Answer:
Given chemical equation is
C2H6(g) + O2(g) -------> CO2(g) + H2O(g)
The balanced chemical equation is
2C2H6(g) + 7O2(g) -------> 4CO2(g) + 6H2O(g)
ΔHrxn=Σ n x ΔHof products - Σ m x ΔHof reactants
where n=number of moles of products and m=number of moles of reactants
ΔHrxn= [(4 mol x ΔHof CO2(g)) + (6 mol x ΔHof H2O(g))] - [(2 mol x ΔHof C2H6(g)) + (7 mol x ΔHof O2(g))]
ΔHof C2H6(g)= -84.667 kJ/mol
ΔHof O2(g)= 0 kJ/mol
ΔHof CO2(g)=-393.5 kJ/mol
ΔHof H2O(g)=-241.826 kJ/mol
ΔHrxn= [(4 mol x -393.5 kJ/mol) + (6 mol x -241.826 kJ/mol)] - [(2 mol x -84.667 kJ/mol) + (7 mol x 0 kJ/mol)]
ΔHrxn=-2855.622 kJ.
llicients. (unbalanced] C2H6(8) + O2(8) — CO2(g) + H2O(g) V C2H6()] = -84.667 kJ/mol Ah (CO2())...
Calculate AH° for the following reaction, after it is properly balanced with smallest whole-number rxn coefficients: CzHg(8) +026) - C026) + H20(8) ſunbalanced] ſunbalanced] AH (C2H5)] = -84.667 kJ/mol 14° (CO26)= 393.5 kJ/mol AH [CO2(aq)] =-412.9 kJ/mol AH (4,0()] = –241.826 kJ/mol AH H200)] = -285.840 kJ/mol DkJ
The combustion reaction of ethane is as follows. C2H6(g) + 7/2 O2(g) → 2 CO2(g) + 3 H2O(l) Using Hess's law and the reaction enthalpies given below, find the change in enthalpy for this reaction. reaction (1): C(s) + O2(g) → CO2(g) ΔH = −393.5 kJ/mol reaction (2): H2(g) + 1/2 O2(g) → H2O(l) ΔH = −285.8 kJ/mol reaction (3): 2 C(s) + 3 H2(g) → C2H6(g) ΔH = −84.0 kJ/mol
en 18 What is AH of the following reaction? CO2(g) + 2CH2(g) → C3H5(g) + O2(g) Substance AH,(kJ/mol) CO2(g) -393.5 out of -74.9 CH4(g) CH3(g) -104.7 Select one: a. -573.1 kJ O b. 348.4 kJ O a. 438.6 kJ O d. -648.0 kJ -348.4 kJ
CO(g) + O2(g) -> CO2(g) (unbalanced) Using the equation and thermodynamic data: AH(rxn) --566.0 kJ (for the balanced equation) Substance sºu/mol*K) O2(g) 205.0 CO(g) 197.7 CO2(g) 213.8 NOTE: Write all answers to four significant figures. a. What is the Assys(J/mol*K) - b. What is the Assurr(J/mol*K) = c. What is the Asuniv(J/mol*K) - d. At what temperature(°C) will the reaction go from spontaneous to non-spontaneous?
Using the equation and thermodynamic data: CO(g) + O2(g) --> CO2(g) (unbalanced) AH(rxn) = -566.0 kJ ( for the balanced equation) Substance sºu/mol*K) O2(g) 205.0 CO(g) 197.7 CO2(g) 213.8 NOTE: Write all answers to four significant figures. a. What is the Assys(J/mol*K) = b. What is the Assurr(J/mol*K) = c. What is the Asuniv( J/mol*K) = d. At what temperature(°C) will the reaction go from spontaneous to non-spontaneous?
Balance the equation for the complete combustion of ethane: C2H6 (g) + O2 (g) ⟶⟶CO2 (g) + H2O (g). Calculate ΔΔHofor the reaction per mole of ethane using the given bond dissociation energies. →CO2(g) + H2O (g). Calculate AH° for Balance the equation for the complete combustion of ethane: C2H6 (g) + O2(g) the reaction per mole of ethane using the given bond dissociation energies. Bond AH” (kJ/mol) C-C 347 H-O 467 C-H 413 O=0 498 C=0 799 CO 358
loab beboo 2CO2 + H2O. 7. Calculate AH for C2H2 +5/202 Given C(s) +O2(g) CO2(g) AH = -393.5 kJ H2+½ O2 H2O AH= -285.8 kJ 2C+H2 C2H2 AH = 226.8 kJ 008700000 08.0 Lon Qoe cOeEo.O60
. For the reaction C(s)+O2(g) CO2(g), AH = -393.5 kJ/mol. What is the amount of heat (in kJ) produced during the combustion of 34.56 g of coal (pure carbon)? pec To abiod to yedmun Decide whether each of these reactinns is exothorm
1) Find the AH of the following reaction: C(s) + O2(g) à CO2(g) Given the following data: Sro(s) + CO2(g) à SrCO3(s) 2Sro(s) à 2Sr(s) +0,(8) AH = -234 kJ AH = +1184 kJ 2SCO,(s) à 25r(s) + 2C(s) + 302(g) AH = +2440 kJ 2) Find the AH of the following reaction: 3NO,(g) + H2O(l) à 2HNO,(aq) + NO(g) Given the following data: 2NO(g) + O2(g) à 2NO(g) AH=-116 kJ 2N2(g) + 502(g) + 2H2O(l) à 4HNO3(aq) AH =...
Sucrose, C12H22011, is table sugar, and it has a (enthalpy of reaction) AH. of –5639.7 kJ/mol. Determine the AH; of sucrose given AH+ (H2O(1)) = -285.8 kJ/mol, and AH+ (CO2(g)) = -393.5 kJ/mol. [3] C12H22O4(s) + 12 O2(g) → 12 CO2(g) + 11 H2O(1)