Q2. Balanced reaction :
2 CO (g) + 5 H2 (g) C2H6 (g) + 2 H2O (g)
enthalpy of reaction, H = enthalpy of formation of products - enthalpy of formation of reactants
H = Ho f (products) - Ho f (reactants)
H = [Ho f C2H6 (g) + 2 * Ho f H2O (g)] - [2 * Ho f CO (g) + 5 * Ho f H2 (g)]
H = [(-84.68 kJ/mol) + 2 * (-241.8 kJ/mol)] - [2 * (-110.5 kJ/mol) + 5 * (0)]
H = -84.68 kJ - 483.6 kJ + 221 kJ
H = -347.28 kJ
2. Given the following heats of formation, calculate AH for the reaction 2 CO(g) + 5...
5. Using standard heats of formation, calculate AH for 4 FeO (s) + O2(g) → 2 Fe2O3 (s) AH1 of FeO (s) = -272.0 kJ/mol AHºf of Fe2O3 (s) = -825.5 kJ/mol 3. Given 3 C (s) + 4 H2(g) → C3H8 (9) AH = -103.85 kJ/mol C(s) + O2(g) + CO2(g) AH = -393.5 kJ/mol H2 (g) + 12 O2(g) → H2O (1) AH = -285.8 kJ/mol find AH for C3H8 (g) + 5 O2(g) → 3 CO2 (g)...
1. Find the heat of combustion of liquid toluene (C6H5-CH3) Table of Heats of Formation Substance AHP (kJ/mole) 716.7 CIB) C graphite) C(diamond) CH4(8) C2H2(g) C2H4(8) C2H618) C6H6(e) CHg(e) OIB) 0318) CO2(aq) CO2(g) CO(R) HB) 1.895 -74.81 226.73 52.26 -84.68 49.04 50.0 249.2 143.0 -412.9 -393.5 -110.5 217.9 -241.8 -285.8 -272.0 -825.5 -1121.0 H2O(g) H20le) Fe(s) Fe2O3(s) Fe30413)
for the following rxn Use the standard enthalpies of formation to calculate AH° reaction. C2H4(g) + H2(g) + C2H6(g) ΔΗ° Substance (kJ/mol) C₂H4 52.4 C2H6 -84.68 0 -32.3 kJ -4.3 x 103 kJ 32.3 kJ 0 -137.1 kJ
Practice with Hess's Law and Standard Heats of Formation 1. (Example) The reaction C2H4 (g) + 6 F2 (g) → 2 CF4(g) + 4 HF (g) can be written as the sum of: C2H4 (9) ► 2 C(s) + 2 H2 (g) AH = -52.3 kJ/mol 2 C(s) + 4 F2 (9) ► 2 CF4(9) AH = -1360 kJ/mol 2 H2(g) + 2 F2 (g) → 4 HF (a) AH = -1074 kJ/mol C2H4(g) + 6 F2(g) → 2 CF4(g)...
C Using the heats of formation below, calculate the heat of reaction for the following reaction: CH4(g) + H2O(g) → C2H5OH(E) AH® (kJ/mol) C2H4(g) 52.26 H2O(g) -241.8 C2H5OH(E) -235.1 kJ d Using the heats of formation below, calculate the heat of reaction for the following reaction: Fe2O3(s) + 2Al(s) - A1203(s) + 2Fe(s) AH(kJ/mol) Fe2O3(s) -824.2 Al(s) 0 Al2O3(s) -1676 Fe(s) 0 KJ
Using the standard heats of formation that follow, calculate the standard enthalpy change for the following reaction. Species ΔΗΡ(kJ/mol) CO2(g) -393.5 C2H2(g) 226.7 H2O(g)241.8
7. Consider the following reaction: H,(8)+CO,(8)=1,0(g)+CO(g) The value of the equilibrium constant K, for the reaction is 0.534 at 700°C. What is the value of K, for this reaction at 298 K? (5 points) (AH; (H20) = -241.8, AH;(CO) = -110.5, AH;(CO2) = -393.5 kJ/mol)
6. Calculate the standard enthal py change for the reaction: CO (g) + H20(g) CO2 (g) + H2 (g) CO (g) H20 (g) CO2 (g) H2 (g) = -110.5 kJ/mol -241.8 kJ/mol -393.5 kJ/mol O kJ/mol 11 a. +41.2 kJ b.-41.2 kJ c. +82.4 kJ d. -82.4 kJ
a Using the heats of formation below, calculate the heat of reaction for the following reaction: C2H2(g) + 5/202(2)→ 2C02() +H20() AH® (kJ/mol) C2H2(g) 226.7 O2(g) 0 CO2(g) -393.5 H20(-285.8 kJ Submit b Using the heats of formation below. calculate the heat of reaction for the following reaction: PC13(2) + Cl2(2)→ PC15(e) AH(kJ/mol) PC13(g) -306.4 Cl2(E) 0 PC1s() -398.9
Practice with Hess's Law and Standard Heats of Formation 1. (Example) The reaction C He(g) + 6 F2 (g) → 2 CF4(g) + 4 HF (9) can be written as the sum of: CH4 (9) ► 2 C(s) + 2 Ha(o) AH = -52.3 kJ/mol 2 C(s) + 4 Faq) → 2 CF4g) SH -1380 kJ/mol 2 Haq) + 2 Fala) > 4 HF HE.1074 kJimol CsHe(g) + 6 F2 (g) → 2 CF.(g) + 4 HF (g) AH =...