Nitric oxide gas, NO(g), can be oxidized in air to produce nitrogen dioxide gas, NO,(g): 2 NO(g) + 0,(g)→2 NO,(g) Determine the enthalpy change for this reaction using any of these thermochemical equations: m 0,(g20(g) NO(g) + 0,(g) → NO,(g) + 0,(g) AH = -199 kJ 20,(2) → 3 0,(g) AH = +495 kJ AH=-427k] %3D

Nitric oxide gas, NO(g), can be oxidized in air to produce nitrogen dioxide gas, NO,(g): 2 NO(g) + 0,(g)→2 NO,(g) Determine the enthalpy change for this reaction using any of these thermochemical equations: m 0,(g20(g) NO(g) + 0,(g) → NO,(g) + 0,(g) AH = -199 kJ 20,(2) → 3 0,(g) AH = +495 kJ AH=-427k] %3D

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...

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Ethylene glycol, HOCH2CH2OH, is used as antifreeze. It is produced from ethylene oxide, C2 H40, by the reaction C2 H4O(g) + H,0(1) HOCH, CH,OH(!) Use Hess's law to obtain the enthalpy change for this reaction from the following enthalpy changes: 2C, HO(g) + 502(9) → 4CO2 (9) + 4H,0(1) AH =-2612.2 kJ HOCH, CH, OH(1) + O2 (9) → 2002 (9) + 3H,0(1) AH=-1189.8 kJ Enthalpy change = kJ %3D
Given the two thermochemical equations below, find the enthalpy change for the reaction: N2H4 (l) + H2 (g) → 2 NH3 (g) delta H = ? Given: N2O4 (g) + 3 H2 (g) → 2 NH3 (g) + 2 O2 (g) delta H = – 100.96 kJ N2O4 (g) + 2 H2 (g) → N2H4 (l) + 2 O2 (g) delta H = + 41.47 kJ Select one: a. – 142.43 kJ b. – 59.49 kJ c. + 41.47 kJ d. + 59.49 kJ e. + 142.43 kJ f. none of these g. – 100.96 kJ
Calculate the enthalpy for the reaction, BaC₂ (s) + 2 H₂O (l) → Ba(OH)₂ (aq) + C₂H₂ (g) Using the appropriate data from the following reactions, Ba (s) + 2 C (graphite, s) → BaC₂ (g) ∆H° = +437 kJ/mol Ba (s) + 2 H₂O (l) → Ba(OH)₂ +H₂ (g) ∆H° = -374.7 kJ/mol Ba (s) + 1/2 O₂ (g) → BaO (s) ∆H° = -553.5 kJ/mol BaO (s) + H₂O (l) → Ba(OH)₂ (aq) ∆H° = -107 kJ/mol C₂H₂ (g) + 5/2 O₂ (g) → 2 CO₂ (g) + H₂O (l) ∆H° = -1300. kJ/mol C (graphite, s) + O₂ (g) → CO₂ (g) ∆H° = -393.5 kJ/mol H₂ (g) + 1/2 O₂ (g) → H₂O (l) ∆H° = -285.8 kJ/mol
10.00 g of Compound X with molecular formula C4H8 are burned in a constant-pressure calorimeter containing 50.00 kg of water at 25 °C. The temperature of the water is observed to rise by 2.151 °C. (You may assume all the heat released by the reaction is absorbed by the water, and none by the calorimeter itself.) Calculate the standard heat of formation of Compound X at 25 °C. Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits.
Using the standard enthalpies of formation, what is the standard enthalpy of reaction? CO(g) + H,O(g) –→ CO,(g) + H,(g) AHân = kJ
The enthalpy change for the oxidation of butane, C4H₁0, is measured by calorimetry. C4H10 (g) + 13/2 O2(g) → 4 CO2 (g) +5 H₂O(l) A₂H = -2877.6 kJ/mol-rxn Use this value, along with the standard enthalpies of formation of CO2(g) and H₂O(l) (-393.509 kJ/mol and -285.83 kJ/mol respectively), to calculate the enthalpy of formation of butane, C4H10, in kJ/mol. Enthalpy of formation = Submit Answer OCT 30 Try Another Version tv kJ/mol S4 I all 9 item attempts remaining Cengage Learning | Cengage Technical Support A MacBook Pro 7 ( O 04
A scientist measures the standard enthalpy change for the following reaction to be -737.2 kJ : 2Co(g) + 2 NO(g)2CO2(g) + N2(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.
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.
Use the References to access important values if needed for this question. A scientist measures the standard enthalpy change for the following reaction to be -103.2 kJ: 4HCl(g) + O2(g) → 2H₂O(g) + 2Cl₂ (g) Based on this value and the standard enthalpies of formation for the other substances, the standard enthalpy of formation of HCl(g) is I kJ/mol red Species AH (kJ/mol) H₂O(g) -241.8 Cl₂(g) 0.0 0₂ (9) 0.0
（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?