Question

Ionic Compound Mass (g) T i (°C ) Tf (°C) ∆T (°C) q (J) ∆H (J/mol)...

Ionic Compound

Mass (g)

T i (°C )

Tf (°C)

∆T (°C)

q (J)

∆H (J/mol)

Calcium chloride

5g

22°C

34°C

+12°C

-251J

Ammonium nitrate

5g

22°C

16°C

-6°C

+125J

Magnesium Carbonate

2g

21°C

21°C

0°C

0

Sodium chloride

5g

21°C

20°C

-1°C

+21J

Cs (water) = 4.18 J/g-°C 
, Density of water = 1g/mL 


Q) Calculate: ∆H (J/mol), for the four ionic compounds?

1.      Were the results seen consistent with the solubility rules? If not, what is one possible explanation as to why? Was there a relationship between solubility and the sign of the enthapy? 


2. Based on the temperature change for each salt, did the water (surroundings) gain or lose energy in the form of heat? 


3. Based on the temperature change for each salt, did the reaction (system) gain or lose energy in the form of heat? 


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