Mixing and Solution: Screencast
Illustrates the changes in state variables (V, H, U, S, G) when ideal solutions form.
We suggest that after watching this screencast, you list the important points as a way to increase retention.
Describes how to use a diagram of enthalpy versus weight percent for a binary mixture to determine the final temperature when mixing is adiabatic.
We suggest that after watching this screencast, you list the important points as a way to increase retention.
Important Equations:
For an ideal solution
\[H = x_AH_A + x_BH_B\]
where \(H\) = enthalpy (kJ/mol) of the binary solution,
\(x_A\) and \(x_B\) are mole fractions of the two components,
\(H_A\) and \(H_B\) are the molar enthalpies (kJ/mol) of the pure components at the same temperature of the solution.
A non-ideal solution can be represented as
\[H = x_AH_A + x_BH_B + \alpha x_Ax_B\]
where \(\alpha\) is a non-ideal parameter.
\[\Delta H_{mix} = H – x_AH_A + x_BH_B\]
where \(\Delta H_{mix}\) = heat of mixing at constant temperature.
For dissolving a solute in a solvent
\[\Delta H_{mix} = H_{solution} – H_{solute} – H_{solvent}\]
\[x_i \gamma _i P_i ^{sat} = y_iP\]
where \(x_i\) = liquid-phase mole fraction of component \(i\)
\(\gamma _i\) = activity coefficient of component \(i\)
\(P_i ^{sat}\) = saturation pressure of component \(i\)
\(y_i\) = vapor-phase mole fraction of component \(i\)
\(P\) = pressure.