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.

Question

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.
they all nedd one answer for all there should be six and make it simple

Answer 1

Sure! Below are the effects on the reaction direction for each condition applied by the experimenter:

1. The experimenter ADDS heat to the closed system.

   • Shift direction: Left (reverse reaction). Adding heat to an exothermic reaction will shift the equilibrium to favor the reactants.

2. The experimenter counts 2 moles of nitrogen and 6 moles of hydrogen gas in the closed system.

   • Shift direction: Right (forward reaction). There are more moles of reactants (2 N2 + 6 H2 = 8 moles) compared to products (8 moles of NH3). The system will shift to the right to form more products.

3. The experiment counts 8 moles of ammonia in the closed system.

   • Shift direction: Left (reverse reaction). With more products (8 moles of NH3) than reactants (2 moles of N2 and 6 moles of H2 = 8 moles), the system will shift left to form reactants.

4. The experimenter counts 1 mole of ammonia in the closed system.

   • Shift direction: Right (forward reaction). With fewer products (1 mole of NH3) compared to the moles of reactants (2 N2 and 6 H2 = 8 moles), the equilibrium will shift right to produce more ammonia.

5. The experimenter ADDS the catalyst of iron to break the triple covalent bonds in nitrogen gas.

   • Shift direction: No shift. A catalyst speeds up both the forward and reverse reactions but does not change the position of equilibrium.

6. The experimenter REMOVES heat from the closed system.

   • Shift direction: Right (forward reaction). Removing heat from an exothermic reaction will shift the equilibrium toward the production of more heat (and thus more products).

I hope this simplifies the response for you!