Question
Calculate the molar enthalpy change for this reaction:
HCl(aq 1.00M) + NaOH -> NaCl(aq,.500M)+ H2O
Initial temp: 22.15 degrees Celsius
Extrapolated temp: 25.87 degrees Celsius
DT: 3.72 degrees Celsius
Notes:
Calculate the enthalpy change for this reaction. The density of .500 M Nacl(aq) is 1.02 g/mL and its specific heat capacity is 4.02 J/g degree celsius.
No matter how long I stare at it, and look for videos online, I can not find a definite way to solve this.
HCl(aq 1.00M) + NaOH -> NaCl(aq,.500M)+ H2O
Initial temp: 22.15 degrees Celsius
Extrapolated temp: 25.87 degrees Celsius
DT: 3.72 degrees Celsius
Notes:
Calculate the enthalpy change for this reaction. The density of .500 M Nacl(aq) is 1.02 g/mL and its specific heat capacity is 4.02 J/g degree celsius.
No matter how long I stare at it, and look for videos online, I can not find a definite way to solve this.
Answers
As I see it you haven't listed a volume; i.e., only mols/L. Without a volume you can't calculate q.
50ml
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