Formation ReactionsCorThe standard heat of formation, AH, is defined as theenthalpy change for the formation of one mole ofsubstance from its constituent elements in theirstandard states. Thus, elements in their standard stateshave AH =0. Heat of formation values can be usedto calculate the enthalpy change of any reaction.with heat of fomation values given by the following table:Substance(kJ /mol)CHs (g)104.7CO2(g)393 5Consider, for example, the reactionH2O(g)-241.82NO(g) + O2(g)=2NO2(g)with heat of formation values given by the followingCalculate the enthalpy for the combustion of 1 mole of propane.table:Express your answer to four significant figures and include the appropriate uAH(kJ/mol)SubstanceView Available Hint(s)NO(g)90.2O2 (g)NO2(g)33.2AH =ValueUnitsThen the standard heat of reaction for the overallreaction isSubmitAHn= AH (products)- AH (reactants)[2(90.2) + 0]2(33.2)-114 kJProvide FeedbackP Pearson田

The standard formation data given is,

with heat of formation values given by the following table: AH (k.J mol) Substance CHa (g) H104.7 CO2(g) 393 5 H O(g) 241.8 Calculate the enthalpy for the combustion of 1 mole of propane. Express your answer to four significant figures and include the approp View Available Hint(s)

with heat of formation values given by the following table: AH (k.J mol) Substance CHa (g) H104.7 CO2(g) 393 5 H O(g) 241.8 Calculate the enthalpy for the combustion of 1 mole of propane. Express your answer to four significant figures and include the approp View Available Hint(s)

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

What is the change in the enthalpy (in kJ) for the complete combustion of 39.0 g of fructose, roughly the amount of sugar in a 12-oz can of soda? C,H12O6 (s) + 602(g) → 6CO2(g)+6H,O(1) AH = -2.83 × 10° kJ mol¬1 A: -6.13 x 102 3703
A student burnt 0.40 g of ethanol using a calorimeter filled with 150 cm³ of water and noted a temperature change from 21.7°C to 29.6°C. Assuming standard conditions calculate a value for the standard enthalpy change of combustion of ethanol.
Given the reaction below, write the thermochemical equation showing the enthalpy of the decomposition reaction of 1 mol hydrogen peroxide into water and oxygen. 2 H2O1) + O2(g) * 2 H202(aq) AH = 196. 4 kJ -->
The combustion of ethanol, C,H$OH@ to form carbon dioxide gas and water. What is the enthalpy of ethanol if the enthalpy of combustion reaction is – 1366.8 kJ? What is the change in internal - energy of the reaction at constant volume? C2H5OH) + 3O2 (g) 2CO2(g) + 3H2O) Substance C2H5OH) O2(g) CO2{g) H2O1) AH°:(kJ/mol) ? -393.5 -285.84
Given the following reaction and enthalpy value:H2(g) + I2(g) -> 2HI(g) deltaH = +52.96 kJCalculate the change in enthalpy for the following reaction:HI(g)-> ½H2(g) + ½I2(g)
a) Calculate the enthalpy variation produced in the butane combustion reaction under standard conditions.b) what amount of heat will be released in the complete combustion of the 12kg of butane contained in a cylinder dH standard CO2 (g) = -393kJ / mol, H2O (l) = -286kJ / mol, C4H10 (g) = -125kJ / mol
Calculate the heat of combustion in kJ 1.0000 mol of ethyl stearate (C20H40O₂), an important component of many biodiesel fuels made from soybean oil and ethanol, given the following standard enthalpies of formation: CO:(g) = -393.5 kJ/mol H₂O(1) = -285.8 kJ/mol C20H40O2(1) = -984.6 kJ/mol
To study the possible amount of energy generated by a person, the person can be roughly viewed as a constant pressure calorimeter using table sugar (sucrose, C12H22O11) as the energy generator. The reaction of table sugar in a calorimeter is given by: C12H22O11(s) + 12O2(g) ----------> 12CO2(g) + 11H2O(g) a. What is the heat released by consuming one mole of sugar (C12H22O11) in this way? b. Calculate the enthalpy of combustion per mole of sugar utilization. c. Does the result of your calculation make sense?
a) From the table of standard enthalpies of formation given below, calculate the standard enthalpy of the following reaction. Ca3P2(s) + 6HCl(g) ----> 3CaCl2(s) + 2PH3(g) Compound ΔHfo(KJ/mole) Ca3P2(s) -504 HCl(g) -92 CaCl2(s) -794 PH3(g) +9
Given the standard enthalpies of formation for the following substances, determine the change in the enthalpy for the combustion of 1.0 mol of propane, C3H8. Substance ΔH ̊f in (kJ/mol) C3H8 (g) -103.8CO2(g) -393.5 H2O(l) -285.8