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So every 2 molecules of water gives 1 molecule of oxygen.
This ratio (
So to produce 2.5 moles of oxygen, you will need the double number of moles of water, i.e. 5 moles.
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For which equation, does the enthalpy of reaction represent $DeltaH_f^@$ for methanol?
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The standard of formation is the enthalpy associated with the formation of 1 mole of substance from its constituent in their standard states under specified conditions. And of course...
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How much heat will be released when 12.0 g of $H_2$ reacts with 76.0 g of $O_2$ according to the following equation? $2H_2 + O_2 -> 2H_2O$ $DeltaH$= -571.6 kJ?
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For the reaction: $2H_2O + 137 kcal -> 2H_2(g) + O_2(g)$ how many kcal are needed to form 2.00 moles $O_2(g)$?
Start by taking a look at the thermochemical equation given to you $2"H"_ 2"O"_ ((l)) + "137 kcal" -> 2"H"_ (2(g)) + "O"_ (2(g))$ Notice that this thermochemical...
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