Elements of Chemical Reaction Engineering, 7th Edition

B. Ideal Gas Constant and Conversion Factors

See www.onlineconversion.com.

Ideal Gas Constant

$\begin{array}{cclccc}R& =& {\displaystyle \frac{0.73{\text{\hspace{0.17em}ft}}^3\cdot \text{atm}}{\text{lb mol}\cdot °\text{R}}}& R& =& {\displaystyle \frac{1.987\text{\hspace{0.17em}\hspace{0.17em}Btu}}{\text{lb mol}\cdot °\text{R}}}\\ R& =& {\displaystyle \frac{8.314\text{\hspace{0.17em}kPa}\cdot {\text{dm}}^3}{\text{mol}\cdot \text{K}}}& R& =& {\displaystyle \frac{8.3144\text{\hspace{0.17em}J}}{\text{mol}\cdot \text{K}}}\\ R& =& 0.082{\displaystyle \frac{{\text{dm}}^3\cdot \text{atm}}{\text{mol}\cdot \text{K}}}={\displaystyle \frac{0.082{\text{\hspace{0.17em}m}}^3\cdot \text{atm}}{\text{kmol}\cdot \text{K}}}& R& =& {\displaystyle \frac{1.987\text{\hspace{0.17em}\hspace{0.17em}cal}}{\text{mol}\cdot \text{K}}}\end{array}$

$\begin{array}{ccl}{\text{Boltzmann’s constant\hspace{0.17em}\hspace{0.17em}}k}_{\text{B}}& =& 1.381\times {10}^{-23}{\displaystyle \frac{\text{J}}{\text{molecule}\cdot \text{K}}}\\ =& 1.381\times {10}^{-23}{\text{\hspace{0.17em}kg m}}^2/{\text{s}}^2/\text{molecule/K}\end{array}$

Volume of Ideal Gas

1 lb-mol of an ideal gas at 32°F and 1 atm occupies 359 ft³ (0.00279 lb-mol/ft³).

1 mol of an ideal gas at 0°C and 1 atm occupies 22.4 dm³ (0.0446 mol/dm³).

$C_{\text{A}}={\displaystyle \frac{P_{\text{A}}}{RT}}={\displaystyle \frac{y_{\text{A}}P}{RT}}$

where	CA = concentration of A, mol/dm3	T = temperature, K
	P = pressure, kPa	yA = mole fraction of A
	R = ideal gas constant, 8.314 kPa·dm3/ mol·K

1M = 1 molar = 1 mol/liter = 1 mol/dm³ = 1 kmol/m³ = 0.062 lb-mol/ft³

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