If you performed a similar experiment in the lab and used the following data to calculate the enthalpy of solution + neutralisation for sodium hydroxide. How many significant figures should you present your answer to? (Pay special attention to your value for temperature change, this may have fewer significant figures than you are expecting.) [1 mark]Volume HCl(aq): 40.0 mLVolume H2O: 60.0 mLMass of NaOH: 1.511 gInitial temperature: 20.5 oCFinal temperature: 29.9 oCQuestion 26Answera.3 significant figuresb.5 significant figuresc.4 significant figuresd.1 significant figuree.2 significant figures

If 0.0244mol hydrochloric acid HCl is mixed with 0.0244mol of sodium hydroxide NaOH in a "coffee cup" calorimeter, calculate the temperature change of 90.4g of the resulting solution if the specific heat of the solution is 1.00cal·g°C and the quantity of heat released by the reaction is ×1.52103cal. Round your answer to 3 significant figures.

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

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.

Determination of Enthalpy Changes in Exothermic Reactions Involving Sodium Hydroxide