Intro to Chemical Engineering

🦫Intro to Chemical Engineering Unit 4 – Energy Balances

Energy balances are a fundamental concept in chemical engineering, applying the conservation of energy principle to analyze systems and processes. They involve accounting for all energy entering, leaving, and accumulating within a system, considering various forms like heat, work, and mass flow. Understanding energy balances is crucial for designing and optimizing real-world applications such as power plants, refrigeration cycles, and chemical reactors. Key concepts include the First Law of Thermodynamics, closed vs. open systems, and steady-state processes, which form the basis for solving complex engineering problems.

Key Concepts and Definitions

  • Energy the capacity to do work or transfer heat
  • Thermodynamics the study of energy and its transformations
  • System a specific region or quantity of matter under study
  • Surroundings everything external to the system
    • Can exchange energy and/or mass with the system
  • State variables properties that describe the state of a system (temperature, pressure, volume)
  • Process a change in the state of a system due to energy transfer or work
  • Equilibrium a state where no changes occur in the system properties over time
    • Thermal equilibrium: no temperature gradient
    • Mechanical equilibrium: no pressure gradient

Energy Balance Fundamentals

  • Conservation of energy principle energy cannot be created or destroyed, only converted from one form to another
  • Energy balance an accounting of all energy entering, leaving, and accumulating within a system
    • Applies the conservation of energy principle
  • Reference states chosen states for assigning a value of zero to a specific property (enthalpy, entropy)
  • Heat transfer energy transfer due to a temperature difference between the system and surroundings
    • Occurs through conduction, convection, or radiation
  • Work energy transfer due to a force acting over a distance
    • Includes expansion/compression work, shaft work, and electrical work
  • Internal energy a state function representing the total kinetic and potential energy of a system
  • Enthalpy a state function equal to the sum of internal energy and the product of pressure and volume (H=U+PVH = U + PV)

Types of Energy in Chemical Systems

  • Kinetic energy energy associated with the motion of an object (KE=12mv2KE = \frac{1}{2}mv^2)
  • Potential energy energy stored due to an object's position or configuration
    • Gravitational potential energy: PE=mghPE = mgh
    • Chemical potential energy: energy stored in chemical bonds
  • Thermal energy (heat) energy associated with the random motion of particles in a substance
  • Mechanical energy the sum of kinetic and potential energy in a system
  • Chemical energy energy stored in chemical bonds and released or absorbed during chemical reactions
  • Electrical energy energy associated with the flow of electric charges
  • Nuclear energy energy released during nuclear reactions (fission or fusion)

First Law of Thermodynamics

  • States that the change in internal energy of a system equals the heat added minus the work done by the system (ΔU=QW\Delta U = Q - W)
  • Applies the conservation of energy principle to thermodynamic systems
  • Heat (QQ) is positive when added to the system and negative when removed from the system
  • Work (WW) is positive when done by the system on the surroundings and negative when done on the system by the surroundings
  • For a cyclic process, the change in internal energy is zero (ΔU=0\Delta U = 0)
    • Heat added equals work done (Q=WQ = W)
  • Enthalpy change (ΔH\Delta H) is often used in place of internal energy change for processes at constant pressure

Closed vs. Open Systems

  • Closed system (control mass) a fixed amount of mass with no exchange of matter with the surroundings
    • May exchange energy (heat and work) with the surroundings
  • Open system (control volume) a region in space with mass flowing in and out
    • Exchanges both energy and mass with the surroundings
  • Isolated system does not exchange energy or mass with the surroundings
  • Adiabatic system does not exchange heat with the surroundings but may exchange work
  • Steady-state system has no change in properties over time (mass flow rates, temperatures, pressures remain constant)
    • Applicable to many open systems (heat exchangers, turbines, pumps)

Energy Balance Equations and Calculations

  • General energy balance equation: ΔU=QW+mi(hi+vi22+gzi)me(he+ve22+gze)\Delta U = Q - W + \sum m_i(h_i + \frac{v_i^2}{2} + gz_i) - \sum m_e(h_e + \frac{v_e^2}{2} + gz_e)
    • ΔU\Delta U: change in internal energy
    • QQ: heat added to the system
    • WW: work done by the system
    • mim_i, mem_e: mass flow rates in and out
    • hih_i, heh_e: specific enthalpies in and out
    • viv_i, vev_e: velocities in and out
    • ziz_i, zez_e: elevations in and out
  • Simplified energy balance for a closed system: ΔU=QW\Delta U = Q - W
  • Steady-state, steady-flow energy balance: 0=Q˙W˙+m˙i(hi+vi22+gzi)m˙e(he+ve22+gze)0 = \dot{Q} - \dot{W} + \sum \dot{m}_i(h_i + \frac{v_i^2}{2} + gz_i) - \sum \dot{m}_e(h_e + \frac{v_e^2}{2} + gz_e)
    • Q˙\dot{Q}, W˙\dot{W}, m˙\dot{m}: rates of heat, work, and mass flow
  • Enthalpy balance for a steady-state, steady-flow process: 0=Q˙W˙s+m˙ihim˙ehe0 = \dot{Q} - \dot{W}_s + \sum \dot{m}_ih_i - \sum \dot{m}_eh_e
    • W˙s\dot{W}_s: rate of shaft work

Real-World Applications

  • Power plants use energy balances to optimize efficiency and minimize waste heat
    • Boilers, turbines, condensers, and pumps are analyzed as open systems
  • Refrigeration cycles (air conditioners, refrigerators) rely on energy balances to calculate heat removal and work input
    • Evaporators, compressors, condensers, and expansion valves are treated as open systems
  • Heat exchangers (shell-and-tube, plate) are designed using energy balances to determine heat transfer rates and outlet temperatures
  • Chemical reactors (batch, continuous stirred-tank, plug-flow) use energy balances to account for heat of reaction and temperature changes
  • Distillation columns employ energy balances to calculate reboiler and condenser duties, as well as stage temperatures and compositions
  • Fuel cells and batteries are analyzed using energy balances to determine efficiency and power output

Common Pitfalls and Tips

  • Ensure consistent units throughout calculations (SI or English)
  • Pay attention to sign conventions for heat and work (positive or negative)
  • Clearly define the system and surroundings for each problem
  • Identify the type of system (closed, open, steady-state) to apply the appropriate energy balance equation
  • Account for all forms of energy entering and leaving the system (heat, work, mass flow)
  • Use reference states consistently when calculating changes in properties (enthalpy, entropy)
  • Double-check that the energy balance equation is satisfied (inputs = outputs + accumulation)
  • Simplify the energy balance equation when appropriate (neglect kinetic/potential energy, assume steady-state)


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© 2024 Fiveable Inc. All rights reserved.
AP® and SAT® are trademarks registered by the College Board, which is not affiliated with, and does not endorse this website.