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 alexvela94 10-25-2008 06:17 PM

50 mL of 1.0 M HCl at 25 degrees C is mixed with 50.0 mL of 1.0 M NaOH at 25 degrees C. When the two are mixed the temp becomes 31.9

Net Ionic Equation

H+ (aq) + OH- (aq) --> H20 (l)

Energy released = s x m x Delta T
the energy released according to this formula is 2.9 x 10^3 J

Everything Below this sentence i do not understand!!!

my book goes on saying that Enthalpies of reaction are often expressed in terms of moles of reacting substances. The number of moles of H+ ions consumed in the preceding experiment is

50 mL x (1L/1000mL) (1.0 mole/L) = 5.0 x 10^-2 mol H+

thus 2.9 x 10^3 J heat was released when 5.0 x 10^-2 mole H+ ions reacted or

(2.9 x 10^3 J)/(5.0 x 10^-2 mole H+) = 5.8 x 10^4 J/mol

of heat released per 1.0 mol H+ ions neutralized. Thus the magnitude of the enthalpy change per mole for the reaction

H+ (aq) + OH- (aq) --> H20 (l)

is 58 kJ/mol. Since heat is evolved, Delta H = -58 kJ/mol

please make this into regular english!

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