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If 0.120 moles of water are produced in the reaction H+(aq)+OH-(aq)=H2O deltaH=-56.2kj/mol
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If 0.120 moles of water are produced in the reaction H+(aq)+OH-(aq)=H2O deltaH=-56.2kj/mol
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If 0.120 moles of water are produced in the reaction H+(aq)+OH-(aq)=H2O deltaH=-56.2kj/mol
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Butane (C4H10) burns in the presence of oxygen (O2) to produce carbon dioxide (CO2) and water (H2O).
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Given the following equations:
2 H2 (g) + O2 (g)--> 2 H2O (l) deltaH = -571.6 kJ N2 (g) + O2 (g)-->2 NO (g) deltaH = +180.5 kJ N2
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