Part A Calculate AHxn for the following reaction: Use the following reactions and given AH values: Express your answer in kilojoules to three significant figures. ► View Available Hint(s) AHrxn= IVE ΑΣΦΑ ? kJ Al2O3(s) + 3CO(g) → 2Al(s) + 3CO2 (g) 2Al(s) + CO(g) + O₂(g) → Al2O3(s), ΔΗ = AH = O₂(g) → CO₂(g), -1675.7 kJ -282.7 kJ

Part A Calculate AHxn for the following reaction: Use the following reactions and given AH values: Express your answer in kilojoules to three significant figures. ► View Available Hint(s) AHrxn= IVE ΑΣΦΑ ? kJ Al2O3(s) + 3CO(g) → 2Al(s) + 3CO2 (g) 2Al(s) + CO(g) + O₂(g) → Al2O3(s), ΔΗ = AH = O₂(g) → CO₂(g), -1675.7 kJ -282.7 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

When a 4.25-g sample of solid sodium nitrate dissolves in 50.0 g of water in a coffee-cup calorimeter, the temperature drops from 28.78 °C to 24.00 °C. Thermometer Glass stirrer Cork stopper Two Styrofoam® cups nested together Reaction mixture in solution ▾ Part A What is AH (in kJ/mol NaNO3) for the dissolution of sodium nitrate: NaNO3(s) →Na+ (aq) + NO3(aq) Assume that the specific heat of the solution is the same as that of pure water (4.18 J/g. K). O 1.08 kJ/mol O 5.19 kJ/mol O 20.0 kJ/mol O 1.24 kJ/mol O 21.7 kJ/mol Submit Request Answer
Calculate the value of AH for the following reaction: 2 NO₂ (g) N₂O4 (g) → based on the formation reactions for each of the reaction components as shown below: N2 (g) + O2(g) →→→ NO₂ (g) AH = 33.2 kJ/mol N₂ (g) + 2O2 (g) →→→ N₂O4 (g) AH₂ = 11.1 kJ/mol AH: kJ/mol
BE’s are: C=O 799, C–H 413, O–H 467, O–O 498, H–H 432 kJ/mol CO2(g) + 4H2(g) → CH4(g) + 2H2O(g) ΔHrxn° = ___ kJ (from ΔHf°s) ΔHrxn°(BE) = ___ kJ (from BEs) = (2x799+432-4x413-4x467) CH4(g) + 2O2(g) → CO2(g) + 2H2O(g) ΔHrxn° = ___ kJ (from ΔHf°s) ΔHrxn°(BE) = ___ kJ (from BEs) ...Calculate ΔHrxn°s from both!
Given the enthalpies for the following reactions: 2 Fe (s) + 3/2 O₂(g) → Fe2O3 (s)Math output error AH₂ ΔΗ, CO (g) + 1/2 O₂ (g) → CO₂ (g) CO2 (g) ΔΗ = -248.7 kJ rxn rxn = 1,091.6 kJ Calculate the enthalpy change (AHrxn) for the following reaction: Fe2O3 (s) + 3 CO (g) → 2 Fe (s) + 3 CO₂ (g)
4. Hess's Law Calculate AH for the reaction: 2 C(s) + H2(g) → C:H2(g), given the following chemical equations and their respective enthalpy changes: C2H2(g)+02(g)→2CO2(g)+H20(1) AH, = -1299.6 kJ (1) %3D C(s)+02(g)→CO2(g) AH, = -393.5 kJ (2) H2(g)+502(g)→H20(1) AH3 = -285.8 kJ (3)
Part A From the following enthalpies of reaction: calculate AH for the reaction of ethylene with F₂: Express your answer in kilojoules to three significant figures. AEO AHTzn = 2486.3 kJ Submit Previous Answers Request Answer H₂(g) + F2(g) → 2HF(g), C(s) +2F2 (g) → CF4(g), 2C(s) + 2H₂(g) → C₂H₂(g), = ΔΗ ΔΗ AH C₂H4(g) +6F2 (g) → 2CF4 (g) + 4HF (g) -537 kJ -680 kJ +52.3 kJ =
Rearrange the thermochemical equations given to determine the AH value for the equation of interest. Determine: 2 Fe203(s) + 3 C(s) → 3 CO2(g) + 4 Fe(s) Given Enthalpy (K/mol) 3 -833.8 O2(g) Fe203(s) 2 1. 2 Fe(s) + ch 2. C(s) + - O2(8) → CO(g) -110.4 1 O2(g) → CO2(g) -264.8 3. CO(g) + K/mol
When 3 moles of Fe2O3(s) react with H2(g) to form Fe3O4(s) and H2O(g) according to the following equation, 6.00 kJ of energy are evolved.3Fe2O3(s) + H2(g)2Fe3O4(s) + H2O(g)Is this reaction endothermic or exothermic? What is the value of q?
The following table contains some standard enthalpies of formation, AH, at 298 K. Substance diamond graphite carbon tetrachloride carbon tetrachloride carbon tetrafluoride methane carbon monoxide carbon dioxide chlorine gas Cl₂ (g) hydrochloric acid fluorine gas hydrofluoric acid hydrogen oxygen water water hydrogen peroxide hydrogen peroxide ΔΗ (kJ/mol) 1.88 Formula C(s) C(s) 0 CCl4 (g) -106.7 CC14 (1) -139.3 CF4 (g) CH4 (g) -74.8 CO(g) -110.5 -679.9 CO₂(g) -393.5 0 HCl(g) -92.30 F2 (g) 0 HF (g) -268.61 H₂(g) 0 O2 (g) 0 H₂O(g) -241.82 H₂O(1) -285.83 H₂O2(g) -136.10 H₂O2 (1) -187.8
How much did our sodium-in-water demonstration raise the temperature of water in the dessicator jar? The reaction we performed was: Na(s) + H2O(l) NaOH(aq) + 1/2H2(g) qreaction = rHo = -184 kJ/mol-rxn Assuming the dessicator jar is well insulated (like our coffee-cup calorimeter), the energy balance is: 0 = qsystem = qreaction + qwater qreaction = -qwater qreaction = -mwater*Cwater*Twater The data from the demonstration was: (a) 1.0 kg water, (b) 22.0oC, (d) Cwater = 4.18 J/g-K, (e) mNa = 0.21 g How many moles of sodium were added to the water (in moles)?
（1）Consider the reaction: 2A (g) + 3 B (g) → 2 C (g) ΔHrxn = +254.3 kJ What will be the enthalpy change (in kJ) if 0.471 mol B reacts in excess A? （2）Consider the reaction: C (s) + O2 (g) → CO2 (g) ΔHrxn = -393.5 kJ What mass of carbon (in g) must be reacted via this mechanism to release 581.2 kJ of heat?