1.5kg of metal is placed in 3.7 kg of an ideal gas with specific heat 14.7J/K. T

Question

1.5kg of metal is placed in 3.7 kg of an ideal gas with specific heat 14.7J/K. The gas has an initial temperature of 240 degrees Celsius, and the metal has an initial temp of 50 degrees Celsius A) if the final temperature is 110 degrees Celsius, what is the specific heat of the metal? Assume no phase shift B) if the process occured under constant pressure, by what percentage did the volume of gas decrease? 1.5kg of metal is placed in 3.7 kg of an ideal gas with specific heat 14.7J/K. The gas has an initial temperature of 240 degrees Celsius, and the metal has an initial temp of 50 degrees Celsius A) if the final temperature is 110 degrees Celsius, what is the specific heat of the metal? Assume no phase shift B) if the process occured under constant pressure, by what percentage did the volume of gas decrease? A) if the final temperature is 110 degrees Celsius, what is the specific heat of the metal? Assume no phase shift B) if the process occured under constant pressure, by what percentage did the volume of gas decrease?

Explanation / Answer

A) heat gained by metal = heat lost by gas

1.5kg*S*(110-50) = 3.7kg*14.7J/kg degC*(240-110)

Specific heat of metal, S = 78.6 J/kg deg C

B) at constant pressure

V1/T1 = V2/T2

V2 = (V1/T1)*T2

= (V1/513K)*383K

= 0.75 V1

Percentage of volume decreased = 25 %

Related Questions

Navigate

• Browse (All)
• Browse 1
• Subjects

---

---

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