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To determine the heat evolved when 186 g of oxygen reacts with excess hydrogen, we first need to identify the reaction involved, which is the combustion of hydrogen to form water: 2H₂ + O₂ → 2H₂O. The molar mass of oxygen is approximately 32 g/mol, so 186 g of oxygen corresponds to about 5.81 moles (186 g / 32 g/mol). The standard enthalpy change of this reaction is approximately -286 kJ per mole of water produced; thus, the heat evolved can be calculated based on the amount of water formed from the available oxygen. For 5.81 moles of O₂, approximately 11.62 moles of H₂O are produced, resulting in around -3,327 kJ of heat evolved (11.62 moles × -286 kJ/mol).

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