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58 Cards in this Set
- Front
- Back
In steady flow |
Velocity is not a function of time |
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In unsteady flow |
Velocity is a function of time |
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In inviscud flow |
Fluid has no viscosity No energy loss from friction between molecules |
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In viscous flow |
Fluid is viscous Has frictional losses |
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Reynolds number in terms of rotational speed |
=rho x N x D^2 /mu As u = N D N is rotational speed and D the diameter of propeller |
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Homogenous system |
Either has constant properties or properties vary continuously |
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Heterogenous system d |
More than one homogenous system Phases separated by physical boundary or discontinuity |
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Define isolated clise |
No mass or energy flow |
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Define closed |
Energy flow but no mass flow |
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Define open |
Define both mass and energy flow (by heat and work) |
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Adiabatic |
No heat flow in or out |
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5 properties of matter |
Volume, pressure, temp, internal energy, entropy |
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3 derived properties |
Enthalpy H Helmholtz free energy A Gibbs free energy G |
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Extensive property |
Depends on the amount |
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Intensive property |
Doesn’t |
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Z |
Thermodynamic variable Extensive |
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Zm |
Molar property |
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State function |
Difference between two values regardless of path |
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Maxwell Relation |
Back (Definition) |
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State function definition |
Back (Definition) |
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Use of Maxwell Relation |
To prove a function is a state function |
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how to use Maxwells relation |
Let M equal what’s in front of do Let N equal what’s in front of dy Diff M in respect to Y with constant x Diff N in respect to X with constant y If values equal, sf |
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U = |
= q + w |
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Formula for heat, q |
= integral dq =integral C dT Where cp may equal a polynomial of T to integrate |
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H = |
U + pV |
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dq = For isochoric vs isobaric |
Isochoric =dU Isobaric = dH |
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To demonstrate cv=(dq/dT)v =(dU/dt)v |
Use u=f(V,T) and dU=(dU/dV)T dv + (dU/dT)V dT Divide it by dT at a constant v Simplify as (dv/dt)v is 0 and (dT/dT)v is 1 |
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Define 2nd law |
Entropy of universe increases to a max |
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dU = (sf) |
dq + dw heat and work - not sf so not exact differentials |
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Isochoric P V graph |
Constant volume |
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Isothermal P V graph |
Back (Definition) |
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Reversible work formula |
Back (Definition) |
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Work done BY system |
Is negative |
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For heat |
Signs are opposite |
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Isochoric P V graph |
Constant volume |
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To demonstrate cv=(dq/dT)v =(dU/dt)v |
Use u=f(V,T) and dU=(dU/dV)T dv + (dU/dT)V dT Divide it by dT at a constant v Simplify as (dv/dt)v is 0 and (dT/dT)v is 1 |
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Reversible work formula |
Back (Definition) |
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Kelli temp and calculating entropy change |
Back (Definition) |
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Definition of fugacity |
Back (Definition) |
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Reversible isothermal expansion of ideal gas And reversible adiabatic expansion |
Back (Definition) |
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Unit of fugacity |
Same as pressure |
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Fugacity co efficient |
Ratio f/p |
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Chemical potential |
Back (Definition) |
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Relationships |
Back (Definition) |
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Vm is |
Gas molar volume |
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Vm ideal is |
Molar volume of gas behaving ideally at same t and p |
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De |
Back (Definition) |
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Definition of fugacity |
Back (Definition) |
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f in terms of p |
Back (Definition) |
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Reversible isothermal expansion of ideal gas And reversible adiabatic expansion |
Back (Definition) |
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Fugacity co efficient |
Ratio f/p |
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To calculate delta U S H and G |
Find value in table Differentiate ideal eq and combine equations For G use other eq LOOK IN BOOK CH3 IF J BEVAN OTT J CHEMICAL THERMODYNAMIC PRINCIPLES AND APPLICATIONS |
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Chemical potential |
Back (Definition) |
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Relationships |
Back (Definition) |
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Gibbs Phase rule |
f = c - p + 2 where c is no of independent components P is no of phases F is degree of freedom |
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Fugacity |
measure of flow of mass in chemical process Can be used to determine point of equil |
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Example of equation of state and alpha from data pVm = RT + Bp + cp^2 + Dp^3 ... |
Divide Vm by p Vm ideal = RT/p So calculate alpha |
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Fugacity for pure condensed phases |
Back (Definition) |