Chemistry: Equilibrium Reactions and Haber Process
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Questions and Answers

What is the balanced chemical equation for the reaction between iodine monochloride and chlorine?

  • I2 + Cl2 → 2ICl (correct)
  • I2 + 2Cl2 → 2ICl3
  • ICl + I2 → 2ICl
  • ICl + Cl2 → ICl3

    • What effect does increasing temperature have on the rate of reaction?

  • The rate decreases due to less kinetic energy.
  • The rate remains unchanged.
  • The rate becomes zero.
  • The rate increases due to more kinetic energy. (correct)

    • The forward and backward reactions in a dynamic equilibrium occur at different rates.

    False

    An increase in temperature will always favor an exothermic reaction.

    <p>False</p> Signup and view all the answers

    What color change indicates that the equilibrium mixture is shifting towards iodine monochloride when heated?

    <p>Darker brown</p> Signup and view all the answers

    Iodine monochloride reacts reversibly with chlorine to form iodine ___________.

    <p>trichloride</p> Signup and view all the answers

    What is the empirical formula of the main compound in AmmoBoost?

    <p>N2H4O3</p> Signup and view all the answers

    The percentage by mass of oxygen in AmmoBoost is _____%.

    <p>60</p> Signup and view all the answers

    Match the following elements with their respective states in the ammonia reaction:

    <p>N2 = Gas H2 = Gas NH3 = Gas Fe = Solid Catalyst</p> Signup and view all the answers

    What happens to the equilibrium position when the pressure of a gas reaction is increased?

    <p>Equilibrium shifts to the side with fewer gas molecules.</p> Signup and view all the answers

    What can be said about the enthalpy change (ΔH) of the reaction forming ammonia?

    <p>Negative value indicates exothermic reaction</p> Signup and view all the answers

    Increasing pressure in a reaction with more moles on one side will favor that side.

    <p>False</p> Signup and view all the answers

    Increasing the temperature will favor the exothermic backward reaction.

    <p>True</p> Signup and view all the answers

    Describe the state of concentrations of reactants and products at dynamic equilibrium.

    <p>They remain constant.</p> Signup and view all the answers

    What is the main compound in AmmoBoost that contains nitrogen and hydrogen?

    <p>AmmoBoost compound</p> Signup and view all the answers

    Match the following statements regarding temperature and pressure changes in equilibrium reactions:

    <p>Higher temperature = Equilibrium shifts left (endothermic) Decrease in pressure = Equilibrium shifts to side with more moles Increase in pressure = Equilibrium shifts to side with fewer moles Lower temperature = Equilibrium shifts right (exothermic)</p> Signup and view all the answers

    What happens to the yield of hydrogen when the reaction is carried out at a higher temperature?

    <p>It decreases.</p> Signup and view all the answers

    A catalyst affects the enthalpy change of a reaction.

    <p>False</p> Signup and view all the answers

    What is the catalyst used in the conversion of nitrogen gas and hydrogen gas into ammonia?

    <p>Iron, Fe</p> Signup and view all the answers

    The enthalpy change for the reaction producing ammonia is represented by the symbol ___ .

    <p>ΔH</p> Signup and view all the answers

    Match the following reactions with their classifications:

    <p>N2 + 3H2 → 2NH3 = Reduction 4NH3 + 5O2 → 4NO + 6H2O = Oxidation 2NO2 → N2O4 = Redox NH3 + HNO3 → NH4NO3 = Non-redox</p> Signup and view all the answers

    What is the relative formula mass of ammonium nitrate (NH4NO3)?

    <p>80</p> Signup and view all the answers

    Increasing temperature always increases the yield of a product in an exothermic reaction.

    <p>False</p> Signup and view all the answers

    How is the maximum mass of ammonium nitrate produced calculated from ammonia?

    <p>Calculate moles of ammonia and use the formula mass of ammonium nitrate.</p> Signup and view all the answers

    The source of nitrogen gas is ___ .

    <p>air</p> Signup and view all the answers

    Match the following gases with their sources:

    <p>Nitrogen gas = Air Hydrogen gas = Water Oxygen gas = Air Ammonia = Natural gas</p> Signup and view all the answers

    What is the main component of nitrogen gas in the atmosphere?

    <p>Nitrogen</p> Signup and view all the answers

    A higher temperature shifts the equilibrium position to favor products in an exothermic reaction.

    <p>False</p> Signup and view all the answers

    What is indicated by a negative ΔH value in a reaction?

    <p>The reaction is exothermic.</p> Signup and view all the answers

    The maximum mass of ammonia obtained from 56 tonnes of nitrogen is ___ tonnes.

    <p>68</p> Signup and view all the answers

    What happens when the temperature is increased at constant pressure in the production of ammonia?

    <p>The yield of ammonia decreases.</p> Signup and view all the answers

    Increasing pressure during a reaction favors the side with more gas molecules.

    <p>False</p> Signup and view all the answers

    What is the expected yield of ammonia in the Haber process?

    <p>30%</p> Signup and view all the answers

    The reaction between nitrogen and hydrogen in the Haber process produces __________.

