11 fg to whoever can answer this.

Nitrogen and hydrogen react in the Haber process to form ammonia. All substances are in the gas phase. If 0.518 atm of nitrogen and 0.719 atm of hydrogen react, what is the partial pressure of ammonia (in mmHg) when this reaction goes 74.8 complete. The volume and temperature are constant.

H2 is the limiting reagent.

You have .719 atm of H2

Reaction goes to 74.8% of completion so you should have

(.719 * .748) amount of hydrogen reacted

This means you should have (.719 * .748) * (2/3) atm of NH2

Convert to mmHg by multiplying by 760

perfect, thanks