1) Nitrogen and hydrogen gases react to form ammonia gas as follows: N,(g) + 3H/

Question

1) Nitrogen and hydrogen gases react to form ammonia gas as follows: N,(g) + 3H/g) 2NH,(g) At a certain temperature and pressure, 1.2 L of N reacts with 3.6 L of H.. If all the N and H are consumed, what volume of NH, at the same temperature and pressure, will be produced? 2) The pressure in a natural gas tank is maintained at 2.20 atm. On a day when the temperature is-15 °C, the volume of gas in the tank is 3.25 x 10 m2. What is the volume of the same quantity of gas on a day when the temperature is 31 ? 3) A sample of 5.00 mL of diethylether (C,H,OC H, density-0.7134 gimL) is introduced into a 6.00 L vessel that already contains a mixture of Na and O, whose partial pressure are P-0.751 atm and Po 0.208 atm. The temperature is held at 35.0°C, and the diethylether totally evaporates. (a) Calculate the partial pressure of the

Explanation / Answer

Ans 1 :

Equal amounts of all gases at same temperature and pressure occupy the same amount of volumes.

The reaction utilises three moles of H2 per mole of nitrogen to produce 2 moles of ammonia.

The volumes mentioned in the question are in consistence with the number of moles participating in the reaction.

So when 1 mole N2 makes 2 moles of ammonia

So 1.2 L of N2 will make 1.2 x 2 = 2.4 L of ammonia.

Related Questions

Navigate

• Browse (All)
• Browse 1
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.