Chemical Engineering Thermodynamics

401. The partial molar enthalpy of a component in an ideal binary gas mixture of composition Z, at a temperature T and pressure P, is a function only of

1. T
2. T and P
3. T, P and Z
4. T and Z

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402. The partial pressure of each constituent present in an alloy is _________ the total vapor ressure exerted by the alloy.

1. Less than
2. Equal to
3. More than
4. Either (B) or (C); depends on the type of alloy

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403. The point at which all the three (solid, liquid and gas) phases co-exist, is known as the _________ point.

1. Freezing
2. Triple
3. Boiling
4. Boyle

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404. The principle applied in liquefaction of gases is

1. Adiabatic expansion
2. Joule-Thomson effect
3. Both (A) and (B)
4. Neither (A) nor (B)

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405. The quantitative effect of temperature on chemical equilibrium is given by the

1. Van’t-Hoff equation
2. Le-Chatelier's principle
3. Arrhenius equation
4. None of these

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406. The rate at which a substance reacts is proportional to its active mass and the rate of a chemical reaction is proportional to the product of active masses of the reacting substances. This is the

1. Lewis-Randall rule
2. Statement of Van't Hoff Equation
3. Le-Chatelier's principle
4. None of these

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407. The ratio of equilibrium constants (Kp2/Kp1) at two different temperatures is given by

1. (R/ΔH) (1/T₁ - 1/T₂)
2. (ΔH/R) (1/T₁ - 1/T₂)
3. (ΔH/R) (1/T₂ - 1/T₁)
4. (1/R) (1/T₁ - 1/T₂)

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408. The reaction A (l) → R(g) is allowed to reach equilibrium conditions in an autoclave. At equilibrium, there are two phases, one a pure liquid phase of A and the other a vapor phase of A, R and S. Initially A alone is present. The numbers of degrees of freedom are:

1. 1
2. 2
3. 3
4. 0

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409. The relation connecting the fugacities of various components in a solution with one another and to composition at constant temperature and pressure is called the _________ equation.

1. Gibbs-Duhem
2. Van Laar
3. Gibbs-Helmholtz
4. Margules

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410. The root mean square speed of molecules of a gas is equal to (where, m = mass of the molecule K = Boltzmann‟s constant, T = absolute temperature)

1. √(2KT/m)
2. √(3KT/m)
3. √(6KT/m)
4. 3KT/m

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