The standard enthapy of formation of H2 is taken to be zero.
Hf(H2) =0
C2H4(g) + H2(g) -------> C2H6(g)
From Hess's law, Horxn = [ Hf(C2H6) ] - [ Hf(H2) + Hf(C2H4) ]
putting the values which is given in the question
Thus Horxn = -137.1 KJ
for the following rxn Use the standard enthalpies of formation to calculate AH° reaction. C2H4(g) +...
Use standard enthalpies of formation (in Appendix G in text) to calculate ∆H°rxn for each reaction. ∑ m∆H°f (products) - ∑n∆H°f (reactants), where m and n are coefficients. C2H4(g) + H2(g) ----- > C2H6(g) CO (g) + H2O (g) ----- > H2(g) + CO2(g) 3NO2(g) + H2O (l) ----- > 2HNO3(aq) + NO (g) 2SO2(g) + O2(g) -----------> 2SO3(g) 2C4H10 (g) + 13O2 (g) -----------> 8CO2 (g) + 10H2O (g) Substance --- ΔH° (kJ mol–) --- ΔG° (kJ mol–1) --- S°298 (J K–1 mol–1) C2H4 52.4 86.4 219.3 H2 0 0 130.7 C2H6 -84.0 -32.0 229.2 CO -110.52 -137.15 197.7 H2O -285.83 -237.1 70.0 CO2 -393.51 -394.36 213.8 NO2 33.2 51.30 240.1 NO 90.25 87.6 210.8 SO2 -296.83 -300.1 248.2 O2 0 0 205.2 SO3 -395.72 -371.06 256.76
Which of the following compounds when dissolved in water, would form an aqueous solution that would not conduct an electric current? Use the standard enthalpies of formation to calculate ΔH°rxn for the following reaction. C2H4( g) + H2(g) ⟶⟶ ⟶⟶ C2H6(g) ΔH°f Substance (kJ/mol) C2H4 52.4 C2H6 -84.68
2. Given the following heats of formation, calculate AH for the reaction 2 CO(g) + 5 H2(g) → C2H6 (g) + 2 H2O(g) Compound AH°F (kJ/mol) Compound AH°F (kJ/mol) 52.28 C₂H6 (8) -84.68 C2H4 (8) -393.5 CO2(g) -241.8 H2O(g) -285.9 CO(g) -110.5 H2O(1)
A 0.704 g of a pure acid, HA, is dissolved in water and an acid- base indicator added. The solution requires 33.78 mL of 0.256 M NaOH solution to reach the end point. What is the molar mass of the acid? HA(aq) + NaOH(aq) → NaA(aq) + H2O(aq) 145 g/mol 81.4 g/mol 20.0 g/mol 199 g/mol Based on the equation below, which is correct? 2 C2H2(g) + 5 O2(g) → 4 CO2(g) + 2 H2O(g) C2H2(g) is reduced O2(g) is...
For the reaction: H2(g)+C2H4(g)-->C2H6(g) Bond & Bond Enthalpy H-H 436.4 kJ/mole C-H 414 kJ/mol C-C 347 kJ/mol C=C 620 kJ/mol Substance & delta Hf H2 0 C2H4 52.3 C2H6 -84.7 (a) estimate the enthalpy of reaction, using the bond enthalpy values from the table in kJ/mol (b) Calculate the enthalpy of reaction, using standard enthalpies of formation
Calculate ΔH∘rxn for this reaction using standard enthalpies of formation. (The standard enthalpy of formation of gaseous propane is -103.9 kJ/mol
1).From the standard enthalpies of formation, calculate ΔH°rxn for the reaction C6H12(l) + 9O2(g) → 6CO2(g) + 6H2O(l) For C6H12(l), ΔH°f = –151.9 kJ/mol (5 points) Substance ∆H°f , kJ/mol C6H12(l) –151.9 O2(g) 0 H2O(l) –285.8 CO2(g) –393.5 2).Determine the amount of heat (in kJ) given off when 1.26 × 104 g of ammonia are produced according to the equation N2(g) + 3H2(g) → 2NH3(g) ΔH°= –92.6 kJ/mol Assume that the reaction takes place under standard conditions at 25oC.
eedback Watch KCV Part A for the reaction: Use standard enthalpies of formation to determine AH Fe2O3(s) + 3 CO(g) + 2 Fe(s) + 3 CO2(g) -24.8 kJ 541.2 kJ -2336 kJ -541.2 kJ Submit Request Answer Provide Feedback emistry.com/myetter View assignment ProblemiD-133941 - 289) ; Watch WE 7.9 Part A What is AH for the reaction 2 B + 3 C? Ο ΔΗ, + ΔΗ, Ο ΔΗΩ – ΔΗ Ο ΔΗ - ΔΗ Ο 2 x (ΔΗ, + ΔΗ,)...
PART A. Use standard enthalpies of formation to calculate ΔH∘rxn for the following reaction: C2H5OH(l)+3O2(g)→2CO2(g)+3H2O(g) Express your answer using four significant figures. PART B. Use standard enthalpies of formation to calculate ΔH∘rxn for the following reaction: CH4(g)+2O2(g)→CO2(g)+2H2O(g) Express your answer using three significant figures. PART C. Use standard enthalpies of formation to calculate ΔH∘rxn for the following reaction: C(s)+O2(g)→CO2(g) Express your answer using four significant figures. PART D. Use standard enthalpies of formation to calculate ΔH∘rxn for the following reaction:...
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)...