Two constant-volume gas thermometers are assembled, one with nitrogen and the ot

Question

Two constant-volume gas thermometers are assembled, one with nitrogen and the other with hydrogen. Both contain enough gas so that p_3 = 80.0 kPa. (a) What is the difference between the pressures in the two thermometers if both bulbs are in boiling water? (b) Which gas is at higher pressure, nitrogen or hydrogen? Indications of the constant-volume gas thermometer for a boiling point of water depending on pressure at the triple point of water for various gases (a) Number 5.5 e - 5 Units kPa nitrogen

Explanation / Answer

Deducing from ideal gas equation:

T/P = T3/P3

P = P3 (T/T3)

For nitrogen, T = 373.35 K ; T3 = 273.16 K ; P3 = 80 kPa

P = 80 x (373.35/273.16) = 109.343 kPa

P = 109.343 kPa

for hydrogen, T = 373.15 ; T3 = 273.16 K ; P3 = 80 kPa

P' = 80 (373.15/273.16) = 109.284 kPa

delta-P = P - P' = 109.343 - 109.284 = 0.059 kPa = 59 Pa

Hence, Pressure Diffrence = delta-P = 59 Pa

(b)Nitrogen is at higher Pressure.

Related Questions

Navigate

• Browse (All)
• Browse T
• Subjects

---

---

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