Worksheet: Uses of Ammonia

In this worksheet, we will practice describing the uses of ammonia, balancing reaction equations, and calculating the quantities of ammonia involved.

Q1:

Bleach, an aqueous solution of sodium hypochlorite (NaClO), is often used alongside ammonia as a cleaning agent. However, it is important that bleach and ammonia are never mixed, as the compounds react to form chloramine (NHCl)2.

Give a balanced chemical equation for this reaction.

  • ANH+2NaClONHCl+2NaCl+O322
  • B2NH+2NaClO2NHCl+NaO+HO3222
  • CNH+NaClONHCl+NaO32
  • DNH+NaClONHCl+NaOH32
  • ENH+3NaClONHCl+3NaOH+Cl322

What is the main hazard associated with the reaction of bleach and ammonia?

  • AChloramine is a toxic gas.
  • BA highly corrosive solution is produced.
  • CThe reaction is highly exothermic.
  • DChloramine is an explosive gas.
  • EChloramine is a corrosive gas.

Q2:

What is the main hazard associated with aqueous ammonia solutions?

  • AOxidizing
  • BToxic
  • CIrritant
  • DFlammable
  • ECorrosive

Q3:

Ammonia and carbon dioxide are both gaseous at room temperature and pressure. The pure materials are widely used and share a large number of industrial applications. The compounds can form aqueous solutions and react together in water to produce a solid material.

In which of the following ways are molecules of ammonia and carbon dioxide similar?

  • ABoth molecules are polar.
  • BBoth molecules are heavier than the average molecule in air.
  • CThe molecules have the same shape.
  • DThe molecules contain the same number of bonding electrons.
  • EBoth molecules react with water.

Which of the following is not an application for which pure ammonia and pure carbon dioxide are both directly useful?

  • AFuel
  • BBiomaterial production
  • CSolvent
  • DRefrigeration
  • EFertilizer manufacture

What is the name of the solid material formed when excess ammonia and carbon dioxide react in water?

  • AAmmonium hydrogen carbonate
  • BAmmonium carbonate
  • CAmmonium carboxylate
  • DAmmonium carbamate
  • EAmmonium carbide

Write a balanced chemical equation for the reaction of excess ammonia with carbon dioxide in water.

  • ANH+CONHCO3232
  • B2NH+2CO+2HO2NHCO+H322432
  • CNH+CO+HO(NH)HCO32243
  • D2NH+CO(NH)CO+HO32222
  • ENH+CO+HO(NH)CO322423

Q4:

Why is the electrical conductivity of a dilute aqueous ammonia solution higher than that of pure water?

  • AAmmonia reacts with water to produce hydroxide and ammonium ions.
  • BAmmonia molecules are smaller than water molecules, so they diffuse more rapidly.
  • CAmmonia reacts with water to produce amide and hydronium ions.
  • DAmmonia is more polar than water, so it responds more strongly to an electric field.
  • EAmmonia molecules interact more weakly than water molecules, so they diffuse more rapidly.

Q5:

Ammonia reacts with nitric acid to produce a solid compound X, which is used as a fertilizer.

What is the name of compound X?

  • ANitrosamine
  • BAmmonium nitrate
  • CAmmonium nitrite
  • DNitrylamine
  • EAmyl nitrate

Give a balanced chemical equation for this reaction.

  • ANH+HNONHNO34
  • BNH+HNONHNO3343
  • CNH+HNO(NH)NO322422
  • D2NH+HNO(NH)NO323423
  • ENH+HNONHNO3242

What color is the solid X?

  • ABrown
  • BRed
  • CBlack
  • DYellow
  • EWhite

When heated, compound X decomposes into nitrous oxide (NO2) and one other product. Give a balanced chemical equation for this reaction.

  • ANHNONO+2H422
  • BNHNONO+2HO4322
  • CNHNONO+2HO4222
  • D2(NH)NO3NO+8H42322
  • E2(NH)NO3NO+HO42222

Q6:

Ammonia can react with oxygen to form nitrogen dioxide (NO)2, nitric oxide (NO), and nitrous oxide (NO)2. Nitrogen dioxide is useful for the manufacture of nitric acid.

