4) Use Hess's law to calculate AG°rxn using the following information. 2 NO(g) + O(g) → NO2(g) AG°rxn=? %3D reverse -489.6KJ 8 2 O3(g) → 3 02(g) 02(g) → 2 0(g) NO(g) + O3(g)→ NO2(g) + O2(g) AG°rxn = +489.6 kJ AG°rxn = +463.4 kJ -463,4 KJ +어9.5K3 AG°rxn = - 199.5 kJ -> A) +753.5 kJ B) +277.0 kJ C-676.0 kJ D) -1152.5 kJ E) -225.7 kJ

4) Use Hess's law to calculate AG°rxn using the following information. 2 NO(g) + O(g) → NO2(g) AG°rxn=? %3D reverse -489.6KJ 8 2 O3(g) → 3 02(g) 02(g) → 2 0(g) NO(g) + O3(g)→ NO2(g) + O2(g) AG°rxn = +489.6 kJ AG°rxn = +463.4 kJ -463,4 KJ +어9.5K3 AG°rxn = - 199.5 kJ -> A) +753.5 kJ B) +277.0 kJ C-676.0 kJ D) -1152.5 kJ E) -225.7 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

Fe O3(s) + 3CO(g) → 2Fe(s) + 3CO;g); AH® = -26.8 kJ %3D FeO(s) + CO(g) -Fe(s) + CO2(g); AH° = -16.5 kJ determine AH for the following thermochemical equation. Fe O(s)+ CO(g) 2FEO(s) + CO;(g) 6.2 kJ O 22.7 kJ O 10.3 kJ 2433KJ 2-103KJ
The enthalpy of decomposition of NO₂Cl is -114.0 kJ. Use the following data to calculate the heat of formation of NO₂Cl from N₂, O₂, and Cl₂: ✓ NO₂Cl(g) →→→ NO₂(g) + Cl₂ (g) ½-½N₂(g) + O₂(g) → NO₂(g) N₂(g) + O₂(g) + Cl₂(g) →→ NO₂CI (g) 1st attempt kJ AH rxn=-114.0 kJ AH = +33.2 kJ AH = ? See Periodic Table See Hint
Iron can be extracted from the iron(III) oxide found in iron ores (such as haematite) via an oxidation-reduction reaction with carbon. The thermochemical equation for this process is: 2 Fe203(s) + 3 C(s) → 4 Fe(1) + 3 CO2(g) AH° = +467.9 kJ
THERMODYNAMICS: A 1.09 g sample of acetic acid (HC2H302) was burned in excess oxygen in a bomb calorimeter. The calorimeter, which alone had a heat capacity of 2.67 KJPC, contained 7 g of water. The temperature of the calorimeter and its contents increased from 24.3°C to 27.95°C. What is AH (in kJ) for the combustion per 1.00 mol of acetic acid? MW of acetic acid is 60 g/mol. (Round off the final answer to ONE decimal place. Do not include the unit.)
the molar heat capacity of iron is 25.10 J mol –1 K–1 . A 25.0 g ball is heated until it is glowing red (to a temperature of 400.°C). It is dropped into a 50.0 mL container of water at 25.0°C. If the density of water is 0.997 g mL–1 , and the molar heat capacity of water is 4.186 J g–1 K–1 , what temperature (in K) will the ball and water equilibrate to? A) 338 B) 300 C) 317 D) 359 E) 342
Using the equations H₂ (g) + Cl₂ (g) → 2 HCI (g) AH° = -184.6 kJ/mol C (s) + 2 Cl₂ (g) →→ CCI (g) AH° = -95.7 kJ/mol Determine the molar enthalpy (in kJ/mol) for the reaction C (s) + 4 HCI (g) → CCI (g) + 2 H₂ (g). 4 2
Given the following Fe,03 (s) + 3 CO (g) →2 Fe (s) + 3 CO2 (g) AG' = - 29.4 kJ 3 Fe203 (s) + Co (g) →2 Fez04 (s) + CO, (g) AG° = -61.6 kJ Calculate AG° for Fez04 (s) + CO (g) → Fe (s) + Fe,03 (s) + CO2 (g)
8
Calculate ΔHo for the process ½ N2(g) + ½ O2(g) → NO(g) from the following information N2(g) + 2 O2(g) → 2 NO2(g) ΔHo = -105.8 kJ/mol 2 NO(g) + O2 → 2 NO2(g) ΔHo = -216.7 kJ/mol
Hess's Law Given the following data: 4C(s) + 3H2(g) + 1/2O2(g) → HCOC(CH2)(CH3)(l) ΔH°=-139.0 kJ CH3CH2OH(l) + 1/2O2(g) → CH3CHO(l) + H2O(l) ΔH°=-204.0 kJ 2C(s) + 3H2(g) + 1/2O2(g) → CH3CH2OH(l) ΔH°=-278.0 kJ H2(g) + 1/2O2(g) → H2O(l) ΔH°=-286.0 kJ calculate ΔH° for the reaction:2CH3CHO(l) → HCOC(CH2)(CH3)(l) + H2O(l)
*ONLY THE SECOND PART*
Determine the amount of heat (in kJ) given off when 2.56 g of NO2 is produced according to the following equation: 2NO(g) + O2(g) → 2NO2(g) ΔH = −114.6 kJ/mol Group of answer choices 3.19 kJ 5.56 kJ 6.38 kJ 1.14 kJ 114.6 kJ