A scientist measures the standard enthalpy change for the following reaction to be 82.5 kJ: 3Fe2O3 (8) + H₂(g) → 2Fe3O4 (s) + H₂O(g) Based on this value and the standard enthalpies of formation for the other substances, the standard enthalpy formation of Fe2O3 (s) is kJ/mol Species AH (kJ/mol) Fe3O4 (8) H₂O(g) H₂(g) Submit Answer -1118.4 -241.8 0.0 Retry Entire Group 2 more group attempts remaining

A scientist measures the standard enthalpy change for the following reaction to be 82.5 kJ: 3Fe2O3 (8) + H₂(g) → 2Fe3O4 (s) + H₂O(g) Based on this value and the standard enthalpies of formation for the other substances, the standard enthalpy formation of Fe2O3 (s) is kJ/mol Species AH (kJ/mol) Fe3O4 (8) H₂O(g) H₂(g) Submit Answer -1118.4 -241.8 0.0 Retry Entire Group 2 more group attempts remaining

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

A scientist measures the standard enthalpy change for the following reaction to be -2929.4 kJ :2C2H6(g) + 7 O2(g)4CO2(g) + 6 H2O(g)Based on this value and the standard enthalpies of formation for the other substances, the standard enthalpy of formation of CO2(g) is kJ/mol.
The standard molar enthalpy of formation of diborane, B₂H₁ (g), cannot be determined directly because the compound cannot be prepared by the reaction of boron and hydrogen. It can be calculated from other enthalpy changes, however. The following enthalpy changes can be measured. 4 B(s) + 3 O₂ (g) → 2 B₂O3 (s) A₁H° = -2543.8 kJ/mol-rxn H₂(g) + 1/2 O₂ (g) → H₂O(g) A, H = -241.8 kJ/mol-rxn B2 H6 (g) + 3 O2 (g) → B₂O3 (g) + 3 H₂O(g) A₁H° = −2032.9 kJ/mol-rxn a we will show how these equations can be added together to give the equation for the formation of B₂ H6 (g) from B(s) and H₂(g) in their standard states and determine the enthalpy of formation. The target reaction is 2 B(s) + 3 H₂(g) → B2H6 (g) Does Reaction 1 need to be used as is, or reversed? as is reversed The reaction is used as is because B(s) is a reactant in the target reaction and in Reaction 1. Correct b Does Reaction 1 need to be multiplied by a scaler? Choose a scaling number for Reaction 1. Target Reaction: 2 B(s) + 3…
A scientist measures the standard enthalpy change for the following reaction to be -876.7 kJ :2NH3(g) + 3 N2O(g)4N2(g) + 3 H2O(g)Based on this value and the standard enthalpies of formation for the other substances, the standard enthalpy of formation of NH3(g) is kJ/mol.
The hypothetical element X and an oxide of X undergo the following reactions with oxygen, with the listed enthalpy changes: 4 X(5) + 3 02(g) – 2 X203(g) AHrxn = -400.0 kJ 4 XO2(g) – 2 X203(g) + O2(g) AHrxn - +200.0 kJ Using the above information, determine AHrxn for the following reaction: X(S) + O2g) – XO22) O -200.0 k) O -600.0 kJ O -150.0 k) O 200.0 kJ
For which one of the following is the enthalpy of the reaction the same as the enthalpy of formation? A) 2 H (g) + Se (s) → H:Se (g) B) KOH (s) → K*(aq) + OH- (aq) C) 2 Fe (s) + 3 Cl2 (g) → 2 FeCl3 (s) D) Ni (s) + ½ O2 (g)- NiO (s)
A scientist measures the standard enthalpy change for the following reaction to be -104.0 kJ : Cog) + Cl2(g)–→COCl2(g) Based on this value and the standard enthalpies of formation for the other substances, the standard enthalpy of formation of CO(g) is kJ/mol.
Methanol (CH3OH) can be used as the fuel in a "canned heat" container that is used to keep food hot on a buffet table. The combustion of methanol can be described by the following BALANCED thermochemical equation: 2 CH3OH(l) + 3 O2(g) → 2 CO2(g) + 4 H2O(g) ΔH° = –1199 kJ Calculate the enthalpy change, in kilojoules, when 151.3 g of methanol is burned via this reaction?
A chemist measures the enthalpy change AH during the following reaction: Fe(s) + 2 HCl(g) →FeCl₂(s) + H₂(g) Use this information to complete the table below. Round each of your answers to the nearest kJ/mol. reaction AH=157. kJ FeCl₂ (s) + H₂(g) → Fe(s) + 2HC1 (g) 2Fe (s) + 4H C1 (g) 3 FeCl₂ (s) + 3H₂(g) 2FeCl₂ (s) + 2H₂(g) 3Fe (s) + 6HCl (g) ΔΗ [ kJ kJ kJ 0x x10 × Ś
A scientist measures the standard enthalpy change for the following reaction to be 216.8 kJ :CH4(g) + H2O(g)3H2(g) + CO(g)Based on this value and the standard enthalpies of formation for the other substances, the standard enthalpy of formation of H2O(g) is kJ/mol.
A scientist measures the standard enthalpy change for the following reaction to be 184.8 kJ:Fe3O4(s) + 4 H2(g) 3Fe(s) + 4 H2O(g)Based on this value and the standard enthalpies of formation for the other substances, the standard enthalpy of formation of Fe3O4(s) is kJ/mol.
A scientist measures the standard enthalpy change for the following reaction to be -912.5 kJ:2NH3(g) + 3 N2O(g)4N2(g) + 3 H2O(g)Based on this value and the standard enthalpies of formation for the other substances, the standard enthalpy of formation of H2O(g) is kJ/mol.
Consider the following balanced reaction: 2 H2S(g) + 3 O2(g) → 2 H2O(l) + 2 SO2(g) ΔHrxn = -1124.0 kJ Calculate the enthalpy of formation (in kJ/mol) for H2S(g). Given: The standard enthalpies of formations (ΔHof) of H2O(l) and SO2(g) are -285.8 kJ/mol and -296.8 kJ/mol, respectively. IMPORTANT: Enter both the sign and the value (no units), using 1 decimal place (e.g. -999.9) Consider the following balanced reaction: 2 H2S(g) + 3 O2(g) → 2 H2O(l) + 2 SO2(g) ΔHrxn = -1124.0 kJ Calculate the enthalpy of formation (in kJ/mol) for H2S(g). Given: The standard enthalpies of formations (ΔHof) of H2O(l) and SO2(g) are -285.8 kJ/mol and -296.8 kJ/mol, respectively. IMPORTANT: Enter both the sign and the value (no units), using 1 decimal place (e.g. -999.9)