Titanium(IV) oxide is converted to titanium carbide with carbon at a high temperature.
Calculate ΔrG° and K at 891°C.
1)
Given:
Gof(TiO2(s)) = -728.24 KJ/mol
Gof(C(s)) = 0.0 KJ/mol
Gof(CO(g)) = -214.92 KJ/mol
Gof(TiC(s)) = -159.09 KJ/mol
Balanced chemical equation is:
TiO2(s) + 3 C(s) ---> 2 CO(g) + TiC(s)
ΔGo rxn = 2*Gof(CO(g)) + 1*Gof(TiC(s)) - 1*Gof( TiO2(s)) - 3*Gof(C(s))
ΔGo rxn = 2*(-214.92) + 1*(-159.09) - 1*(-728.24) - 3*(0.0)
ΔGo rxn = 139.31 KJ
Answer: 139.31 KJ
2)
T= 891.0 oC
= (891.0+273) K
= 1164 K
ΔGo = 139.31 KJ/mol
ΔGo = 139310 J/mol
use:
ΔGo = -R*T*ln Kc
139310 = - 8.314*1164.0* ln(Kc)
ln Kc = -14.3953
Kc = 5.60*10^-7
Answer: 5.60*10^-7
Titanium(IV) oxide is converted to titanium carbide with carbon at a high temperature. Calculate ΔrG° and...
Can somebody help me solve this?? Titanium (IV) oxide is converted to titanium carbide with carbon at high temperature. TiO2(s) + 3 C(s) --> 2 CO(g) + TiC(s) compound free energies of formation at 727°C, kJ/mol TiO2(s) -757.8 TiC(s) - 162.6 -200.2 CO(g) Calculate K
Titanium oxide (TiO2) is reduced by carbon to form titanium metal and carbon monoxide (CO). If 5.00g of TiO2 is reacted with 10.0 g of C, which reactant is the limiting reagent?
Calcium carbide (CaC) is manufactured by the reaction of CaO with carbon at a high temperature (calcium carbide is then used to make acetylene): CaO (s)+3C (s) + CaC2 (s)+CO (g) AH =+464.8 kJ mol- Is this reaction endothermic or exothermic? If 10.0 g of CaO is allowed to react with an excess of carbon, how much heat is absorbed or evolved by the reaction?
Calcium carbide, CaC2, is manufactured by the reaction of CaO with carbon at a high temperature. CaO (s) + 3 C (s) → CaC2 (s) + CO (g) Hrxn = –464.8 kJ a) Is the reaction endothermic or exothermic? Do the reactants or products have more energy? b) If 10.0 g carbon is allowed to react with an excess of CaO, what quantity of heat is absorbed or evolved by the reaction? c) If 45.0 L of CO at 1.70...
5. The first step in the commercial production of titanium metal is the reaction of TiO2 with chlorine an graphite: TiO2 (s) + 2 Clz (g) + 2 C(s) TiCl4 (1) + 2 CO (g) Calculate AGⓇ for the reaction. Substance AG? (kJ/mol Substance AG® (kJ/mol) C() 0 TiCl4 (1) -804.2 CO(g) -110.5 TiO2 (s) -944.0 121.3 Cl2 (g)
5. The first step in the commercial production of titanium metal is the reaction of TiO2 with chlorine and graphite: TiO2 (s) + 2 Cl2 (g) + 2 C(s) TiCl4 (1) + 2 CO (g) Calculate AGº for the reaction. Substance AG? (kJ/mol) Substance AG (kJ/mol) C(s) 0 TiCl4 (1) -804.2 CO (g) -110.5 TiO2 (s) -944.0 Cl2 (8) 121.3
Calculate the standard free-energy change at 25°C for the reduction of iron (III) oxide with carbon monoxide: Fe,0,(s) + 3 CO(g) → 2 Fe(s) + 3 CO2(g) AG®(Fe,0,) = -742.2 kJ/mol AG (CO) = -137.2 kJ/mol AG® (CO2) = -394.4 kJ/mol
AH-116.4 kJ/mol 4. Consider the following reaction: NH.NO, (s) N20 (8) + 2 H20 (g) Calculate AGⓇ for the reaction. Substance S” (J/mol K) NH.NO, (3) 151 N:0 (8) 220 H:0 (9) 183 5. The first step in the commercial production of titanium metal is the reaction of Tio: with chlorine an graphite: TiO2 (s) + 2 Cl: (g) + 2C (5) Tici: (1) + 2 CO(g) Calculate AGº for the reaction. Substance AG? (kJ/mol Substance AG® (kJ/mol) C(s) TiCl...
2. (a) Rutile, the high-temperature form of titanium oxide, TiO2, adopts a tetragonal P structure with a 4.59 Å and c 2.96 Å Calculate the separation between the planes with the Miller indices (11). 110 (b) When radiation of wavelength 495 nm from a monochromatic flash lamp of power 0.500 kW is used to irradiate a low-pressure sample of iodine vapour, I2, the rate of production of iodine atoms is 3.24 x 1019 s 1. Assuming that all of the...
The first step in the commercial production of titanium metal is the reaction of rutile (TiO2) with chlorine and graphite: TiO2(s) + 2Cl2(g) + 2C (s) TiCl4(l) + 2CO (g) Use the following data to calculate Keq for this reaction at 25° C. Formula ?H°f (KJ/mol) S° (J/K mol) TiO2(s) -944.0 50.6 Cl2(g) 0 223.0 C (s) 0 5.7 TiCl4(l) -804.2 252.3 CO (g) -110.5 197.6