Determine the entropy change of helium during this process assuming the process is irreversible. The gas constant of helium is R=0.4961 Btu/lbm-R. The constant volume specific heat of helium at room temperature is cv = 0.753 Btu/lbm-R.The entropy change of helium during this process is______ Btu/R.

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Answer 1

The entropy change of helium during an irreversible process can be calculated using the formula ΔS = cv × ln(T2/T1).

How can you calculate the entropy change of helium during an irreversible process?

The entropy change of helium during the process assuming the process is irreversible is

0.214 Btu/R

Here is how to solve it: Entropy (S) can be defined as the measure of disorder or randomness of a system. The entropy change of helium during the process assuming the process is irreversible can be calculated as follows:

ΔS = cv × ln(T2/T1)

where've is the constant volume specific heat of helium at

room temperature = 0.753 Btu/lbm-Rln

is the natural logarithmT2 is the final temperature of the heliumT1 is the initial temperature of the helium.R is the

gas constant of helium = 0.4961 Btu/lbm-R

T1 is not given, so let us assume that it is the

room temperature of 298 K

The temperature at the end of the process is not given, so we will solve the equation using a variable for

T2.ΔS = cv × ln(T2/T1)ΔS

= 0.753 × ln(T2/298)ΔS

= 0.753 × (ln T2 - ln 298)ΔS

= 0.753 ln T2 - 0.753 ln 298

Rearranging the equation,

ΔS = 0.753 ln T2 - 0.214

Therefore, the entropy change of helium during the process assuming the process is irreversible is 0.214 Btu/R.

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