nitrogen and hydrogen react in the haber process to form ammonia. All substances are in the gas phase. If 0.385atm of nitrogen and 0.792 atm of hydrogen react, what is the partial pressure of ammonia(in mmHg) when this reaction goes 67 complete. The volume and temperature are constant.

To determine the partial pressure of ammonia, we need to calculate the partial pressures of nitrogen and hydrogen first and then use the stoichiometry of the reaction to determine the change in partial pressure.

1. Calculate the partial pressures of nitrogen and hydrogen:
- Given: Nitrogen pressure (P₁) = 0.385 atm, Hydrogen pressure (P₂) = 0.792 atm
- The partial pressure of a gas is the pressure it would exert if it alone occupied the whole container at the same temperature.
- Since the volume and temperature remain constant, the partial pressures of nitrogen and hydrogen are equal to their initial pressures (P₁ and P₂).

2. Determine the change in partial pressure:
- We know that the reaction goes 67% complete. This means that if we assume 100% completion as the total pressure, then the partial pressure of ammonia will be 67% of the total pressure.
- Let's denote the partial pressure of ammonia as P₃. So, P₃ = 0.67 * Total Pressure.

3. Find the total pressure:
- To find the total pressure, we need to use the stoichiometry of the reaction.
- The balanced equation for the reaction is:
N₂ + 3H₂ → 2NH₃
- This means that for every 1 mole of nitrogen reacting, we produce 2 moles of ammonia.
- Given only partial pressures, we need to make sure to consider the mole fraction of the gases.
- Since the number of moles of a gas is directly proportional to its partial pressure, we can write the following relationship:
(P₁/P₃) = (moles of nitrogen reacted/moles of ammonia produced)
- Since the mole fractions remain constant, the moles of nitrogen reacted is proportional to its initial partial pressure (P₁) and the partial pressure of ammonia is proportional to the total pressure (P₃).
- Therefore, we can rewrite the equation as:
(P₁/P₃) = (initial moles of nitrogen/total moles of ammonia)
Note: 1 mole of nitrogen reacts to produce 2 moles of ammonia.

4. Solve for P₃ (partial pressure of ammonia):
- Rearrange the equation to find P₃:
P₃ = (P₁ * total moles of ammonia) / (initial moles of nitrogen * 2)

5. Convert the final answer to mmHg:
- The final answer should be in mmHg since the question asks for it.
- 1 atm = 760 mmHg, so we can convert the pressure from atm to mmHg by using the conversion factor.
- Multiply the found pressure (P₃) by 760 mmHg/atm to get the pressure in mmHg.

Well, 67 percent of the reactants have changed to product, so the relative proportion of reactants is now...

reactants=.37 of total pressure, so

pressure nitrogen=.37 initial nitrogen partial pressure, and the same thinking for H2.

check my thinking.