Question

number 5 and 6 only

5. Part B.3. Jacob carelessly added only 40.0 mL (instead of the recommended 50.0 mL) of 1.1 M HCl to the 50.0 mL of 0 M NaOH. Explain the consequence of the error this factory error cause the reported energy of neutralization, AH, to be higher, lower, or unaffected? Explain. will the enthalpy of solution for the salt be reported too high or too low? Explain not a perfect insulator, will the enthalpy of solution, AH, for ammonium nitrate be reported as too high or too low if The chemist used a thermometer that was miscalibrated by a plus 2"C over the entire thermometer scale. Will me of the salt remains adhered to the weighing paper (and therefore is not transferred to the calorimeter), 8. Part C. The dissolution of ammonium nitrate, NH,NO, in water is an endothermic process. Since the calorimeter is 7. Part C.3. If som this heat change is ignored? Explain. 304 Calorimetry

actually only #6 please

Answer 1

5. As 50 ml of HCl is required for 50 ml of NaOH , but Jacob added only 40 ml HCl so all the H⁺ ions gets consumed and it is the limiting reactant which limits the formation of product as.

NaOH + HCl -> NaCl + H2O

6. In the Calorimeter Change in temperature is observed as heat capacity measurement is considered

so if temperature measured is 2 degree higher , so enthalpy of solution reported is higher