Question 9 THERMODYNAMICS: Given the following hypothetical thermochemical equations: 2QJ3 (g) + 3Q2X (g) → 4Q2 (g) + 3J2X (1) AH = -1,003.7 kJ 4QJ3 (g) + 3X2 (g) → 2Q2 (g) + 6J2X (1) AH = -1,544.6 kJ...

Question 9<br>THERMODYNAMICS: Given the following hypothetical thermochemical equations:<br>2QJ3 (g) + 3Q2X (g) → 4Q2 (g) + 3J2X (1)<br>AH = -1,003.7 kJ<br>4QJ3 (g) + 3X2 (g) → 2Q2 (g) + 6J2X (1)<br>AH = -1,544.6 kJ<br>Calculate the value of AH (in kJ) for the reaction:<br>Q2 (g) + ½ X2 (g) → Q2X (g)<br>(Round off the final answer to ONE decimal place. Do not include unit.)<br>A Moving to another question will save this response.<br>

Extracted text: Question 9 THERMODYNAMICS: Given the following hypothetical thermochemical equations: 2QJ3 (g) + 3Q2X (g) → 4Q2 (g) + 3J2X (1) AH = -1,003.7 kJ 4QJ3 (g) + 3X2 (g) → 2Q2 (g) + 6J2X (1) AH = -1,544.6 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.) A Moving to another question will save this response.

Jun 09, 2022

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Question 9 THERMODYNAMICS: Given the following hypothetical thermochemical equations: 2QJ3 (g) + 3Q2X (g) → 4Q2 (g) + 3J2X (1) AH = -1,003.7 kJ 4QJ3 (g) + 3X2 (g) → 2Q2 (g) + 6J2X (1) AH = -1,544.6 kJ...

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