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.Management Sciences
Category: Thermodynamics for Chemical
Heat evolved/absorbed during conversion of a substance from one allotropic form to another is termed as the heat of______________?
A. Fusion
B. Vaporisation
C. Transition
D. None of these
A refrigeration cycle is the same as a _____________ cycle?
A. Turbine
B. Heat engine
C. Reversed heat engine
D. None of these
In which of the following reaction equilibrium, the value of equilibrium constant Kp will be more than is Kc ?
A. 2HI ⇌ H2 + I2
B. N2O4 ⇌ 2NO2
C. 2SO2 + O2 ⇌ 2SO3
D. None of these
Isotherm on an enthalpy-concentration diagram, for an ideal solution will be a __________________?
A. Straight line
B. Sine curve
C. Parabola
D. Hyperbola
For a constant volume process _____________ by the system is used only to increase the internal energy?
A. Heat absorbed
B. Work done
C. Both A. & B
D. Neither A. nor B
The internal energy of an ideal gas is a function of its _____________ only?
A. Molecular size
B. Volume
C. Pressure
D. Temperature
For a given substance at a specified temperature, activity is ______________ to fugacity?
A. Directly proportional
B. Inversely proportional
C. Equal
D. None of these
High pressure steam is expanded adiabatically and reversibly through a well insulated turbine, which produces some shaft work. If the enthalpy change and entropy change across the turbine are represented by ΔH and ΔS respectively for this process ?
A. Δ H = 0 and ΔS = 0
B. Δ H ≠ 0 and ΔS = 0
C. Δ H ≠ 0 and ΔS ≠ 0
D. Δ H = 0 and ΔS ≠ 0
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 (∂P/∂V)s and the slope of the reversible isothermal line (∂P/∂V)T are related as (where, y = Cp/Cv) ?
A. (∂P/∂V)S = (∂P/∂V)T
B. (∂P/∂V)S = [(∂P/∂V)T]Y
C. (∂P/∂V)S = y(∂P/∂V)T
D. (∂P/∂V)S = 1/y(∂P/∂V)T
Pick out the wrong statement?
A. Cp of monatomic gases such as metallic vapor is about 5 kcal/kg.atom
B. The heat capacity of solid inorganic substance is exactly equal to the heat capacity of the
substance in the molten state
C. There is an increase in entropy, when a spontaneous change occurs in an isolated system
D. At absolute zero temperature, the heat capacity for many pure crystalline substances is zero
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