Data Table: Mass of Al - 0.0352 g Temperature- 19.0 degrees C Barometric pressur

Question

Data Table: Mass of Al - 0.0352 g Temperature- 19.0 degrees C Barometric pressure- 762.5 mm Hg Volume of H2 gas- 46.92 a) write the balanced equation for the reaction betweenAluminum and hydrochloric acid? b) how many moles of Al were consumed? c) how many moles of H2 were produced? Data Table: Mass of Al - 0.0352 g Temperature- 19.0 degrees C Barometric pressure- 762.5 mm Hg Volume of H2 gas- 46.92 a) write the balanced equation for the reaction betweenAluminum and hydrochloric acid? b) how many moles of Al were consumed? c) how many moles of H2 were produced?

Explanation / Answer

(a)   2 Al + 6 HCl   ------>   2 Al Cl3   + 3 H2 . (b) Mass of Al = 0.0325 g Moles of Al = Mass / atomic mass                   = 0.0325 g / 26.98 g/mol                   = 0.0013 mol . . (c)     Volume of H2 = 46.92 mL = 0.04692 L P = 762.5 mm Hg = 1.0032 atm T = 273 + 19 = 292 K Moles of H2, n = P V/ RT                      = 1.0032 atm *0.04692 L / (0.0821 L-atm/mol/K * 292 K)                       = 0.00196 moles

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