In the presence of a platinum-rhodium catalyst, ammonia reacts with oxygen to produce nitric oxide and water. Give a balanced chemical equation for this reaction.

  • A5NH+6O5NO+7HO322
  • B4NH+5O4NO+6HO322
  • C3NH+2O3NO+3HO322
  • D6NH+7O6NO+9HO322
  • E2NH+3O2NO+3HO322

In the presence of a catalyst containing manganese dioxide, ammonia reacts with oxygen to produce nitrous oxide and water. Give a balanced chemical equation for this reaction.

  • A3NH+4O3NO+5HO3222
  • B2NH+ONO+HO3222
  • C3NH+3O2NO+4HO3222
  • D2NH+2ONO+3HO3222
  • E4NH+3O2NO+4HO3222

Nitric oxide and nitrous oxide can react with further oxygen to form nitrogen dioxide. Calculate the mass of oxygen required to produce 60.0 g of nitrogen dioxide from ammonia.

Q7:

Ammonia is useful for the production of nylon 6,6, a polymer with the empirical formula CHNO.611 If all the nitrogen atoms in nylon 6,6 are derived from ammonia, calculate the mass of ammonia needed to produce 139 g of the polymer.

Q8:

Which property of ammonia is the most important for industrial purposes?

  • AEnergy content
  • BNitrogen content
  • CToxicity
  • DBasicity
  • ELow boiling point

Q9:

Inexpensive large-scale manufacture of ammonia began in the early 20th century. By the year 2000, the global annual production of ammonia was approximately 110 million metric tons.

Which industry produces the greatest demand for synthetically manufactured ammonia?

  • AEnergy
  • BPharmaceutical
  • CMilitary
  • DAgriculture
  • ECleaning

The majority of synthetically manufactured ammonia is used in the production of a single type of product. To the nearest 10%, what percentage of the global annual production of ammonia was consumed for this purpose in the year 2000?

Q10:

Excess nitrogen is excreted by fish in the form of ammonia. By contrast, humans and most other mammals excrete nitrogen mainly as urea, CHNO42.

What property of ammonia makes it suitable for excretion by fish?

  • ALow boiling point
  • BHigh basicity
  • CHigh solubility
  • DSmall molecular size
  • ELow toxicity

What property of ammonia necessitates its conversion to urea before it is excreted by humans?

  • AHigh toxicity
  • BLow solubility
  • CSmall molecular size
  • DHigh acidity
  • ELow boiling point

Q11:

The reaction of lithium metal with liquid ammonia is similar to its reaction with water. Give a balanced chemical equation for this reaction.

  • A2Li+2NH2LiNH+H322
  • BLi+2NHLi(NH)332
  • C4Li+2NH2LiNH+H3222
  • DLi+2NHLi(NH)+H3222
  • ELi+NHLiNH33

Q12:

Which of the following organic molecules would react with ammonia most readily?

  • AEthene
  • BEthanol
  • CEthane
  • DEthyl acetate
  • EEthanoic acid

Q13:

Ammonia reacts with hydrogen chloride to produce a solid compound X.

What is the name of compound X?

  • ANitrogen hydrochloride
  • BAmmonium hydrochloride
  • CAmmonium chloride
  • DHydrochloramine
  • ENitrogen trichloride

Give a balanced chemical equation for this reaction.

  • A2NH+2HCl2NHCl+H332
  • B2NH+4HCl2NHCl+H3422
  • C4NH+4HCl2(NH)Cl+Cl3422
  • DNH+HClNHCl34
  • ENH+2HClNHCl352

Why is the melting point of X higher than that of ammonia, which is a gas at room temperature?

  • AIonic bonds in the product are stronger than the hydrogen bonds in ammonia.
  • BHydrogen bonds in the product are stronger than the ionic bonds in ammonia.
  • CHydrogen bonds in the product are stronger than the covalent bonds in ammonia.
  • DCovalent bonds in the product are stronger than the covalent bonds in ammonia.
  • EIonic bonds in the product are stronger than the covalent bonds in ammonia.

Q14:

Ammonia reacts with oxygen to form nitric acid and one other product.

