Input your answer for the enthalpy of solution of NaOH (ΔH3) here. Your answer should be in kJ mol-1 to 2 decimal places. INCLUDE A SIGN. Do not include units.

Another student in the class repeated this experiment. The student's calculated values for ΔH1 and ΔH2 are shown below. ΔH1 PART B1 (heat of neutralisation of NaOH) = -42.54 kJ mol-1ΔH2 PART B2 (heat of solution + neutralisation of NaOH) = -120.42 kJ mol-1Use these values to determine this students experimentally determined answer for the enthalpy of solution for NaOH (ΔH3) in kJ mol-1.Provide your answer to 1 decimal place. INCLUDE A SIGN. Do not include units.

(ii) Show that the heat energy change, Q, in the student’s experiment is about 1100 J.[for the mixture, c = 4.2 J/g/°C][massof1.0 cm 3of mixture = 1.0 g] (3)(iii) The student uses 0.020 mol of potassium hydroxide in his experiment.Calculate the enthalpy change (ΔH) in kJ/mol, for 1.0 mol of potassium hydroxide.Include a sign in your answer.

Youhcl + naoh --> nacl + h2o. 200cm^3 of 0.2 mol/dm^3 hcl was reacted with 100 cm^3 of 0.15 mol/dm^3 naoh, where the enthalphy change is -57.3 kJ. find the overall enthalpy change using moles

When 1.00g of sodium hydroxide is dissolved in 100.0 g of water in an insulatedcontainer the temperature rises from 20.00°C to 22.66°C. Calculate the enthalpychange for the solution. State any assumptions made.NOTE: Dissolving reactions due not have limiting reagents.

When 100.0 cm-3of 1.00 mol dm-3 NaOH is added to 100.0 ml of 1.00 moldm-3 HCl in aninsulated container the temperature rises from 21.0°C to 34.6°C.NaOH(aq) + HCl (aq) → NaCl(aq) + H2O(l) Calculate the enthalpy change for theneutralization reaction. State any assumptions made