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you add equal amounts of heat to two identical cylinders containing equal amounts of the same ideal gas. cylinder a is allowed to expand, while cylinder b is not. Part A How do the temperature changes of the two cylinders compare?

Answer :

The temperature rise the second cylinder B is 5/3 times the temperature in the cylinder A.

Explain the ideal gas equation?

  • PV = nRT is the equation for an ideal gas.
  • In this equation,
  1. P stands for the ideal gas's pressure,
  2. V for the ideal gas' volume,
  3. n for the total amount of the ideal gas expressed in moles,
  4. R for the universal gas constant, and
  5. T for temperature.

The heat source for both cylinders was:

ΔQ₁ = ΔQ₂  .....eq 1

Gas will expand in a cylinder with a free piston so that the pressure is always constant.

P = constant

Then,

ΔQ₁ = n.Cp.ΔT

ΔQ₁ = n.Cp.T₀  .....eq 2

With Fixed piston for cylinder (constant volume process),

V = constant

ΔQ₁ = n.Cv.ΔT  .....eq 3

From eq 1

n.Cp.T₀  =  n.Cv.ΔT

ΔT = (Cp/Cv) . T₀

ΔT = γ T₀

For the monatomic gas (γ = 5/3)

ΔT = 5/3 T₀

Thus, the temperature rise the second cylinder B is 5/3 times the temperature in the cylinder A.

To know more about the ideal gas equation, here

https://brainly.com/question/27870704

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