OpenStudy (ars22):
Webassign help: How much energy is involved in the dissolving of sodium hydroxide in water? The table shows data from an experiment in which a measured amount of NaOH is dissolved in water in a foam cup calorimeter. Calculate ΔH for the process in kJ/mol. If the enthalpy change for the solution of NaOH is -44.87 kJ/mol, what is the percent error of the experiment? mass of water: 99.6 grams mass of NaOH: 4.01 grams change in temperature of water: 10.4 degrees
OpenStudy (jfraser):
plug into the equation for calculating heat loss or gain by calorimetry:\[Q = m*C*\Delta T\] where the m is the mass of WATER, not the sodium hydroxide. This will get you the change in energy for that small mass of NaOH. To find DH in kJ/mol, divide the heat you calculate by the moles of NaOH contained in 4.01g Learn to love the units
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