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Lesson: The Haber Process

Worksheet • 16 Questions

Q1:

A sample of nitrogen is reacted with excess hydrogen to produce 2.80 tonnes of product via the Haber process. The yield of the reaction is 41.0%. Calculate the mass of the nitrogen sample.

Q2:

Illustrated in the plot is the maximum percentage yield of the Haber process at different values of the variables 𝑋 and π‘Œ .

Identify the variable 𝑋 and the units used.

  • APressure in atmospheres
  • BPressure in Pascals
  • CTemperature in kelvins
  • DTemperature in celsius
  • ECatalyst surface area in square meters per gram

Identify the variable π‘Œ .

  • ATemperature in celsius
  • BCatalyst surface area in square meters per gram
  • CTemperature in kelvins
  • DPressure in Pascals
  • EPressure in atmospheres

Q3:

The Haber process involves the reversible reaction of two gaseous reactants. What is the main disadvantage of increasing the temperature at which the reaction is performed?

  • AReduced maximum percentage yield
  • BIncreased equipment and running costs
  • CReduced reaction rate
  • DMelting of the solid catalyst
  • EIncreased formation of unwanted side products

Q4:

The Haber process involves the reversible reaction of nitrogen and hydrogen.

Give a balanced chemical equation for this reaction.

  • A N + 3 H 2 N H 2 2 3
  • B N + 2 H N H 2 2 2 4
  • C N + 2 H 2 N H 2 2 2
  • D N + 4 H 2 N H 2 2 4
  • E N + 3 H N H 2 2 2 6

Why is this reaction described as reversible?

  • ASome of the product converts back to the original reactants under the reaction conditions.
  • BThe product cannot undergo further reactions.
  • CThe product converts slowly back to the original reactants once the reaction is complete.
  • DIt is possible to use a different reaction to convert the product back to the original reactants.
  • EThe product is less stable than the reactants.

If the reaction is performed at a higher gas pressure, what happens to the reaction rate and percentage yield?

  • AThe reaction rate and percentage yield both increase.
  • BThe reaction rate increases and the percentage yield decreases.
  • CThe reaction rate and percentage yield both decrease.
  • DThe reaction rate decreases and the percentage yield increases.
  • EThe reaction rate increases and the percentage yield remains approximately constant.

If the reaction is performed at a lower temperature, what happens to the reaction rate and percentage yield?

  • AThe reaction rate decreases and the percentage yield increases.
  • BThe reaction rate increases and the percentage yield decreases.
  • CThe reaction rate and percentage yield both increase.
  • DThe reaction rate decreases and the percentage yield remains approximately constant.
  • EThe reaction rate and percentage yield both decrease.

Q5:

The nitrogen molecule has a bond energy of 945 kJ/mol and the hydrogen molecule has a bond energy of 436 kJ/mol. The reaction of nitrogen and hydrogen in the Haber process releases 46 kJ for each mole of product. Calculate the bond energy per mole of bonds in the product molecule.

Q6:

What is the main reason for removing the product from the reaction mixture during the Haber process?

  • ATo increase the reaction yield
  • BTo increase the reaction rate
  • CTo prevent the formation of unwanted side products
  • DTo prevent degradation of the catalyst
  • ETo lower the pressure of the reaction mixture

Q7:

At what temperature, in degrees Celsius, is the reaction of the Haber process typically performed?

Q8:

Which of the following changes could lower the reaction rate in the Haber process?

  • AIncreasing the flow rate over the catalyst
  • BIncreasing the mass of the catalyst
  • CReducing the size of catalyst particles
  • DIncreasing the reaction temperature
  • EIncreasing the pressure of the reaction mixture

Q9:

The Haber process is a gas-phase reaction involving hydrogen gas ( H ) 2 . A major source of hydrogen gas is the reaction of methane ( C H ) 4 with steam. This process is known as steam reforming.

Give a balanced chemical equation for the steam reforming of methane gas, which generates carbon monoxide as a gaseous by-product.

