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CHEMISTRY HELP?

8.000 moles of H2(g) react with 4.000 mol of O2(g) to form 8.000 mol of H2O(l) at 25°C and a constant pressure of 1.00 atm. If 546.4 kJ of heat are released during this reaction, and PΔV is equal to -29.60 kJ, then?

ΔH° = -546.4 kJ and ΔE° = -576.06 kJ.

ΔH° = -546.4 kJ and ΔE° = -516.8 kJ.

ΔH° = +546.4 kJ and ΔE° = +576.06 kJ.

ΔH° = +546.4 kJ and ΔE° = +516.8 kJ.

1 Answer

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  • david
    Lv 7
    2 months ago

    ΔH° = -546.4 kJ and ΔE° = -576.06 kJ.

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