One mole of liquid CCl 4 at 298 K has an entropy of 214 J / K. What is the entropy of one mole of CCl 4 vapours in equilibrium with the liquid at this temperature, if heat of vapourization of CCl 4 is 43.0 kJ / mol ?

Question

One mole of liquid CCl 4 at 298 K has an entropy of 214 J / K. What is the entropy of one mole of CCl 4 vapours in equilibrium with the liquid at this temperature, if heat of vapourization of CCl 4 is 43.0 kJ / mol ? (A) 358.3 J / K (B) 69.7 J / K (C) 144.3 J / K (D) 214 J / K

Tardigrade Admin · Accepted Answer

CCl 4(l) arrow CCl 4(g) ; Δ H=43.0 kJ =43 × 103 J Δ S=(Δ H text vap /T)=(43 × 103/298)=144.3 J We know Δ S=S text vap -S text liq ⇒ 144.3=S text vap -214 S text vap =144.3+214=358.3 J K -1 mol -1

Q. One mole of liquid $CC l_{4}$ at $298 K$ has an entropy of $214 J / K$ . What is the entropy of one mole of $CC l_{4}$ vapours in equilibrium with the liquid at this temperature, if heat of vapourization of $CC l_{4}$ is $43.0 k J / m o l ?$

$358.3 J / K$

$69.7 J / K$

$144.3 J / K$

$214 J / K$

$CC l_{4 (l)} \to CC l_{4 (g)}; Δ H = 43.0 k J = 43 \times 1 0^{3} J$

$Δ S = \frac{Δ H _{vap}}{T} = \frac{43 \times 1 0 ^{3}}{298} = 144.3 J$

We know $Δ S = S_{vap} - S_{liq}$

$\Rightarrow 144.3 = S_{vap} - 214$

$S_{vap} = 144.3 + 214 = 358.3 J K^{- 1} m o l^{- 1}$

Q. One mole of liquid CCl4​ at 298K has an entropy of 214J/K. What is the entropy of one mole of CCl4​ vapours in equilibrium with the liquid at this temperature, if heat of vapourization of CCl4​ is 43.0kJ/mol?

358.3J/K

69.7J/K

144.3J/K

214J/K