**Thermochemistry Reaction Exercise****Reaction Discussion:**The chemical reaction under consideration is:\[ \text{Al}_2\text{O}_3 (s) + 3 \text{CO} (g) \rightarrow 2 \text{Al} (s) + 3 \text{CO}_2 (g) \]The goal is to calculate \( \Delta H_{\text{reaction}} \) using known thermochemical reactions.**Known Thermochemical Reactions:**1. \( 2 \text{Al} (s) + \frac{3}{2} \text{O}_2 (g) \rightarrow \text{Al}_2\text{O}_3 (s) \) - \( \Delta H = -1675.7 \, \text{kJ} \)2. \( \text{CO} (g) + \frac{1}{2} \text{O}_2 (g) \rightarrow \text{CO}_2 (g) \) - \( \Delta H = -292.7 \, \text{kJ} \)**Questions:****A. Calculate \( \Delta H_{\text{reaction}} \) for the above reaction using the given thermochemical equations.****B. Is this reaction endothermic, exothermic, or both? How do you know?**- **Blank #1**- **Blank #2**The exercise involves using Hess's Law, which states that the overall enthalpy change of a reaction is the sum of the enthalpy changes of the steps into which the reaction can be divided. Determine the total enthalpy change and describe whether the reaction releases or absorbs heat.

Answered: Image /qna-images/answer/9acdfad4-aabc-488c-b1c4-eaf97950c6de.jpg

Al203 (s) + 3 CO (g) → 2 Al (s) + 3 CO2 (g) AH = A. Calculate AHreaction for the reaction above using the following known thermochemical reactions. 2 Al (s) + 3/2 O2 (g) → Al203 (s) AH = - 1675.7 kJ CO (g) + 1/2 O2 (g) → CO2 (g) AH = - 292.7 kJ B. Is this reaction endothermic, exothermic, or both? How do you know? Blank # 1 Blank # 2

Al203 (s) + 3 CO (g) → 2 Al (s) + 3 CO2 (g) AH = A. Calculate AHreaction for the reaction above using the following known thermochemical reactions. 2 Al (s) + 3/2 O2 (g) → Al203 (s) AH = - 1675.7 kJ CO (g) + 1/2 O2 (g) → CO2 (g) AH = - 292.7 kJ B. Is this reaction endothermic, exothermic, or both? How do you know? Blank # 1 Blank # 2

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

Use Hess's Law to calculate the enthalpy for this reaction: 4SO3(g) → 4S(s) + 602(g) AH° ??? kJ !! rxn Given the following thermochemical equations: SO2(g)→ S(s) + O2{g) AH° = +296.8 kJ 2SO2(g) + O2(g) → 2SO3(g) AH° = -197.8 kJ
10. Calculate the standard enthalpy for the reaction: 4NH3(g) + 5O2(g) → 4NO(g) + 6H2O(g), given the following data: N2(g) + O2(g) → 2NO(g) ΔHrxn = -43.1 kcal mol-1 N2(g) + 3H2(g) → 2NH3(g) ΔHrxn = -21.9 kcal mol-1 2H2(g) + O2(g) → 2H2O(g) ΔHrxn = -115.6 kcal mol-1
4. When 1.00 L of 1.05 M Ba(NO3)2 solution is mixed with 1.00 L of 1.10 M NazSO4 solution at 25.0°C in a coffee-cup calorimeter. The reaction is Ba(NOs)2(aq) + NazSO4(aq) → BaSO4(s) + 2NANO:(aq). The final temperature of the mixture increases to 28.1°C. Calculate the enthalpy change per mole for this process. (Assuming C=4.18 J °C' g' and density of the final solution is 1.05 g/ml).
Use the following information to calculate the amount of heat involved in the complete reaction of 7.20 g of carbon to form PbCO3(s) in reaction 4. Be sure to give the proper sign (positive or negative) with your answer. Reaction 1 Pb(s) + O₂(g) PbO(s) Reaction 2 C(s,graphite) + O₂(g) →→→ CO₂(g) Reaction 3 PbCO3(s). PbO(s) + CO₂(g) Reaction 4 Pb(s) + C(s,graphite) + O₂(g) →→→ PbCO3(s) 1st attempt AH rxn4° = ? kJ AH rxnl AHO rxn2 AHO rxn3 AHXn4 = -219 kJ = - 394 kJ = 86 kJ = ? See Periodic Table See Hint
What is the enthalpy change when 47.6 g Al completely react, given the reaction below? The molar mass of Al = 27.0 g/mol. Fe2O3(s) + 2 Al(s) → Al2O3(s) + 2 Fe(s) ΔH°rxn = -852 kJ
The standard enthalpy change for the following reaction is -135 kJ at 298 K. 1/2 N2(g) + 1/2 H2(g) + 3/2 O2(g) HNO3(g) ΔH° = -135 kJ What is the standard enthalpy change for the reaction at 298 K? N2(g) + H2(g) + 3 O2(g)2 HNO3(g) kJ
A chemist measures the enthalpy change AH during the following reaction: 2 KCl(s) + 302(g) →2 KClO3(s) AH=78. kJ Use this information to complete the table below. Round each of your answers to the nearest kJ. reaction ΔΗ ㅁ x10 2K C103 (s) → 2KC1(s) + 302(g) KCIO, (s)-KCI(s) + 0,(s) 3 KCI(s)+0, (g)KCIO, (s) kJ kJ 1 5
Determine AH for the following reaction, N₂(g) + 3 H₂(g) → 2 NH3(g) given the thermochemical equations below. N₂(g) + O₂(g) → 2 NO(g) 4 NH3(g) + 5 O₂(g) → 4 NO(g) + 6 H₂O(g) 2 H₂(g) + O₂(g) → 2 H₂O(g) A. -1209.0 kj B.-1189.0 kJ OO OC. 150.3 k OD.-241.8 kJ E. -91.5 kJ Reset Selection o Ei C 6 AH = +180.8 kJ AH = -906.2 kJ ΔΗ = -483.6 k S IA
（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?
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)
Consider the following information: A + B → C + D AH° = -15 kJ mol-1 C + D → E AH° = +5 kJ mol-1 Calculate the enthalpy for the following reaction: 2A+2B → 2E