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C with the value listed in the Background section of the lab manual. Calculate the experimental error according to:% error = | experimental molar volume - listed molar volume | / (listed molar volume) * 100%% Error[24.137-24.26]/(24.26)*100%=0.507%3| P a g e
ResultsAnswer the following questions in the report you submit. Lab Notes and detailed calculations should accompany submitted report. Use the area below to supply your notes and your report.1)Write balanced equation for reaction that took place.Zn(s) + 2HCl (aq) → ZnCl2 (aq) + H2(g) 2)How many moles of H2were produced when 0.25 grams of Zinc and 0.5 grams of Zinc were added?3)Which is the limiting reactant - zinc or HCl? Was all of the zinc used up in the reactions?4)Compared experimental value for the molar volume of H2with the literature value and calculated experimental error.| 24.137 - 24.26 | / (24.26) * 100% = 0.507%Notes and Report:Initial Pressure: 1.00 atmInitial Temp: 21.5 CAfter adding zinc, the mixture began to bubble. Immediately, the pressure and temp raised. Then the temp began to drop again.Pressure: 1.66 atmVolume: 92.2mL10 mL HCL + 0.5g Zinc: same initial pressure and temp with only HCLPressure and temp rose quickly and both began to drop. Pressure stops at 2.32 atmVolume: 184.5 mL50mL HCL + 20g Zinc: same initial presure and temp with only HCLWhen adding the zinc, the flask explodes. 4| P a g e