THERMODYNAMICS: Given the following hypothetical thermochemical equations: 2QJ3 (g) + 3Q2X (g)→4Q2 (g) + 3J2X (I) AH = -1,053.2 kJ 4QJ3 (g) + 3X2 (g) → 2Q2 (g) + 6J2X (1) AH = -1,536.5 kJ %3D...

THERMODYNAMICS: Given the following hypothetical thermochemical equations:<br>2QJ3 (g) + 3Q2X (g)→4Q2 (g) + 3J2X (I)<br>AH = -1,053.2 kJ<br>4QJ3 (g) + 3X2 (g) → 2Q2 (g) + 6J2X (1)<br>AH = -1,536.5 kJ<br>%3D<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>

Extracted text: THERMODYNAMICS: Given the following hypothetical thermochemical equations: 2QJ3 (g) + 3Q2X (g)→4Q2 (g) + 3J2X (I) AH = -1,053.2 kJ 4QJ3 (g) + 3X2 (g) → 2Q2 (g) + 6J2X (1) AH = -1,536.5 kJ %3D 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.)

Jun 09, 2022

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THERMODYNAMICS: Given the following hypothetical thermochemical equations: 2QJ3 (g) + 3Q2X (g)→4Q2 (g) + 3J2X (I) AH = -1,053.2 kJ 4QJ3 (g) + 3X2 (g) → 2Q2 (g) + 6J2X (1) AH = -1,536.5 kJ %3D...

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