On a P-V diagram of an ideal gas, suppose a reversible adiabatic line intersects a reversible isothermal line at point A. Then at a point A, the slope of the reversible adiabatic line $${\left( {\frac{{\partial {\text{P}}}}{{\partial {\text{V}}}}} \right)_{\text{S}}}$$ and the slope of the reversible isothermal line $${\left( {\frac{{\partial {\text{P}}}}{{\partial {\text{V}}}}} \right)_{\text{T}}}$$ are related as (where, $${\text{y}} = \frac{{{{\text{C}}_{\text{p}}}}}{{{{\text{C}}_{\text{v}}}}}$$ )
A. $${\left( {\frac{{\partial {\text{P}}}}{{\partial {\text{V}}}}} \right)_{\text{S}}} = {\left( {\frac{{\partial {\text{P}}}}{{\partial {\text{V}}}}} \right)_{\text{T}}}$$
B. $${\left( {\frac{{\partial {\text{P}}}}{{\partial {\text{V}}}}} \right)_{\text{S}}} = {\left[ {{{\left( {\frac{{\partial {\text{P}}}}{{\partial {\text{V}}}}} \right)}_{\text{T}}}} \right]^{\text{y}}}$$
C. $${\left( {\frac{{\partial {\text{P}}}}{{\partial {\text{V}}}}} \right)_{\text{S}}} = {\text{y}}{\left( {\frac{{\partial {\text{P}}}}{{\partial {\text{V}}}}} \right)_{\text{T}}}$$
D. $${\left( {\frac{{\partial {\text{P}}}}{{\partial {\text{V}}}}} \right)_{\text{S}}} = \frac{1}{{\text{y}}}{\left( {\frac{{\partial {\text{P}}}}{{\partial {\text{V}}}}} \right)_{\text{T}}}$$
Answer: Option C
Solution(By Examveda Team)
For an adiabatic process → $$P{V^y}$$ = constantFor an isothermal process → $$PV$$ = constant
So, slope for adiabatic process in $$PV$$ plane is $$\frac{{dp}}{{dv}} = - y\frac{p}{v}$$
Slope for isothermal process is $$\frac{{dp}}{{dv}} = - \frac{p}{v}$$
Hence, $${\left( {\frac{{\partial p}}{{\partial v}}} \right)_S} = - y{\left( {\frac{{\partial p}}{{\partial v}}} \right)_T}$$
A. Maxwell's equation
B. Thermodynamic equation of state
C. Equation of state
D. Redlich-Kwong equation of state
Henry's law is closely obeyed by a gas, when its __________ is extremely high.
A. Pressure
B. Solubility
C. Temperature
D. None of these
A. Enthalpy
B. Volume
C. Both A & B
D. Neither A nor B
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