a. The first step in the synthesis of trichloromethane (chloroform) from natural
ID: 541986 • Letter: A
Question
a. The first step in the synthesis of trichloromethane (chloroform) from natural gas (methane).
b. The final step in the industrial production of nitric acid.
Chemical Principles 7th Edition MHE/Freeman presented by Sapling Leaming Mapdot Calculate the equilibrium constant, K, at 25.0 °C for each of the following reactions. Use the thermodynamic information provided in the table Compoundl mot CH3CI(g) 48.50 CH4(g) C2Hzlg) 209.2 C2Hs9) Cl2(g) H2(g) H20(e) HCI(g) HNO3(aq)11125 NO(g) NO2g)51.31 a. The first step in the synthesis of trichloromethane (chloroform) from natural gas (methane) 50.72 n,(g) + Cl2(g) CH3Cl(g) + HCI(g) 32.82 0.00 0.00 Number 237.13 95.30 b. The final step in the industrial production of nitric acid 86.55 NumberExplanation / Answer
a)
Given:
Gof(CH4(g)) = -50.72 KJ/mol
Gof(Cl2(g)) = -0.0 KJ/mol
Gof(CH3Cl(g)) = 48.5 KJ/mol
Gof(HCl(g)) = -95.3 KJ/mol
Balanced chemical equation is:
CH4(g) + Cl2(g) ---> CH3Cl(g) + HCl(g)
Go rxn = 1*Gof(CH3Cl(g)) + 1*Gof(HCl(g)) - 1*Gof( CH4(g)) - 1*Gof(Cl2(g))
Go rxn = 1*(48.5) + 1*(-95.3) - 1*(-50.72) - 1*(-0.0)
Go rxn = 3.92 KJ/mol
T= 25.0 oC
= (25.0+273) K
= 298 K
G = 3.92 KJ/mol
G = 3920 J/mol
use:
G = -R*T*ln Kc
3920 = - 8.314*298.0* ln(Kc)
ln Kc = -1.5822
Kc = 0.2055
Answer: 0.2055
b)
Given:
Gof(NO2(g)) = 51.31 KJ/mol
Gof(H2O(l)) = -237.13 KJ/mol
Gof(HNO3(aq)) = -111.25 KJ/mol
Gof(NO(g)) = 86.55 KJ/mol
Balanced chemical equation is:
3 NO2(g) + H2O(l) ---> 2 HNO3(aq) + NO(g)
Go rxn = 2*Gof(HNO3(aq)) + 1*Gof(NO(g)) - 3*Gof( NO2(g)) - 1*Gof(H2O(l))
Go rxn = 2*(-111.25) + 1*(86.55) - 3*(51.31) - 1*(-237.13)
Go rxn = -52.75 KJ/mol
G = -52.75 KJ/mol
G = -52750 J/mol
use:
G = -R*T*ln Kc
-52750 = - 8.314*298.0* ln(Kc)
ln Kc = 21.291
Kc = 1.76*10^9
Answer: 1.76*10^9
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