Ethanol, CH;CH,OH, is used as a gasoline additive because it boosts octane ratings. Gasoline that contains ethanol is known asgasohol. Calculate the amount of energy released by burning one gallon of ethanol. The density of ethanol is 0.787 g/mL.1 gallon = 3.785 LAH"{(CO2(s)) = -393.5 kJ/molAH?(H2O() = -285.83 kJ/molTABLEAVERAGE BOND ENERGIES*Diatomic Molecules (Dissociation Energy of Gaseous Molecules)H-H435F-FCI-CI1550-0495H-F240565430N=0N=NC=0605H-CIH-BrBr-Br1901509453651070H-I295Single Covalent Bonds (Average Values)Si- SiSi-FSi-CI415225H-CH-NC-CC-NC-0C-Si345N-N1600-01454505653900-Si0-P390305360N-O200H-O460320N-F285335H-Si300265Si-Br310N-CIP-PP-FP-CI2002100-F0-CI0-Br190H-PH-S320C-PSi-N320220200365145315C-S270Sn-Sn490H-Te240C-FSn-CI320485330275215S-0S-FS-SS-CI265C-CIC-BrP-BrP-I270285185240C-As-CI295255Multiple Covalent Bonds (Average Values)C=CC=NC=C615420605545N=N835890C=NC=0N=0750-800* 0=P0=S615C=S575515* All values are in kilojoules per mole (kJ/mol) and are rounded to the nearest 5 kJ/mol.*c=0 bond energy in CO2x 10kJ

Given the volume of ethanol burned, V = 1 gallon Density of ethanol, d = 0.787 g/mL Required…

Ethanol, CH;CH,OH, is used as a gasoline additive because it boosts octane ratings. Gasoline that contains ethanol is known as gasohol. Calculate the amount of energy released by burning one gallon of ethanol. The density of ethanol is 0.787 g/mL. 1 gallon = 3.785 L AH°{(CO2(s)) = -393.5 kJ/mol AH°{(H20O() = -285.83 kJ/mol TABLE AVERAGE BOND ENERGIES* Diatomic Molecules (Dissociation Energy of Gaseous Molecules) H-H 435 F-F 155 0-0 495 605 H-F H-CI H-Br H-I 565 CI-CI 240 N=0 N=N C=0 430 Br- Br 190 150 945 1070 365 295 Single Covalent Bonds (Average Values) 345 305 360 C-C Si- Si 225 N-N 160 145 H-C H-N H-O 415 N-O N-F N-CI 390 C-N C-0 Si-F 565 390 310 320 200 Si 0-P 450 335 Si-CI 460 320 320 365 240 285 200 210 C-Si C-P H-Si 300 Si-Br Si-N 0-F 190 220 P-P CI H-P H-S 265 C-S C-F C-CI C-Br C-I 270 Sn-Sn Sn-CI 145 315 P-F 490 0-Br S-0 200 265 H-Te P-CI 320 485 330 275 215 P-Br P-I As-CI 270 185 295 S-F S-S S-CI 285 240 255 Multiple Covalent Bonds (Average Values) C=C N=N 420 C=C 835 615 615 890 C=N C=0 N=0 605 545 515 C=N 750-800* 0=P 575 C=S 0=S *All values are in kilojoules per mole (kl/mol) and are rounded to the nearest 5 kJ/mol. *c=0 bond energy in CO2 x 10 i kJ

Ethanol, CH;CH,OH, is used as a gasoline additive because it boosts octane ratings. Gasoline that contains ethanol is known as gasohol. Calculate the amount of energy released by burning one gallon of ethanol. The density of ethanol is 0.787 g/mL. 1 gallon = 3.785 L AH°{(CO2(s)) = -393.5 kJ/mol AH°{(H20O() = -285.83 kJ/mol TABLE AVERAGE BOND ENERGIES* Diatomic Molecules (Dissociation Energy of Gaseous Molecules) H-H 435 F-F 155 0-0 495 605 H-F H-CI H-Br H-I 565 CI-CI 240 N=0 N=N C=0 430 Br- Br 190 150 945 1070 365 295 Single Covalent Bonds (Average Values) 345 305 360 C-C Si- Si 225 N-N 160 145 H-C H-N H-O 415 N-O N-F N-CI 390 C-N C-0 Si-F 565 390 310 320 200 Si 0-P 450 335 Si-CI 460 320 320 365 240 285 200 210 C-Si C-P H-Si 300 Si-Br Si-N 0-F 190 220 P-P CI H-P H-S 265 C-S C-F C-CI C-Br C-I 270 Sn-Sn Sn-CI 145 315 P-F 490 0-Br S-0 200 265 H-Te P-CI 320 485 330 275 215 P-Br P-I As-CI 270 185 295 S-F S-S S-CI 285 240 255 Multiple Covalent Bonds (Average Values) C=C N=N 420 C=C 835 615 615 890 C=N C=0 N=0 605 545 515 C=N 750-800* 0=P 575 C=S 0=S All values are in kilojoules per mole (kl/mol) and are rounded to the nearest 5 kJ/mol. c=0 bond energy in CO2 x 10 i kJ