    <p>ammonia</p> Signup and view all the answers

    Match the following terms with their definitions:

    <p>Haber process = A method of synthesizing ammonia Equilibrium = State where the rates of forward and reverse reactions are equal Catalyst = Substance used to increase the rate of a reaction without being consumed Exothermic reaction = Reaction that releases heat</p> Signup and view all the answers

    Which statement about equilibrium is true?

    <p>Concentrations of reactants and products remain constant.</p> Signup and view all the answers

    A higher temperature in the Haber process will result in a higher yield of ammonia.

    <p>False</p> Signup and view all the answers

    Explain why the actual yield of ammonia in the Haber process is lower than expected.

    <p>The position of equilibrium is not reached.</p> Signup and view all the answers

    To separate ammonia from unreacted nitrogen and hydrogen, the gas mixture is __________.

    <p>cooled</p> Signup and view all the answers

    In the equilibrium of 2NO2(g) ⇌ N2O4(g), pulling the plunger out reduces the pressure. What happens?

    <p>The mixture becomes darker in color.</p> Signup and view all the answers

    The Haber process uses an iron catalyst to speed up the reaction.

    <p>True</p> Signup and view all the answers

    What happens to the unreacted nitrogen and hydrogen after the reaction?

    <p>They are recycled.</p> Signup and view all the answers

    The relative formula mass of nitrogen (N2) is __________.

    <p>28</p> Signup and view all the answers

    What is the role of pressure in the Haber process?

    <p>Favors the side with fewer gas molecules.</p> Signup and view all the answers

    In the reaction 2NO2(g) ⇌ N2O4(g), NO2 is the colorless compound.

    <p>False</p> Signup and view all the answers

    Which statement is true regarding the reaction between nitrogen dioxide and dinitrogen tetroxide?

    <p>Decreasing temperature favors the formation of N2O4.</p> Signup and view all the answers

    An increase in temperature shifts the equilibrium towards the exothermic direction.

    <p>False</p> Signup and view all the answers

    What is the change in color observed when the mixture of NO2 and N2O4 is cooled?

    <p>The color changes from brown to pale yellow.</p> Signup and view all the answers

    The reaction of carbon monoxide and hydrogen to form methanol is an example of a __________ reaction.

    <p>reversible</p> Signup and view all the answers

    What happens to methanol when the temperature is decreased at constant pressure?

    <p>The amount of methanol increases.</p> Signup and view all the answers

    A catalyst alters the activation energy of a reaction.

    <p>True</p> Signup and view all the answers

    Write the chemical equation for the complete combustion of methanol.

    <p>2CH3OH + 3O2 → 2CO2 + 4H2O</p> Signup and view all the answers

    The reaction of CO(g) + H2O(g) ↔ CO2(g) + H2(g) has a ΔH value of __________.

    <p>-41 kJ/mol</p> Signup and view all the answers

    What is the effect of increasing pressure on the equilibrium mixture of CO(g) + 2H2(g) ↔ CH3OH(g)?

    <p>Favors the formation of methanol.</p> Signup and view all the answers

    Bond making is an exothermic process.

    <p>True</p> Signup and view all the answers

    Explain how changing temperature affects the yield of products in a reversible reaction.

    <p>A decrease in temperature favors the exothermic reaction and increases product yield, whereas an increase in temperature favors the endothermic reaction, which can reduce product yield.</p> Signup and view all the answers

    A __________ provides an alternative reaction pathway with a lower activation energy.

    <p>catalyst</p> Signup and view all the answers

    In the reaction CO + 2H2 ↔ CH3OH, how many moles of gas are present on both sides?

    <p>3 moles on left, 1 mole on right.</p> Signup and view all the answers

    What is the role of an iron oxide catalyst in the conversion of methanol to methanal?

    <p>To increase the rate of the reaction without being consumed.</p> Signup and view all the answers

