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Estimate the entropy change of vaporization of benzene at $50C.$ The vapor pressure of benzene is given by the equation

$ln\frac{P^{\text{s}\text{a}\text{t}}}{k}PA=13\mathrm{.}8858-\frac{2788\mathrm{.}51}{tC+220\mathrm{.}79}$

The values of $R$ are given in the table below.

Values of the Universal Gas Constant

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

$=83\mathrm{.}14c{m}^3*$ bar $*mo{l}^{-1}*K^{-1}=8314c{m}^3*kPa*mo{l}^{-1}*K^{-1}$

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

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

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

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

Use the following condition to calculate $V^{lv}.$

Consider the Clausius$/$Clapeyron equation.

The entropy change of vaporization of benzene is

$J*mo{l}^{-1}*K^{-1}$