seld=D16741788&OpenVellumHMAC=9482457e8005a6d7cf55ed791e04593b#10001田I Review | Constants Periodic TableThe standard heat of formation, AH?, is defined asthe enthalpy change for the formation of one mole ofson eTextsubstance from its constituent elements in theirSubmitstandard states. Thus, elements in their standard stateshave AH= 0. Heat of formation values can be usedy Areato calculate the enthalpy change of any reaction.Part Bument SharingConsider, for example, the reaction2NO(g) + O2(g) = 2NO2(g)The combustion of heptane, C7H16, occurs via the reactioner Settingswith heat of formation values given by the followingC,H16(g) + 1102(g)→7CO2(g) +8H20(g)table:urse Toolswith heat of formation values given by the following table:AH?(kJ/mol)ΔΗΡ(kJ/mol)SubstanceSubstanceNO(g)90.2C7 H16 (g)-187.9O2(g)CO2 (g)-393.5NO2(g)33.2H2O(g)-241.8Then the standard heat of reaction for the overallCalculate the enthalpy for the combustion of 1 mole of heptane.reaction isExpress your answer to four significant figures and include the appropriate units.AHöm= AH (products)- AH: (reactants)[2(90.2) + 0]IXn• View Available Hint(s)2(33.2)-114 kJHAAHn =ValueUnitsrxnSubmitNext >Provide FeedbackP PearsonCopyright O 2021 Pearson Education Inc. All rights reserved. I Terms of Use . Privacy Policy I Permissions Contact Us |7:49 PM2281°F Sunny6/18/202190P Type here to searchPgDnHomeF9EndF10PgUpF11PrtScnF8F7F6

Combustion Reaction :- For organic compounds in presence of oxygen, they oxidised and forms carbon…

The combustion of heptane, C,H16, occurs via the reaction C;H16(g) + 1102(g)→7CO2(g) + 8H20(g) with heat of formation values given by the following table: AH (kJ/mol) Substance CH16 (g) -187.9 CO2(g) -393.5 H20(g) -241.8 Calculate the enthalpy for the combustion of 1 mole of heptane. Express your answer to four significant figures and include the appropriate units. > View Available Hint(s) ΔΗ Value Units Submit

The combustion of heptane, C,H16, occurs via the reaction C;H16(g) + 1102(g)→7CO2(g) + 8H20(g) with heat of formation values given by the following table: AH (kJ/mol) Substance CH16 (g) -187.9 CO2(g) -393.5 H20(g) -241.8 Calculate the enthalpy for the combustion of 1 mole of heptane. Express your answer to four significant figures and include the appropriate units. > View Available Hint(s) ΔΗ Value Units Submit

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter12: Thermodynamic Processes And Thermochemistry

Section: Chapter Questions

Problem 75AP

See similar textbooks

Similar questions

Does the standard enthalpy of formation of H2O(g) differ from H for the reaction 2H2(g)+O2(g)2H2O(g)?
How many moles of isooctane must be burned to produce loo U of heat under standard state conditions?
9.56 Using heats of formation tabulated in Appendix E, calculate the heats of reaction for the following. (a) C2H2(g)+52O2(g)2CO2(g)+H2O(l) (b) PCl3(g)+Cl2(g)PCl5(g) (c) C2H4(g)+H2O(g)C2H5OH(g) (d) Fe2O3(s)+2Al(s)Al2O3(s)+2Fe(l)
Would the amount of heat absorbed by the dissolution in Example 5.6 appear greater, lesser, or remain the same if the heat capacity of the calorimeter were taken into account? Explain your answer.
The heat of neutralization, Hneut, can be defined as the amount of heat released (or absorbed), q, per mole of acid (or base) neutralized. Hneut for nitric acid is -52 kJ/mol HNO3. At 27.3C, 50.00 mL of 0.743M HNO3 is neutralized by 1.00 M Sr(OH)2 in a coffee-cup calorimeter. (a) How many mL of Sr(OH)2 were used in the neutralization? (b) What is the final temperature of the resulting solution? (Use the assumptions in Question 11.)
In a coffee-cup calorimeter, 1.60 g NH4NO3 is mixed with 75.0 g water at an initial temperature of 25.00C. After dissolution of the salt, the final temperature of the calorimeter contents is 23.34C. Assuming the solution has a heat capacity of 4.18 J/C g and assuming no heat loss to the calorimeter, calculate the enthalpy change for the dissolution of NH4NO3 in units of kJ/mol.
The thermite reaction was once used to weld rails: 2Al(s)+Fe2O3(s)Al2O3(s)+2Fe(s)(a) Using heat of formation data, calculate H for this reaction. (b) Take the specific heats of Al2O3 and Fe to be 0.77 and 0.45 J/g C, respectively. Calculate the temperature to which the products of this reaction will be raised, starting at room temperature, by the heat given off in the reaction. (c) Will the reaction produce molten iron (mpFe=1535C,Hfus=270J/g)?
A student is asked to calculate the amount of heat involved in changing 10.0 g of liquid bromine at room temperature (22.5C) to vapor at 59.0C.To do this, one must use Tables 8.1 and 8.2 for information on the specific heat, boiling point, and heat of vaporization of bromine. In addition, the following step-wise process must be followed. (a) Calculate H for: Br2(l,22.5C)Br2(l,59.0C) (b) Calculate H for: Br2(l,59.0C)Br2(g,59.0C) (c) Using Hess's law, calculate H for: Br2(l,22.5C)Br2(g,59.0C)
Although the gas used in an oxyacetylene torch (Figure 5.7) is essentially pure acetylene, the heat produced by combustion of one mole of acetylene in such a torch is likely not equal to the enthalpy of combustion of acetylene listed in Table 5.2. Considering the conditions for which the tabulated data are reported, suggest an explanation.
When one mol of KOH is neutralized by sulfuric acid, q=56 kJ. (This is called the heat of neutralization.) At 23.7C, 25.0 mL of 0.475 M H2SO4 is neutralized by 0.613 M KOH in a coffee-cup calorimeter. Assume that the specific heat of all solutions is 4.18J/gC, that the density of all solutions is 1.00 g/mL, and that volumes are additive. (a) How many mL of KOH is required to neutralize H2SO4? (b) What is the final temperature of the solution?
Calculate the standard heat of formation of the compound ICl(g) at 25C. (Hint: Use Table 8.5 and Appendix 4 data.)
9.63 Reactions of hydrocarhons are often studied in the petroleum industry. One example is 2C3H8(g)C6H6(l)+5H2(g) , with H = 698 kJ. If 35 L of propane at 25C and 0.97 atm is to be reacted, how much heat must he supplied?