For the reaction, CaCO 3( g ) leftharpoons CaO ( s )+ CO 2( g ) partial pressure of CO 2 at 1000 K is 0.003 atm . Δ G°=27.2 kcal. Calculate the value of Δ G.

Question

For the reaction, CaCO 3( g ) leftharpoons CaO ( s )+ CO 2( g ) partial pressure of CO 2 at 1000 K is 0.003 atm . Δ G°=27.2 kcal. Calculate the value of Δ G. (A) 12.6 kcal (B) 15.6 kcal (C) 13.4 kcal (D) 14.2 kcal

Tardigrade Admin · Accepted Answer

CaCO 3( g ) leftharpoons CaO ( s )+ CO 2( g ) Kp =pCO2 =0.003 atm ΔG = ΔG° + 2.303 RT logKp = 27200 + 2.303 × 2 × 1000 × log 0.003 = 15.6 kcal. (R = 2 cal mol-1 K-1)

Q. For the reaction, $C a C O_{3 (g)} ⇌ C a O_{(s)} + C O_{2 (g)}$ partial pressure of $C O_{2}$ at $1000 K$ is $0.003 a t m .Δ G^{\circ} = 27.2 k c a l$ . Calculate the value of $Δ G$ .

$12.6 k c a l$

$15.6 k c a l$

$13.4 k c a l$

$14.2 k c a l$

$C a C O_{3 (g)} ⇌ C a O_{(s)} + C O_{2 (g)}$
$K_{p} = p_{C} O_{2} = 0.003$ atm
$Δ G = Δ G^{°} + 2.303 RT l o g K_{p}$
$= 27200 + 2.303 \times 2 \times 1000 \times l o g 0.003$
$= 15.6 k c a l . (R = 2 c a l m o l^{- 1} K^{- 1})$

Q. For the reaction, CaCO3(g)​⇌CaO(s)​+CO2(g)​ partial pressure of CO2​ at 1000K is 0.003atm.ΔG∘=27.2kcal. Calculate the value of ΔG.

12.6kcal

15.6kcal

13.4kcal

14.2kcal