thermochem lad C3_C4-5

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Jan 9, 2024

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If you mixed 5.09 g of NH4NO3 with 99.14 mL of water, and the initial temperature was 20.9 and the final temperature was 27.6, calculate energy, in joules, and the change in enthalpy ( ∆ H) of this reaction. Was this process exothermic or endothermic? If CaCl2 was heated before dropping it into the foam cup, what effect would it have on your measured data? If your labmate accidentally used 4g instead of 2g for the experiment, how would this effect your data (q and ∆ H)? If your labmate accidentally used 100ml instead of 50ml for the experiment, how would this effect your data (q and ∆ H)? If the solution was 10 ℃ warmer to start, how would this effect your data?
If your cup had a hole in it or you used a plastic cup instead of styrofoam, how would this effect your data? If you had 2.06g of NaOH in 52 mL HCl in RXN A and the temperature changed from 19.5 to 26.4, what is the Q and what is the enthalpy in kJ/mol? If you mixed this solution with 1M HCl and 50mL in RXN C and the temperature changed from 22.1 to 27.8, what is the Q and what is the enthalpy in kJ/mol? Use Hess’ Law to solve for what the calculated ∆ H should be. If you had 2.02g of NaOH with 50 mL of HCl in RXN B and the temperature changed from 21.7 to 39.7 what is the Q and what is the enthalpy in kJ/mol? Use 2 of these equations to determine the percent error of this experiment. Why does CaCl2 get hot and why does NH4NO3 get cold? Justify. Why do you have to use exactly 2g for experiment B? What if you didn’t use 2g for experiment C? Would your calculations be off?
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