Question

Use the standard heats of formation from the textbook to calculate delta H for the following...

Use the standard heats of formation from the textbook to calculate delta H for the following unbalanced reaction: C6H12O6 + O2 (g) --> CO2 (g) + H2O (g)

Homework Answers

Answer #1

The balanced reaction goes as

C6H12O6 + 6O2 = 6CO2 + 6H2O

The delta H of the reaction can be calculated by subtracting the enthalpy of formation of reactants from that of products .

Enthalpy of formation of :

C6H12O6 = -1271 KJ/mol

O2 = 0 KJ/mol

CO2 = -393.5 KJ/mol

H2O (g) = -241.8 KJ/mol

So now the enthalpy of formation of products :

6x (-393.5) + 6 x (-241.8) = -3811.8 KJ

Enthalpy of formation of reactants :

(-1271) + 6 x 0 = -1271 KJ

Delta H = -3811.8 - (-1271)

= -2540.8 KJ

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
Use standard heats of formation data from your textbook to calculate deltaH in kJ for the...
Use standard heats of formation data from your textbook to calculate deltaH in kJ for the following reactions: a). 2H2O2(l) --> 2H2O(l) + O2(g) b). HCl(g) + NaOH(s) --> NaCl(s) + H2O(l)
Use tabulated standard molar enthalpy changes of formation to calculate Delta H rxn for the following...
Use tabulated standard molar enthalpy changes of formation to calculate Delta H rxn for the following (unbalanced) reactions: SHOW WORK a. N2O4 (g) + H2 (g) --> N2 (g) + H2O(g) b. H2S (g) + O2 (g) --> SO2 (g) + H2O(g) c. Fe2O3 (s) + HCl(g) --> FeCl3 (s) + H2O(g)
Data Tables Heats of Formation Compound delta Hf (kJ mol-1) H20 (l) -285.83 CO2 (g) -391.51...
Data Tables Heats of Formation Compound delta Hf (kJ mol-1) H20 (l) -285.83 CO2 (g) -391.51 Bond Enthalpies Reaction delta H (298K) C(s, graphite) to C(g) 716.7 H-H to 2H(g) 436 C-H to C(g) + H(g) 413 C-C to 2C(g) 348 *****For the word "to" it means arrow, or reacts to form this (not able to put an arrow on here) a) If the standard enthalpy of combustion of gaseous cyclopropane, C3H6, is -2091.2kJ mol-1 at 25 C, calculate the...
Calculate the standard enthalpy of formation (∆H°f) at 298.15 K for CO(g)      Known: Reaction      ∆H°R298.15 K,...
Calculate the standard enthalpy of formation (∆H°f) at 298.15 K for CO(g)      Known: Reaction      ∆H°R298.15 K, cal/mol    for C(gr) + O2(g) → CO2(g)  =     -94,052 cal/mol and  2CO(g) + O2(g) → 2CO2(g)     = -135,272
Calculate the heat of reaction, ∆H°, for the following reaction using Standard Enthalpy of Formation 3...
Calculate the heat of reaction, ∆H°, for the following reaction using Standard Enthalpy of Formation 3 FeCl2(s) + 4 H2O(g) --> Fe3O4(s) + 6 HCl(g) + H2(g)
Use the table to calculate delta G rxn for the following reaction at 25 degree C....
Use the table to calculate delta G rxn for the following reaction at 25 degree C. A.) 2Mg(s) +O2(g) --> 2MgO(s) B.) 2SO2(g) +O2(g) --> 2SO3(g) C.) 2C2H2(g) + 5O2(g) --> 4CO2(g) + 2H2O(l) Species           Delta G (kJ/mol) Mg(s)               0 O2 (g)              0 MgO(s)            -255.0 SO2(g)            -300.57 SO3(g)            -370.53 C2H2(g)          168.43 CO2(g)            -394.65 H2O(l)             -237.35 H2O(g)            -228.77
9. Use the following experimentally derived combustion data to calculate the standard molar enthalpy of formation...
9. Use the following experimentally derived combustion data to calculate the standard molar enthalpy of formation (ΔH°f ) of liquid methanol (CH3OH) from its elements. 2 CH3OH(l) + 3 O2(g) → 2 CO2(g) + 4 H2O(l)     ΔH°rxn = −1452.8 kJ C(graphite) + O2(g) → CO2(g)                               ΔH°rxn = −393.5 kJ 2 H2(g) + O2(g) → 2 H2O(l)                                     ΔH°rxn = −571.6 kJ (1) −238.7 kJ/mol    (2) 487.7 kJ/mol       (3) −548.3 kJ/mol    (4) 20.1 kJ/mol         (5) 47.1 kJ/mol
Consider this reaction: 6CO2 + 6H2O ----> C6H12O6 + 6O2 Calculate the deltaG(degrees) for this reaction...
Consider this reaction: 6CO2 + 6H2O ----> C6H12O6 + 6O2 Calculate the deltaG(degrees) for this reaction using the following Gibb's free energy of formation values: Molecule:                                        G(degrees)f(kJ) CO2                                                    -394.4 H2O                                                    -237.2 C6H12O6                                            -917.3 O2                                                         0
Calculate the delta H degrees reaction for the following reaction: 2Ni(s) + 2S(s) +3O2 (g) ->...
Calculate the delta H degrees reaction for the following reaction: 2Ni(s) + 2S(s) +3O2 (g) -> 2NiSO3(s) from the following info: NiSO3(s) -> NiO(s) + SO2(g) delta H=156kJ S(s) + O2(g) -> SO2(g) delta H= -297 Ni(s) + 1/2O2(g) -> NiO(s) delta H = -241
Using this information together with the standard enthalpies of formation of O2(g), CO2(g), and H2O(l) from...
Using this information together with the standard enthalpies of formation of O2(g), CO2(g), and H2O(l) from Appendix C, calculate the standard enthalpy of formation of acetone. Complete combustion of 1 mol of acetone (C3H6O) liberates 1790 kJ: C3H6O(l)+4O2(g)?3CO2(g)+3H2O(l)?H?=?1790kJ
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT