Chemistry, asked by vadlakuntapravallika, 5 hours ago

Consider a thermodynamic process for which initial pressure and temperature are 8 bar and 350 K respectively. Upon expansion process, pressure and temperature changes to 2 bar and 300 K Calculate is the change in entropy for 1 kmol of an ideal gas. Use. Co = 29.3 kJ/kmol-K a) 8.50kJ kamol-K b) 7.00 kJ/kmol-K c) 6.32 kJ/kmol-K d) 5.00kJ/kmol-K​

Answers

Answered by mintu78945
0

7.00 kJ K⁻¹ kmol⁻¹ is the change in entropy for 1 kmol of an ideal gas.

Explanation:

Given:

  • n = 1 kilomole
  • P₁ = 8 bar
  • P₂ = 2 bar
  • T₁ = 350 K
  • T₂ = 300 K
  • Cp = 29.3 kJ K⁻¹ kmol⁻¹

To find:

  • ΔS = ?

The change in entropy of a system can be given by the following formula:

  • \Delta S=nC_{p}ln\frac{T_{2}}{T_{1}}+nRln\frac{P_{1}}{P_{2}}

On substituting the value of the given variables in the above formula, we get:

  • \Delta S=1\times 29.3 \times ln\frac{300}{350}+1\times 8.314 \times ln\frac{8}{2}
  • \Delta S=7.00kJK^{-1} kmol^{-1}
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