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Enthalpy of neutralization = -54.3 kJ/mol (accepted value ≈ -57 kJ/mol, slight difference due to heat loss).
n=massMr=2.5074.55=0.0335 moln equals the fraction with numerator mass and denominator cap M sub r end-fraction equals 2.50 over 74.55 end-fraction equals 0.0335 mol Because the temp dropped, it is endothermic (+).
Heat escapes to the air or warms up the container walls (polystyrene cup or copper can) instead of changing the water's temperature. calorimetry worksheet 2 answers chemsheets
Find answers for a (e.g., Task 4 - Hess's Law) Let me know which question number you're stuck on! CHEMISTRY Topic 8 Energetics Calorimetry answers Y12.pdf
Note: If your worksheet has different numbers (e.g., 0.30 g ethanol, 250 g water), simply plug your values into the steps above.
Heat loss to the surroundings and the heat capacity of the calorimeter itself are often ignored unless specified. from the worksheet? CHEMISTRY Topic 8 Energetics Calorimetry answers Y12.pdf This public link is valid for 7 days
Add the volumes of both liquids together to get your mass (
= Mass of the substance being heated or cooled (measured in grams, g). Note: In solution calorimetry, we often assume of an aqueous solution has a mass of
equation. Use the mass of the water inside the copper calorimeter. The mass of the fuel is only used later to calculate the number of moles. Can’t copy the link right now
( m = 50.0 , g ), ( \Delta T = 23.5 - 100.0 = -76.5°C )
[ q = m \times c \times \Delta T ]
If you are looking for specific answers, I can help walk through the calculations if you can share the problem details (e.g., masses, temperature changes, type of reaction).