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Lesson Worksheet: The Haber Process Chemistry • 10th Grade

In this worksheet, we will practice describing the reaction of nitrogen and hydrogen in the Haber process and explaining the choices of reaction conditions.

Q1:

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.

Q2:

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

  • ADrying of the reaction mixture
  • BRecycling of reactants
  • CCompression of the reaction mixture
  • DHeating of the reaction mixture
  • EThe presence of a catalyst

Q3:

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

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

Q4:

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

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

Q5:

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

Q6:

The Haber process is a gas-phase reaction involving hydrogen gas (H)2. A major source of hydrogen gas is the reaction of methane (CH)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.

  • ACH+2HOCO+8H4222
  • BCH+HOCO+2H422
  • CCH+2HO2CO+4H422
  • DCH+2HOCO+4H4222
  • ECH+HOCO+3H422

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 and percentage yield both increase.
  • DThe reaction rate and percentage yield both decrease.
  • EThe reaction rate decreases and the percentage yield increases.

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.

  • ACO+2HOCO+2H232
  • BCO+HOCO+H222
  • CCO+2HOHCO+H2232
  • DCO+HOC+O+H222
  • E2CO+4HO2HCO+3H232

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

Q7:

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.

Q8:

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?

  • ACondensation of the gaseous reactants
  • BReduced reaction rate
  • CReduced maximum percentage yield
  • DIncreased equipment and running costs
  • EIncreased formation of unwanted side products

Q9:

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?

  • AIncreased formation of unwanted side products
  • BIncreased equipment and running costs
  • CReduced reaction rate
  • DReduced maximum percentage yield
  • EMelting of the solid catalyst

Q10:

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?

  • ACarbon dioxide and water
  • BOxygen and argon
  • COxygen and water
  • DOxygen and carbon dioxide
  • EWater and argon

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

  • AN+3H2NH223
  • BN+2H2NH222
  • CN+3O+H2HNO2223
  • DO+HHO2222
  • EO+2H2HO222

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

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

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

  • AHeating and distilling
  • BCooling and drying
  • CHeating and filtering
  • DFiltering and distilling
  • ECooling and distilling

This lesson includes 17 additional questions for subscribers.

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