q = mass H2O x specific heat H2O x delta T.
That gives you delta H for 14.3 g and the unit is joules.
Usually dH is given in kJ/mol. To convert to kJ/mol, convert 14.3 g NaOH to mols. mols NaOH = grams/molar mass = ?
Then divide q by mols to get J/mol and convert J/mol to kJ/mol knowing 1000 J/kJ. Post your work if you get stuck.
Calculate the change in enthalpy produced by dissolving 14.3 g of NaOH in 65.0 g of water if the temperature increases 49.1°C and the specific heat of water is 4.18 J/g°C
Do I have to use the 14.3g of NaOH?
2 answers
So just q=(65.0)(4.18)(49.1) = 13340.5 J
What about the sign for enthalpy? If the temperature is technically measured from the surroundings which increase in temperature, then the reaction itself loses heat, correct? (Exothermic, negative enthalpy?)
What about the sign for enthalpy? If the temperature is technically measured from the surroundings which increase in temperature, then the reaction itself loses heat, correct? (Exothermic, negative enthalpy?)
1 answer