b. If we assume that the specific heat of the solution is 1.0 cal/g · °C, calculate the ΔHsol for this compound in kcal/g and in kcal/mol. Show your work.

(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.

An insulated calorimeter contains 100 g of water at 10 °C. A salt is added to the solution, causing the temperature to drop by 3.0 °C. Given that water has a specific heat of 4.184 J/g°C, how much heat was transferred to or from the water?Group of answer choices1.3 kJ3.4 kJ4.2 kJ2.9 kJ

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.

To calculate the heat absorbed by the solution you:Question 3Select one:multiply the specific heat capacity of the solution by the temperature change. multiply the calorimeter constant by the temperature change.multiply the mass of the solution by its specific heat capacity and by the temperature change. multiply the calorimeter constant by the mass of the calorimeter and by the temperature change.

Match the correct term on the right with an example value on the left (5 marks) _____ 11. 456 kJ a. specific heat capacity of a substance _____ 12. 56 mol/L s b. total enthalpy (ΔH) _____ 13. 0.355 J/g0C c. rate constant _____ 14. 2.34 kJ/mol d. molar enthalpy (ΔHx) _____ 15. 18 L3/mol3s e. rate of reaction