Can someone explain in detail all the steps for thisproblem? What is the percent
ID: 680141 • Letter: C
Question
Can someone explain in detail all the steps for thisproblem? What is the percent purity of a sample of iron ore if 1.25g ofsample, when reacted with an excess of HCl, produces 220 mL of H2gas collected over water at a total pressure of 1.00atm and 26degrees C? The vapor pressure of water at this temperature is 25mmHg. The reaction is: 2Fe + 6HCL = 2 FeCl3 +3H2 Can someone explain in detail all the steps for thisproblem? What is the percent purity of a sample of iron ore if 1.25g ofsample, when reacted with an excess of HCl, produces 220 mL of H2gas collected over water at a total pressure of 1.00atm and 26degrees C? The vapor pressure of water at this temperature is 25mmHg. The reaction is: 2Fe + 6HCL = 2 FeCl3 +3H2Explanation / Answer
Total pressure of gas collected = 1.00 atm = 760 mm Hg So pressure of pure hydrogen gas = 760 mm Hg - 25 mm Hg = 735mm Hg = 0.967 atm Volume = 220 mL or 0.22 L Temperature = 26 C = 299 K Moles of Hydrogen , n = PV / RT =0.967 atm * 0.22 L / (0.0821 L-atm/(mol.K) *299K) =0.00867 2Fe+ 6HCL = 2 FeCl3 +3H2 Since 2 moles of Fe give out three moles of hydrogen, moles of Fe in the sample = 0.00867 * 2 / 3 =0.00578 moles So mass of Fe = moles * atomic mass = 0.00578 mol * 55.84 g/mol = 0.3227 g So percent purity = ( Mass of Fe / mass of sample) * 100 =(0.3227 / 1.25 ) * 100 =25.81 % Since 2 moles of Fe give out three moles of hydrogen, moles of Fe in the sample = 0.00867 * 2 / 3 =0.00578 moles So mass of Fe = moles * atomic mass = 0.00578 mol * 55.84 g/mol = 0.3227 g So percent purity = ( Mass of Fe / mass of sample) * 100 =(0.3227 / 1.25 ) * 100 =25.81 %