Chemical Engineering - MCQ Practice Questions

Which of the following is NOT an extensive property?

According to the first law of thermodynamics, ΔU = Q - W. In this equation, W represents:

A system absorbs 500 J of heat and does 200 J of work. The change in internal energy is:

The compressibility factor Z for an ideal gas is:

In a constant pressure calorimeter, 1 kg of water is heated from 25°C to 75°C. Heat absorbed is approximately (Cₚ of water = 4.18 kJ/kg·K):

Which process is represented by a horizontal line on a T-S (Temperature-Entropy) diagram?

A gas mixture contains N₂ (40% mole) and O₂ (60% mole) at 1 atm and 298 K. Calculate the partial pressure of O₂ in the mixture.

The entropy change for an isothermal irreversible expansion of an ideal gas from V₁ to V₂ is:

Which of the following represents a state function?

For a closed system at constant volume, the first law of thermodynamics simplifies to:

The standard Gibbs free energy change (ΔG°) for a reaction at equilibrium is:

A heat engine operates between 600 K and 300 K. What is the maximum theoretical efficiency (Carnot efficiency)?

The equation of state for a real gas that considers molecular volume and intermolecular forces is:

A system undergoes a process where Q = 100 J and W = 60 J. The change in internal energy is:

A reversible adiabatic process is also known as:

The enthalpy change for a constant pressure process equals:

In a constant volume process, the heat added to the system equals:

A system absorbs 500 J of heat and does 200 J of work on surroundings. The change in internal energy is:

At constant temperature and pressure, which of the following represents the Gibbs free energy change for a spontaneous process?

The Clausius-Clapeyron equation relates vapor pressure to temperature. Which statement is correct?