### Flow Rate

#### Standard to Actual: Gas Flow

${\frac{{\mathrm{ft}}^{3}}{\mathrm{hr}}}_{\left[S\right]}={\frac{{\mathrm{ft}}^{3}}{\mathrm{hr}}}_{\left[A\right]}×\frac{520}{T+460}×\frac{P+14.7}{14.7}$

$T=\text{Temperature}\phantom{\rule{5px}{0ex}}\left[°\mathrm{F\right]}\phantom{\rule{0ex}{0ex}}P=\text{Pressure}\phantom{\rule{5px}{0ex}}\mathrm{\left[psig\right]}$

### Pressure

$P=\frac{\mathrm{SG}×H}{2.31}$

### Viscosity

$\gamma =\frac{\Phi }{\mathrm{SG}}$

$\gamma =\text{Kinematic Viscosity}\phantom{\rule{5px}{0ex}}\mathrm{\left[cSt\right]}\phantom{\rule{0ex}{0ex}}\Phi =\text{Dynamic Viscosity}\phantom{\rule{5px}{0ex}}\mathrm{\left[cP\right]}\phantom{\rule{0ex}{0ex}}\mathrm{SG}=\text{Specific Gravity}$

### API

$\mathrm{API}=\left(\frac{141.5}{\mathrm{SG}}\right)-131.5$

### Partial Pressure

The Product of the total pressure P, of the gas, times the mole fraction of that species y(i) in the gas.

Raoult's Law

The partial vapor pressure of each component of an ideal mixture of liquids is equal to the vapor pressure of the pure component multiplied by its mole fraction in the mixture.

For a single component in an ideal solution:

### General Reference

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