THERMODYNAMICS: Given the following hypothetical thermochemical equations: 2QJ3 (g) + 3Q2X (g) 4Q2 (g) + 3J2X (1) AH = -1,080 kJ 4QJ3 (g) + 3X2 (g) 2Q2 (g) + 6J2X (1) AH = -1,520 kJ Calculate the value of AH (in kJ) for the reaction: Q2 (g) + ½ X2 (g) → Q2X (g) (Round off the final answer to ONE decimal place. Do not include unit.)

Chemistry
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Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Chapter1: Chemical Foundations
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THERMODYNAMICS. Given the following hypothetical thermochemical equations:
2QJ3 (g) + 302X (g) → 4Q, (g) + 3J½X (1)
AH = -1,080 kJ
4QJ3 (g) + 3X2 (g) → 202 (g) + 6J2X ()
AH = -1,520 kJ
Calculate the value of AH (in kJ) for the reaction:
Q2 (g) + % X2 (g)
- Q2X (g)
(Round off the final answer to ONE decimal place. Do not include unit.)
A Moving to another question will save this response.
Transcribed Image Text:A Moving to another question will save this response. Question 2 THERMODYNAMICS. Given the following hypothetical thermochemical equations: 2QJ3 (g) + 302X (g) → 4Q, (g) + 3J½X (1) AH = -1,080 kJ 4QJ3 (g) + 3X2 (g) → 202 (g) + 6J2X () AH = -1,520 kJ Calculate the value of AH (in kJ) for the reaction: Q2 (g) + % X2 (g) - Q2X (g) (Round off the final answer to ONE decimal place. Do not include unit.) A Moving to another question will save this response.
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