Have a few problems of this type but am totally stuck on how to proceed. Please

Question

Have a few problems of this type but am totally stuck on how to proceed. Please help. For the equation C2H5OH (l) + 3O2 (g) --> 2CO2 (g) + 3H2O (g), deltaUr = -1373 kJ at 298 K. How much heat is released per mole of ethanol combusted?

Explanation / Answer

The equation C2H5OH (l) + 3O2 (g) --> 2CO2 (g) + 3H2O (g),   H =-1373 kJ at 298 K. The equation given in the problem is a balanced chemical equationcalled as stoichiometric equation That eq gives the following information              C2H5OH (l) + 3O2 (g) --> 2CO2 (g) + 3H2O (g),   H =-1373 kJ at 298 K.                1 mole          3 moles        2moles    3moles        H negativeindicates the rxn is exothermic There fore 1 mole ethyl alcohol burns to produce 1373 kj heat at298 K more over balanced eq tells us the inter relation shipsamong the reactants & products regarding 1)moles            2)molecules          3)weights                      4)volumes     5) energy Clearly observe the stoichiometric relationships mentionedbellow                C2H5OH (l) + 3O2 (g) --> 2CO2 (g)  +    3H2O (g),    H = -1373 kJ at 298 K.                1 mole          3 moles        2moles          3moles        H negativeindicates the rxn is exothermic                1molecule    3 molecules     2molecules     3 molecules               75.427 g      32X3= 96g      2X44=88g       3X18=54 g If any reactants or products are gases ,at STP theyfollow the volume relation ship as given bellow                                  3X22.4 lits         2X 22.4lits     3X22.4lits by keeping in view all these aspects we attempt to solve this typeof problams good wishes

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