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Using the below enthalpy of formation values, determine the enthalpy for dissolution (dissolving) of ammonium nitrate in water: NH4NO3(s) →NH4NO3 (aq) NH4NO3 (aq) AH = -339.9 kJ/mol NH4NO3 (s) AH = -365.6 kJ/mol O 705.5 kJ O -705.5 kJ 25.7 kJ -25.7 kJ O 64.1 kJ
What is DH°rxn (in kJ) for the reaction - CH4(g) + 202(g) · CO2(g) + 2H,0(1). --> DH°; (CH4(g)) = -74.8 kJ/mol DH° (CO2(g)) =–393.5 kJ/mol DH°F (H2O(1)) = -285.5 kJ/mol
1. TRUE OR FALSE (a) A desirable characteristic of a calorimeter is its ability to allow exchange of heat with the surroundsings. True False (b) An endergonic reaction is non-spontaneous and requires absorption of energy. True False
SHOW COMPLETE HANDWRITTEN SOLUTION. WRITE LEGIBLY.
Solve correctly please.
ered You want to determine the enthalpy change for the neutralization of HCI(aq). The equipment you are allowed to use are listed below: • safety goggles tion • lab coat • protective gloves • coffee cups (2) • styrofoam lid • thermometer • scale • stirring rod • beaker 16-ml of 0.345 mol/L HCI(a) added to 42.6-ml of NaOH (aq) for a total volume which is equivalent to water (m) in the q equation a. Based on the equipment provided above, design a lab to determine the enthalpy change of neutralization of HCI(aq). Ensure you use numbered steps. When you carry out the experiment, you observe a temperature change of 3.80°C. b. Calculate the quantity of heat transferred to the calorimeter based upon the data provided. c. Based upon the data provided, calculate the molar enthalpy for the neutralization of HCI(aq). d. If the mass of volume of the HCl(aq) was increased, would the value of Q be different. Explain your reasoning. e. Provide a thorough concluding statement that includes the…
A reaction has a rH value of -32.5 kJ mol-1. Is this reaction endothermic or exothermic?
A) Given the standard enthalpy changes for the following two reactions:(1) 2C(s) + H2(g)C2H2(g)...... ΔH° = 226.7 kJ(2) 2C(s) + 2H2(g)C2H4(g)......ΔH° = 52.3 kJwhat is the standard enthalpy change for the reaction:(3) C2H2(g) + H2(g)C2H4(g)......ΔH° = ?------- kJ B) Given the standard enthalpy changes for the following two reactions:(1) 2Pb(s) + O2(g)2PbO(s)...... ΔH° = -434.6 kJ(2) Pb(s) + Cl2(g)PbCl2(s)......ΔH° = -359.4 kJwhat is the standard enthalpy change for the reaction:(3) 2PbCl2(s) + O2(g)2PbO(s) + 2Cl2(g)......ΔH° = ?------ kJ
This is not a graded question
Question 15.62
Consider the reaction A B with AH° = 25.39 kJ/molxn- What should be the AH° in kJ/molm for the reaction 3 A 3 B? Report your answer to three decimal places.
Calculate AH for the following reaction, given the data in the table below: H2SO4() → So:(g) + H2O(g) AH = ??? kJ/mol H2S(g) +202(g)→ H2SO4(1) AH = -749.7 kJ H,S(g) + 202(g) → SO3(g) + H2O(1) AH = -355.0 kJ H20(1) H20(g) AH = +53.95 kJ