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The values of the ideal gas constant $(R)$ are given in the following table:

Values of the Universal Gas Constant

$R=8\mathrm{.}314J*mo{l}^{-1}*K^{-1}=8\mathrm{.}314m^3*Pa*mo{l}^{-1}*K^{-1}$

$=83\mathrm{.}14c{m}^3\frac{*}{b}ar*mo{l}^{-1}*K^{-1}=8314c{m}^3*kP{a}^{-1}*mo{l}^{-1}*K^{-1}$

$=82\mathrm{.}06c{m}^3*(atm)*mo{l}^{-1}{K}^{-1}=62,356c{m}^3*(torr)*mo{l}^{-1}*K^{-1}$

$=1\mathrm{.}987(cal)*mo{l}^{-1}*K^{-1}=1\mathrm{.}986(Btu)(lbmole{)}^{-1}(R{)}^{-1}$

$=0\mathrm{.}7302(ft{)}^3(atm)(lbmol{)}^{-1}(R{)}^{-1}=10\mathrm{.}73(ft{)}^3(a)(lbmol{)}^{-1}(R{)}^{-1}$

$=1545(ft)(l{b}_f)(lbmol{)}^{-1}(R{)}^{-1}$

Calculate compressibility $(Z)$ and the molar volume $(V$ for ammonia for the following condition. $($ For ammonia, $T_C=405\mathrm{.}7$

$K,P_C=112\mathrm{.}8$ bar, and $=0\mathrm{.}253.)$

Consider ammonia at $320K$ and $15$ bar and use the Peng$/$Robinson equation.

The molar volume is

$c{m}^3*mo{l}^{-1}.$

The compressibility is