equation for each of the following: (i) Reaction of excess ammonia with chlorine. (ii) Reaction of lead nitrate solution with ammonium hydroxide.

Distinguish between the following pairs of compounds using a reagent as a chemical test. Ammonium sulphate crystals and sodium sulphate crystals

Identify the substance underlined in the following sentence: The catalyst used to oxidize ammonia into nitric oxide.