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: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter5: Thermochemistry
Section: Chapter Questions
Problem 5.43QE: Another reaction that is used to propel rockets is N2O4(l)+2N2H4(l)3N2(g)+4H2O(g) This reaction has...
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![5. 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,(g)20(g)
NO(g) + 0,(g) → NO,(g) + 0,(g) AH = -199 kJ
20,(g)→3 0,(g)
AH = +495 k]
%3D
AH = -427k]](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F9b0e2cb9-5d4b-4b91-88f5-0f8b61ab6afb%2Fa68bd4b2-e34a-40d7-a897-9d426d8ccd98%2F9iaj4rs_processed.jpeg&w=3840&q=75)
Transcribed Image Text:5. 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,(g)20(g)
NO(g) + 0,(g) → NO,(g) + 0,(g) AH = -199 kJ
20,(g)→3 0,(g)
AH = +495 k]
%3D
AH = -427k]
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