Give a balanced chemical equation for this reaction.

  • A2NH+4O2HNO+HO322322
  • B2NH+2O2HNO+H32222
  • CNH+OHNO+HO322
  • DNH+2OHNO+HO3232
  • ENH+OHNO+H3222

Calculate the mass of nitric acid formed when 20.0 kg of ammonia reacts with excess oxygen.

Calculate the mass of oxygen needed to produce 50.5 metric tons of nitric acid from ammonia.

A 12.3 kg sample of ammonia reacts with 41.5 kg of oxygen to form 35.0 kg of nitric acid. By identifying the limiting reagent and determining the maximum mass of nitric acid that can be produced, calculate the percentage yield of this reaction.

Q15:

In the presence of a catalyst, ammonia reacts with oxygen to form nitrogen gas and one other product.

Give a balanced chemical equation for this reaction.

  • A2NH+ON+3HO3222
  • B2NH+3ON+6OH322
  • C2NH+3ON+3HO32222
  • D4NH+3O2N+6HO3222
  • E4NH+3O2N+6HO32222

A sample of ammonia reacts with excess oxygen to produce 24.0 g of nitrogen gas. Calculate the mass of ammonia reacted.

A sample of ammonia requires 36.5 kg of oxygen for complete combustion. Calculate the mass of nitrogen gas produced.

Q16:

What is the most common method used to manufacture ammonia?

  • AElectrolysis
  • BSteam refining
  • CHaber process
  • DWater-gas shift reaction
  • EContact process

Q17:

A student prepares a dilute solution of ammonia in water and tests the pH using a universal indicator.

What color does the universal indicator change into?

  • AYellow
  • BRed
  • CGreen
  • DBlue
  • EPurple

Give a balanced chemical equation for the main reaction responsible for the change in pH when ammonia is dissolved in water.

  • A2NHNH+NH34+2
  • BNH+HONH+HO3223+
  • CNH+HONHOH+H3222
  • D2NH+2HO2NHOH+H3232
  • ENH+HONH+OH324+

Q18:

Ammonia can be used in the production of fertilizers. Which biomolecules in plants are produced directly from ammonia in the largest quantities?

  • AProteins
  • BSterols
  • CLipids
  • DDNA
  • ESugars

Q19:

The rocket propellants hydrogen peroxide (HO)22 and hydrazine (NH)24 both contain single covalent bonds between atoms of the same element:

OOHHNNHHHH

Ammonia reacts with hydrogen peroxide to form hydrazine and one other product. The bond energies of selected bonds are shown in the table.

BondHHOHOOOONHNNNNNN
Bond Energy kJ/mol432459142494386167418942

Give a balanced chemical equation for the formation of hydrazine from ammonia and hydrogen peroxide.

  • A2NH+HONH+3HO322242
  • B2NH+2HONH+3HO322242
  • C2NH+HONH+2HO322242
  • D2NH+HONH+2H+O3222422
  • E2NH+2HONH+3H+2O3222422

What is the energy released by the reaction of ammonia and hydrogen peroxide per mole of hydrazine produced?

When used as a rocket propellant, hydrazine thermally decomposes into its constituent elements in their standard state. Calculate the energy released per mole of hydrazine reacted.

Whereas hydrazine thermally decomposes into its constituent elements, hydrogen peroxide converts to steam and oxygen when heated. The compounds are useful as rocket propellants because their decomposition reactions increase the temperature of the surroundings, 𝑇, and the number of gas molecules in the system, 𝑁. Compare the changes in 𝑇 and 𝑁 when a mole of each compound thermally decomposes.

  • AHydrazine produces a smaller increase in 𝑇 and a larger increase in 𝑁.
  • BHydrazine produces a larger increase in 𝑇 and the same increase in 𝑁.
  • CHydrazine produces a larger increase in both 𝑇 and 𝑁.
  • DHydrazine produces a smaller increase in 𝑇 and the same increase in 𝑁.
  • EHydrazine produces a larger increase in 𝑇 and a smaller increase in 𝑁.

Q20:

Which of the following symbols does not represent a hazard of pressurized ammonia gas?

  • A
  • B
  • C
  • D
  • E

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