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es. N2(g) + 3H2(g) ⇌ 2NH3 (g) + heat energy nitrogen gas + hydrogen gas react reversibly to form ammonia gas + heat Please use the image above to help you count moles of reactants and products to determine which direction the shift will take the experimenter under the conditions applied. The equation is balanced for you. (6 points) Forward Reaction (shift right) Reverse Reaction (shift left) The experimenter ADDS heat to the closed system. The experimenter counts 2 moles of nitrogen and 6 moles of hydrogen gas in the closed system. The experiment counts 8 moles of ammonia in the closed system. The experimenter counts 1 mole of ammonia in the closed system. The experimenter ADDS the catalyst of iron to break the triple covalent bonds in nitrogen gas. [Check Lesson 7.4 for help if needed!] The experimenter REMOVES heat from the closed system. Skip to navigation they all nedd one answer for all there should be six and make it simple

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Let's analyze each scenario based on Le Chatelier's Principle, which states that if a system at equilibrium is disturbed, it will shift to counteract the disturbance.

  1. Experimenter ADDS heat to the closed system:

    • The forward reaction produces heat (exothermic). Adding heat shifts the equilibrium to the left (toward reactants).
    • Direction of shift: Reverse Reaction (shift left)

  2. Experimenter counts 2 moles of nitrogen and 6 moles of hydrogen gas, and 8 moles of ammonia:

    • Moles: 2 (N2) + 6 (H2) ⇌ 8 (NH3)
    • There are more product moles (8) than reactant moles (8 total, which is 2 + 6).
    • This suggests the reaction favors products at this moment, but does not indicate a shift due to changes.
    • No shift indicated for this scenario.

  3. Experimenter counts 1 mole of ammonia in the closed system:

    • Moles: 2 (N2) + 6 (H2) ⇌ 1 (NH3)
    • This indicates a higher concentration of reactants compared to products, implying a shift toward products.
    • Direction of shift: Forward Reaction (shift right)

  4. Experimenter ADDS the catalyst of iron:

    • A catalyst speeds up the rate of both the forward and reverse reactions equally but does not affect the position of equilibrium.
    • No shift indicated (no change in direction).

  5. Experimenter REMOVES heat from the closed system:

    • Removing heat shifts the equilibrium to the right (toward products, which release heat).
    • Direction of shift: Forward Reaction (shift right)

In summary:

  1. ADDS heat: Shift left
  2. Counts 2 N2, 6 H2, 8 NH3: No shift
  3. Counts 1 NH3: Shift right
  4. ADDS catalyst: No shift
  5. REMOVES heat: Shift right