A balloonist begins a trip in a helium-filled balloon in early morning when the temperature is 15°C. By mid-afternoon, the temperature is 30.°C. Assuming the pressure remains at 1.00 atm, for each mole of helium, calculate the following:
(b) The change in internal energy, ΔE (Hint: Helium behaves like an ideal gas, so E=3/2 nRT. Be sure the units of R are consistent with those of E.)

Question

23-08-2022
Chemistry

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A balloonist begins a trip in a helium-filled balloon in early morning when the temperature is 15°C. By mid-afternoon, the temperature is 30.°C. Assuming the pressure remains at 1.00 atm, for each mole of helium, calculate the following:
(b) The change in internal energy, ΔE (Hint: Helium behaves like an ideal gas, so E=3/2 nRT. Be sure the units of R are consistent with those of E.)

Answer :

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tripatsingh039 tripatsingh039 · Answer 1 · 2022-08-26T08:05:44-04:00

The change in internal energy, ΔE is 187.06J.

A thermodynamic system's internal energy is its total internal energy. The internal energy of an isolated system is constant. It is the energy required to prepare the system for its current internal condition or to develop it from scratch.

Internal energy, which is provided by the kinetic energy of the molecules, is the microscopic energy that is present in a substance. It also contains the nuclear energy held in the atoms of these molecules as well as the potential energy between them.

Cv =3/2 R

ΔE = nCvΔT

ΔE = 1×3/2 R × (303 −288)

ΔE = [tex]\frac{3* 8.314}{2}[/tex] × 15

ΔE = 187.06 J

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