Question

The standard enthalpy change of combustion [to CO2(g) and H2O(l)] at 25°C of the organic solid...

The standard enthalpy change of combustion [to CO2(g) and H2O(l)] at 25°C of the organic solid diphenyl phthalate, C20H14O4(s), is determined to be -9364.7 kJ mol-1. What is the Hf° of C20H14O4(s) based on this value?   

Use the following data: Hf° H2O (l) = -285.83 kJ mol-1 ;   Hf° CO2(g) = -393.51 kJ mol-1

__________ kJ mol-1

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

0 0
Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
The standard enthalpy change of combustion [to CO2(g) and H2O()] at 25°C of the organic solid...
The standard enthalpy change of combustion [to CO2(g) and H2O()] at 25°C of the organic solid phthalic acid, C8H6O4(s), is determined to be -3207.3 kJ mol-1. What is the Hf° of C8H6O4(s) based on this value? Use the following data: Hf° H2O () = -285.83 kJ mol-1 ; Hf° CO2(g) = -393.51 kJ mol-1 kJ mol-1
A sample of solid azulene (C10H8) that weighs 0.4925 g is burned in an excess of...
A sample of solid azulene (C10H8) that weighs 0.4925 g is burned in an excess of oxygen to CO2(g) and H2O() in a constant-volume calorimeter at 25.00 °C. The temperature rise is observed to be 2.150 °C. The heat capacity of the calorimeter and its contents is known to be 9.455×103 J K-1. (a) Write and balance the chemical equation for the combustion reaction. Use the lowest possible coefficients. Use the pull-down boxes to specify states such as (aq) or...
The standard enthalpy change for the combustion of 1 mole of ethylene is -1303.1 kJ C2H4(g)...
The standard enthalpy change for the combustion of 1 mole of ethylene is -1303.1 kJ C2H4(g) + 3 O2(g) ----> 2 CO2(g) + 2 H2O Calculate the change of Hf for ethylene based on the following standard molar enthalpies of formation. molecules Change in Hf (kJ/mol) CO2 -393.5 H2O -241.8
The enthalpy of combustion (ΔH°c) of cis-1-ethyl-4-methylcyclohexane (C9H18) is -5875.10 kJ/mol. Using the appropriate information given...
The enthalpy of combustion (ΔH°c) of cis-1-ethyl-4-methylcyclohexane (C9H18) is -5875.10 kJ/mol. Using the appropriate information given below, calculate the enthalpy of formation (ΔH°f), in kJ/mol, for cis-1-ethyl-4-methylcyclohexane. Report your answer to two decimal places. ΔH°f (CO2 (g)) = -393.51 kJ/mol ΔH°f (H2O (l)) = -285.83 kJ/mol
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...
The enthalpy of combustion (∆Hc) of aluminum borohydride, Al(BH4)3(l), was measured to be -4138.4 kJ/mol [Rulon...
The enthalpy of combustion (∆Hc) of aluminum borohydride, Al(BH4)3(l), was measured to be -4138.4 kJ/mol [Rulon and Mason, J. Am. Chem. Soc.,73, 5491 (1951)]. The combustion reaction for this compound is given by Al(BH4)3(l) + 6 O2(g) → ½ Al2O3(s) + 3/2 B2O3(s) + 6 H2O(l) Given the following additional data, calculate the enthalpy of formation of Al(BH4)3(g). Substance Property Al2O3(s) ∆Hf = -1669.8 kJ/mol B2O3(s) ∆Hf = -1267.8 kJ/mol H2O(l) ∆Hf = -285.84 kJ/mol Al(BH4)3(l) ∆Hvap = 30.125 kJ/mol...
The enthalpy of combustion (∆Hc) of aluminum borohydride, Al(BH4)3(l), was measured to be -4138.4 kJ/mol [Rulon...
The enthalpy of combustion (∆Hc) of aluminum borohydride, Al(BH4)3(l), was measured to be -4138.4 kJ/mol [Rulon and Mason, J. Am. Chem. Soc., 73, 5491 (1951)]. The combustion reaction for this compound is given by Al(BH4)3(l) + 6 O2(g) → ½ Al2O3(s) + 3/2 B2O3(s) + 6 H2O(l) Given the following additional data, calculate the enthalpy of formation of Al(BH4)3(g). Substance Property Al2O3(s) ∆Hf = -1669.8 kJ/mol B2O3(s) ∆Hf = -1267.8 kJ/mol H2O(l) ∆Hf = -285.84 kJ/mol Al(BH4)3(l) ∆Hvap = 30.125...
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
A sample of asparagine was burned in the bomb calorimeter calibrated above. The following energy value...
A sample of asparagine was burned in the bomb calorimeter calibrated above. The following energy value was determined for the balanced reaction: 2 C4H8N2O3(s) + 13 O2(g) → 8 CO2(g) + 8 H2O(l) + 4 NO2(g) ΔrU = -3720 kJ Calculate the enthalpy of formation for solid asparagine, ΔfH(C4H8N2O3, ΔfH(CO2, g) = -393.52 kJ/mol ΔfH(H2O, l) = -285.83 kJ/mo lΔfH(NO2, g) = +33.10 kJ/mol Assume that ΔrU= ΔrH The answer is -790 kJ/mol enthalpy of formation solid asparagine 1. What...
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
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT