Given the standard enthalpy changes for the following two reactions: (1) Zn(s) + Cl₂(g) ZnCl₂(s) AH° -415.0 kJ (2) Pb(s) + Cl₂(g) →→→→PbCl₂(s) AH° -359.4 kJ Submit Answer = KJ what is the standard enthalpy change for the reaction: (3) Zn(s) + PbCl₂(s) ZnCl₂(s) + Pb(s) AH° = = ? = Retry Entire Group 2 more group attempts remaining.

Given the standard enthalpy changes for the following two reactions: (1) Zn(s) + Cl₂(g) ZnCl₂(s) AH° -415.0 kJ (2) Pb(s) + Cl₂(g) →→→→PbCl₂(s) AH° -359.4 kJ Submit Answer = KJ what is the standard enthalpy change for the reaction: (3) Zn(s) + PbCl₂(s) ZnCl₂(s) + Pb(s) AH° = = ? = Retry Entire Group 2 more group attempts remaining.

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 43P

See similar textbooks

Similar questions

The octane number of gasoline is based on a comparison of the gasolines behavior with that of 2,2,4-trimethylpentane, C8H18(), which is arbitrarily assigned an octane number of 100. The standard enthalpy of combustion of this compound is 5456.6 kJ/mol. (a) Write the thermochemical equation for the combustion of 2,2,4-trimethylpentane. (b) Use the standard enthalpies of formation in Appendix G to calculate the standard enthalpy of formation of 2,2,4-trimethylpentane.
One of the components of jet engine fuel is n-dodecane, C12H26(), which has a standard enthalpy of combustion of 8080.1 kJ/mol. (a) Write the thermochemical equation for the combustion of n-dodecane. (b) Use the standard enthalpies of formation in Appendix G to calculate the standard enthalpy of formation of n-dodecane.
The reaction enthalpy for oxidation of styrene, C8H8, has been measured by calorimetry. C8H8() + 10 O2(g) 8 CO2(g) + 4 H2O() rH = 4395.0 kJ/mol Use this value, along with the data from Table 4.2, to calculate the standard formation enthalpy of styrene, in kJ/mol. Table 4.2 Selected Standard Formation Enthalpies, fH, at 25C
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.
sample of natural gas is analyzed and found to be88.4% methane (CH4) and 11.6% ethane (C2H6) bymass. The standard enthalpy of combustion of methaneto gaseous carbon dioxide (CO2) and liquid water (H2O) is -891 kJ/mol. Write the equation for the combustionof gaseous ethane to carbon dioxide and water.Calculate the standard enthalpy of combustion of ethaneusing standard enthalpies of formation from Table R-11on page 975. Using that result and the standard enthalpyof combustion of methane in Table 15.3, calculate theenergy released by the combustion of 1 kg of natural gas.
When 1.000 g of ethylene glycol, C2H6O2, is burned at 25C and 1.00 atmosphere pressure, H2O(l) and CO2(g) are formed with the evolution of 19.18 kJ of heat. a Calculate the molar enthalpy of formation of ethylene glycol. (It will be necessary to use data from Appendix C.) b Gf of ethylene glycol is 322.5 kJ/mol. What is G for the combustion of 1 mol ethylene glycol? c What is S for the combustion of 1 mol ethylene glycol?
Peanuts and peanut oil are organic materials and bum in air. How many burning peanuts does it take to provide the energy to boil a cup of water (250 mL of water)? To solve this problem, we assume each peanut, with an average mass of 0.73 g, is 49% peanut oil and 21% starch; the remainder is noncombustible We further assume peanut oil is palmitic acid, C16H32O2, with an enthalpy of formation of 848.4 kJ/mol. Starch is a long chain of C6H10O5 units, each unit having an enthalpy of formation of 960 kJ.
In a coffee-cup calorimeter, 100.0 mL of 1.0 M NaOH and 100.0 mL of 1.0 M HCI are mixed. Both solutions were originally at 24.6C. After the reaction, the final temperature is 31.3C. Assuming that all the solutions have a density of 1.0 g/cm3 and a specific heat capacity of 4.18 J/Cg, calculate the enthalpy change for the neutralization of HCl by NaOH. Assume that no heat is lost to the surroundings or to the calorimeter.
The enthalpy of combustion of diamond is -395.4 kJ/mol. C s, dia O2 g CO2 g Determine the fH of C s, dia.
Write reactions for which the enthalpy change will be a. Hf for solid aluminum oxide. b. the standard enthalpy of combustion of liquid ethanol, C2H5OH(l). c. the standard enthalpy of neutralization of sodium hydroxide solution by hydrochloric acid. d. Hf for gaseous vinyl chloride, C2H3Cl(g). e. the enthalpy of combustion of liquid benzene, C6H6(l). f. the enthalpy of solution of solid ammonium bromide.
In a constant-volume calorimeter, 35.0g of H2cools from 75.3C to25.0C. Calculate w, q, U, and H for the process.
A 250-g sample of water at 20.0C is placed in a freezer that is held at a constant temperature of 20.0C. Considering the water as the system, answer the following questions: a What is the sign of qsys for the water after it is placed in the freezer? b After a few hours, what will be the state of the water? c How will the initial enthalpy for the water compare with the final enthalpy of the water after it has spent several hours in the freezer? d What will the temperature of the water be after several hours in the freezer?