  • A C H + H O C O + 3 H 4 2 2
  • B C H + 2 H O 2 C O + 4 H 4 2 2
  • C C H + H O C O + 2 H 4 2 2
  • D C H + 2 H O C O + 8 H 4 2 2 2
  • E C H + 2 H O C O + 4 H 4 2 2 2

Steam reforming involves a reversible reaction. How do the reaction rate and percentage yield change if the pressure of the reacting gases is increased?

  • AThe reaction rate increases and the percentage yield decreases.
  • BThe reaction rate increases and the percentage yield is approximately constant.
  • CThe reaction rate decreases and the percentage yield increases.
  • DThe reaction rate and percentage yield both decrease.
  • EThe reaction rate and percentage yield both increase.

Additional hydrogen can be produced by reacting carbon monoxide from steam reforming with additional water, in a process known as the water-gas shift reaction. There is only one other product. Give a balanced chemical equation for this reaction.

  • A C O + H O C O + H 2 2 2
  • B 2 C O + 4 H O 2 H C O + 3 H 2 3 2
  • C C O + 2 H O C O + 2 H 2 3 2
  • D C O + 2 H O H C O + H 2 2 3 2
  • E C O + H O C + O + H 2 2 2

The water-gas shift reaction is reversible. How do the reaction rate and percentage yield change if the pressure of the reacting gases is increased?

  • AThe reaction rate increases and the percentage yield is approximately constant.
  • BThe reaction rate increases and the percentage yield decreases.
  • CThe reaction rate and percentage yield both decrease.
  • DThe reaction rate decreases and the percentage yield increases.
  • EThe reaction rate and percentage yield both increase.

Q10:

Which catalyst is typically used in the Haber process?

  • AIron
  • BCopper
  • CNickel
  • DVanadium
  • EPlatinum

Q11:

The reaction of 381.2 kg of nitrogen with 86.1 kg of hydrogen in the Haber process results in a yield of 75.0%. Calculate the mass of product in this reaction.

Q12:

The Haber process is a gas-phase reaction involving nitrogen gas ( N ) 2 . Pure nitrogen can be produced by reacting air with hydrogen gas and removing the products.

Besides nitrogen, what are the two most abundant components of dry air?

  • AOxygen and argon
  • BOxygen and water
  • CCarbon dioxide and water
  • DWater and argon
  • EOxygen and carbon dioxide

Give a balanced chemical equation for the reaction of air with hydrogen.

  • A O + 2 H 2 H O 2 2 2
  • B O + H H O 2 2 2 2
  • C N + 3 H 2 N H 2 2 3
  • D N + 3 O + H 2 H N O 2 2 2 3
  • E N + 2 H 2 N H 2 2 2

The reaction of air with hydrogen is an example of an irreversible reaction. What is meant by this term?

  • AThe amount of product that converts back to the original reactants is very close to zero under the reaction conditions.
  • BThe product of the reaction is removed as it forms, preventing it from converting back to the original reactants.
  • CThe products of the reaction can never be converted back to the original reactants under the reaction conditions.
  • DThe reaction is highly exothermic.
  • EThe products of the reaction are much more stable than the reactants.

Which method can be used to separate the product of this reaction from the nitrogen gas?

  • ACooling and drying
  • BFiltering and distilling
  • CCooling and distilling
  • DHeating and distilling
  • EHeating and filtering

Q13:

At what gas pressure, in atmospheres, is the reaction of the Haber process typically performed?

Q14:

The reaction of 30.0 kg of hydrogen with excess nitrogen generates 93.5 kg of product via the Haber process. Calculate the percentage yield of this reaction.

Q15:

Which feature of a typical reactor in the Haber process allows very high maximum percentage yields to be achieved?

  • ARecycling of reactants
  • BDrying of the reaction mixture
  • CThe presence of a catalyst
  • DHeating of the reaction mixture
  • ECompression of the reaction mixture

Q16:

The Haber process involves the reversible reaction of two gaseous reactants. What is the main disadvantage of increasing the pressure at which the reaction is performed?

  • AIncreased equipment and running costs
  • BCondensation of the gaseous reactants
  • CReduced maximum percentage yield
  • DIncreased formation of unwanted side products
  • EReduced reaction rate
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