CPE553 Chemical Engineering Thermodynamics UITM Assignment Sample Malaysia

CPE553 Chemical Engineering Thermodynamics at UITM focuses on the fundamental principles of chemical engineering thermodynamics. The course covers topics such as thermodynamics of mixtures, vapor-liquid equilibria, and chemical reaction equilibria. 

Students learn to apply these equilibrium concepts to various chemical engineering processes. The course provides a comprehensive understanding of thermodynamics and its practical applications in the field of chemical engineering.

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Assignment Task 1: Determine the bubble point and dew point as well as composition at equilibrium.

In the context of thermodynamics and phase behavior of a mixture, determining the bubble point and dew point involves finding the conditions at which vapor and liquid phases coexist in equilibrium.

Bubble Point:

• The bubble point is the temperature and pressure at which the first bubble of vapor appears in a liquid mixture. It represents the starting point of vaporization.
• To calculate the bubble point, you need to solve the phase equilibrium equations for the given system. These equations often involve the use of phase diagrams, Raoult’s law, and other relevant thermodynamic models.

Dew Point:

• The dew point is the temperature and pressure at which the first drop of liquid forms in a vapor mixture. It signifies the beginning of condensation.
• Similar to the bubble point, the dew point is determined by solving the phase equilibrium equations. This may involve the use of the phase diagrams, Antoine’s equation, and other relevant thermodynamic models.

Composition at Equilibrium:

• At the bubble point and dew point, the compositions of the vapor and liquid phases are in equilibrium. The composition at equilibrium can be found by evaluating the concentrations of each component in both phases using mass or mole balances.
• Raoult’s law and the concept of partial pressures are often used to calculate the vapor and liquid phase compositions.

Remember, the specific methodology and equations used for these calculations depend on the nature of the mixture, the thermodynamic model chosen, and the available data. It’s advisable to refer to your course materials, textbooks, or relevant literature for specific details and equations tailored to your system.

Assignment Task 2: Interpret experimental data and select the appropriate models to calculate the phase equilibria thermodynamic properties of a specific mixture.

Interpreting experimental data and selecting appropriate models for calculating phase equilibria thermodynamic properties of a specific mixture is a crucial aspect of chemical engineering and thermodynamics. Here is a step-by-step guide for Task 2:

Data Interpretation:

• Begin by thoroughly analyzing the experimental data you have. This data may include temperature, pressure, and composition measurements at different conditions.
• Identify trends, patterns, and anomalies in the data to understand the behavior of the mixture.

System Characterization:

• Understand the nature of the mixture: Is it an ideal solution, non-ideal solution, azeotropic, etc.? This knowledge will guide your choice of thermodynamic models.

Model Selection:

• Choose appropriate thermodynamic models based on the characteristics of the mixture. Common models include the Ideal Gas Law, Raoult’s Law, Henry’s Law, Van der Waals equation, and various activity coefficient models (Wilson, NRTL, UNIQUAC, etc.).
• If the mixture shows non-ideal behavior, consider models that account for deviations from ideality.

Phase Equilibrium Calculations:

• Implement the selected models to calculate phase equilibrium properties such as bubble point, dew point, vapor-liquid equilibrium, and fugacity coefficients.
• Depending on the complexity of the system, iterative methods or advanced numerical techniques may be needed.

Model Validation:

• Validate the selected models by comparing the calculated results with the experimental data. Assess the accuracy and reliability of the models in predicting phase behavior.
• Adjust model parameters if needed to improve the agreement between experimental and calculated values.

Sensitivity Analysis:

• Perform sensitivity analyses to understand how changes in model parameters affect the calculated properties. This helps in assessing the robustness of the chosen models.

Documentation:

• Clearly document the models selected, parameters used, and the methodology employed in your calculations. This documentation is crucial for reproducibility and future reference.

Remember that the choice of models and methods may vary based on the specific characteristics of the mixture and the available experimental data. Consult relevant literature and textbooks for guidance, and consider seeking assistance from instructors or experts if needed.

Assignment Task 3: Predict the equilibrium products and their concentration involving with chemical reactions system.

Predicting the equilibrium products and their concentrations in a chemical reaction system involves applying principles of chemical thermodynamics and reaction kinetics. Here’s a guide for Task 3:

Chemical Reaction Equations:

• Begin by writing down the balanced chemical equations that represent the reactions occurring in the system.
• Make sure the equations are properly balanced in terms of mass and charge.

Determine Reaction Quotient (Q):

• Calculate the initial reaction quotient, Q, using the initial concentrations of reactants and products. This is similar to the equilibrium constant expression but evaluated at the initial conditions.

Equilibrium Constant (K):

• Identify the equilibrium constant, K, for each reaction. K is a ratio of the concentrations of products to reactants at equilibrium.
• Use known thermodynamic data or experimental values to determine equilibrium constants.

Reaction Quotient vs. Equilibrium Constant:

• Compare the initial reaction quotient (Q) with the equilibrium constant (K).
• If Q is not equal to K, the system is not at equilibrium. Use this information to predict the direction in which the reaction will proceed.

Determine Reaction Shift:

• Apply Le Chatelier’s Principle to predict the direction in which the reaction will shift to reach equilibrium. This involves considering the effect of changes in concentration, temperature, and pressure on the equilibrium position.

Equilibrium Concentrations:

• Calculate the concentrations of reactants and products at equilibrium using the reaction quotient and the known equilibrium constant.
• Depending on the complexity of the system, you may need to solve a system of nonlinear equations.

Consideration of Reaction Kinetics:

• If the reactions are not instantaneous, consider the kinetics of the reactions. Reaction rates and the time required to reach equilibrium can impact the final concentrations.

Temperature and Pressure Effects:

• Be mindful of the impact of temperature and pressure changes on the equilibrium constants. The Van’t Hoff equation can be useful for predicting how equilibrium constants change with temperature.

Validation:

• Compare your predicted equilibrium concentrations with experimental data or literature values to validate your predictions.

Remember that predicting equilibrium concentrations involves a combination of thermodynamic principles and a good understanding of reaction kinetics. Consider the specifics of your system and the reactions involved when applying these principles. If the system is complex, computer software and simulation tools may be helpful in performing detailed calculations.

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