In a constant-pressure calorimeter, 55.0 mL of 0.890 M H2SO4 was added to 55.0 mL of 0.370 M NaOH. The reaction caused the temperature of the solution to rise from 22.93 °C to 25.45 °C. If the solution has the same density and specific heat as water, what is ΔH for this reaction (per mole of H2O produced)? Assume that the total volume is the sum of the individual volumes.

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In a constant-pressure calorimeter, 55.0 mL of 0.890 M H2SO4 was added to 55.0 mL of 0.370 M NaOH. The reaction caused the temperature of the solution to rise from 22.93 °C to 25.45 °C. If the solution has the same density and specific heat as water, what is ΔH for this reaction (per mole of H2O produced)? Assume that the total volume is the sum of the individual volumes.

Chemistry
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1) write down the chemical equation for the reaction H2SO4+NaOH, and balance the equation 2) determine the limiting reactant and calculate the moles of H2O formed according to the stoichiometry of the balanced equation 3) calculate the delta H for the reaction delta H= m Ce delta T m= mass (55.0 mL + 55.0 mL) Ce= Ce of water delta T= Tfinal-Tinitial (you dont need to convert to K the delta is going to be the same if you use Celsius). 4) the delta H calculated in 3) is for the number of moles of H2O that you calculate in 2), divide the value of 3) by the value of 2) to calculate the delta H per mole of H2O.

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