Determine the value of ∆H2 in kJ mol -1. Q= mc∆T Q= 13.35g x 4.18J/g°C x 2.3°C= J = 0.13kJ 0.13/0.017= 7.6kJ/mol or Q= 16.13g x 4.18J/g°C x 2.3°C= J = 0.16kJ 0.16kJ/ 0.017mol= 9.4 kJ/molUsing the values obtained for ∆H1 in #65 and #67, determine the value for ∆Hx in kJ mol ∆Hx = ∆H1- ∆H2 ∆Hx = = -49.1The magnitude (the value without the + or – sign) found in a data book for ∆Hx is 68.0 kJ mol -1. Calculate the percentage error obtained in this experiment. (If you did not obtain an answer for the experimental value of ∆Hx then use the value 60.0 kJ mol -1, but this is not the true value.) % error = theoretical – experimental/ theoretical x 100= -68- ( )/ -68 x 100 = 29.26% or -68-(-60)/ -68 x 100 = 11.76%The student recorded in her qualitative data that the anhydrous copper (I) sulfate she used was pale blue rather than completely white. Suggest a reason why it might have had this pale blue color and deduce how this would have affected the value she obtained for ∆Hx. The anhydrous copper (I) sulfate absorbed water from the air. The value would be less exothermic or less negative than expected as temperature increase would be lower or less heat evolved when anhydrous copper (I) sulfate is dissolved in water.