Fe(s) + 2 HBr (aq) ======> FeBr2 (aq) +H2(g)
Part A
Step-1 Calculate moles of Fe
Molar mass of Fe is 55.8450 g/mol
Weight of iron =3.4g iron
Moles of Iron = 3.4g/ 55.8450 g/mol = 0.06088 moles
Step-2 Calculate moles of HBr
1 mol of Fe is reacted with 2 moles of HBr
So, 0.06088 moles of Fe is reacted with 2 x 0.06088 moles of HBr = 0.12176 moles of HBr
Step-3 Calculate mass of HBr
Molar mass of HBr is 80.9119 g/mol
Mass of HBr = Moles of HBr x Molar mass of HBr
Mass of HBr = 0.12176 moles x 80.9119 g/mol = 9.85g
Mass of HBr = 9.9 g (2sig. fig.)
Part B
1 mol of Fe is produces with 1 moles of H2
So, 0.06088 moles of Fe produces with 0.06088 moles of H2
Molar mass of H2 = 2.01588g/mol
Mass of H2 = Moles of H2 x Molar mass of H2
Mass of H2 = 0.06088 moles x 2.01588g/mol = 0.12 g
Mass of H2 = 0.12 g (2sig. fig.)
8.41: Can explain this to me? Hydrobromic acid dissolves solid iron according to the following reaction...
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MISSED THIS? Read Section 4.3 (Pages 145-149); Watch KCV 4.3, IWE 4.4 Part A Hydrobromic acid dissolves solid iron according to the followiaung reaction What mass of HBr (in g) would you need to dissolve a 3.4-g pure iron bar on a padlock? Express your answer using two significant figures. View Available Hint(s) m Submit
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