    Study Notes

    Equilibrium Reactions and Haber Process

    • Iodine Monochloride and Chlorine Reaction: Iodine monochloride (ICl) reacts reversibly with chlorine (Cl₂) to form iodine trichloride (ICl₃). The reaction is represented as: ICl + Cl₂ ⇌ ICl₃.
    • Dynamic Equilibrium Features: A reaction in dynamic equilibrium has the following features:
      • Simultaneous forward and backward reactions
      • Constant concentrations of reactants and products
      • Equal rates of forward and reverse reactions
    • Balancing Chemical Equations: Correct formulae for reactants and products are crucial in balancing chemical equations. Halogens are diatomic. The balanced equation for iodine and chlorine forming iodine monochloride is: I₂ + Cl₂ → 2ICl
    • Effect of Heat on Equilibrium: Heating the ICl/Cl₂ reaction mixture leads to a darker brown colour. This indicates that the backward reaction (formation of ICl and Cl₂) is favored, and thus the backward reaction is endothermic.
    • Haber Process (Ammonia Production): Ammonia (NH₃) is produced by reacting nitrogen (N₂) and hydrogen (H₂). The reaction is reversible, and the conditions used strongly influence the yield. The reaction is exothermic, as represented by: N₂(g) + 3H₂(g) ⇌ 2NH₃(g) ∆H = –92 kJ/mol
      • Increase in temperature: Decreases ammonia yield as the backward (endothermic) reaction is favored.
      • Increase in pressure: Increases ammonia yield as the reaction favors the side with fewer gas molecules (2 moles of NH₃).
    • Haber Process Actual Yield: The actual yield (15%) of ammonia is lower than the expected yield (30%) due to factors like not reaching equilibrium conditions.
      • Separation of Ammonia: Ammonia is separated from unreacted nitrogen and hydrogen by cooling the mixture, which causes the ammonia to liquefy.
      • Unreacted Gases: Unreacted nitrogen and hydrogen gases are recycled for reuse in the process.
      • Temperature Limitation: Higher temperatures speed up the reaction, but would result in greater energy costs
    • Nitrogen Dioxide/Dinitrogen Tetraoxide Equilibrium: Nitrogen dioxide (NO₂) and dinitrogen tetraoxide (N₂O₄) exist in equilibrium: 2NO₂(g) ⇌ N₂O₄(g). Brown color, when pressure is decreased, equilibrium shifts to the left, favoring NO₂ formation & increasing brown color.
      • Effect of Temperature: A decrease in temperature favors the exothermic direction (forward reaction), leading to a pale yellow color, indicating more N₂O₄ formation.
      • Supports Exothermic Forward Reaction: Bond formation (exothermic) in the forward reaction supports the claim that it's exothermic.

    Methanol Production

    • Methanol Production Conditions: Carbon monoxide (CO) and hydrogen (H₂) are used to produce methanol (CH₃OH): CO(g) + 2H₂(g) ⇌ CH₃OH(g) ∆H = –91 kJ/mol. At 100 atm and 250°C
      • Decrease in Temperature: Favor the forward reaction (exothermic), increasing methanol yield.
      • Increase in Pressure: Favor the forward reaction (fewer gas molecules), increasing methanol yield.
    • Methanol to Methanal Conversion: Methanol (CH₃OH) can be converted to methanal (H₂CO) in the presence of an iron oxide catalyst: 2CH₃OH + O₂ → 2H₂CO + 2H₂O
    • Catalyst Definition: A catalyst increases reaction rate, remaining chemically unchanged.
    • Catalyst Mechanism: Catalyst provides an alternative reaction pathway with lower activation energy.
    • Complete Combustion of Methanol: The complete combustion of methanol produces carbon dioxide (CO₂) and water (H₂O): 2CH₃OH + 3O₂ → 2CO₂ + 4H₂O
    • Fertilizer Production (Ammonia): Ammonia (NH₃) is manufactured using nitrogen (from air) and hydrogen (produced by steaming methane). Key Haber Process materials include nitrogen, hydrogen, ammonia, iron catalyst and nitric acid.
      • Reaction 1 (Steam Methane Reaction): CH₄ + H₂O → CO + 3H₂.
      • Reaction 2 (CO/H₂O reaction): CO(g) + H₂O(g) ⇌ CO₂(g) + H₂(g) ∆H = –41 kJ/mol. Higher pressure has no effect on yield. Higher temperatures decreases reaction yield/favors endothermic reaction.
      • Iron Oxide Catalyst: Improves reaction rate without altering enthalpy change.
      • Redox Reactions in Fertilizer Manufacture: The redox reactions are reaction 3 (nitrogen and hydrogen producing ammonia) and reaction 4 (ammonia reacting with oxygen producing water and nitric oxide).

    Further Calculations and Concepts

    • Ammonia Production from Nitrogen: Calculating the theoretical and practical (15%) yields of ammonia from 112 kg of nitrogen.
      • Moles of Nitrogen: 112,000 g / 28 g/mol = 4000 moles
      • Theoretical Moles of Ammonia: 4000 moles × 2 = 8000 moles
      • Actual Moles of Ammonia: The actual yield is 15% of 8000 moles = 1200 moles
    • Ammonia to Ammonium Nitrate: Calculating the maximum mass of ammonium nitrate produced with reaction 6, from 34 kg of ammonia:
      • Mass of ammonia (g): 34,000 g
      • Moles of ammonia: 34,000 g / 17 g/mol = 2000 moles
      • Moles of Ammonium Nitrate: 2000 moles
      • Molar Mass of Ammonium Nitrate: 80 g/mol
      • Mass of Ammonium Nitrate: 2000 moles × 80 g/mol = 160,000 g = 160 kg
    • AmmoBoost Fertilizer Composition: AmmoBoost contains 35% nitrogen and 5% hydrogen by mass. Calculating the empirical formula and compound name for the fertilizer are not addressed in this summary as details have been skipped out.

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    Description

    This quiz explores the principles of equilibrium reactions, focusing on the iodine monochloride reaction and the effects of heat on equilibrium. Additionally, it covers the Haber process, emphasizing the importance of balancing chemical equations and the dynamic nature of chemical reactions. Test your knowledge of these concepts!

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