Consider the balanced chemical equations shown below. When a 6.00 g sample of a mixture of iron (Fe) and aluminum (Al) is treated with excess HCl(aq), 0.177 moles of H2 are obtained. What is the mass percentage of Fe in the original mixture? Choose the closest answer. Fe(s) + 2 HCI(aq) FeCl2(aq) + H2(g) → 2 AICI3(aq) + 3 H2(g) 2 Al(s) + 6 HCl(aq) 96 % 69 % 47 % 33 % 17 %
Consider the balanced chemical equations shown below. When a 6.00 g sample of a mixture of iron (Fe) and aluminum (Al) is treated with excess HCl(aq), 0.177 moles of H2 are obtained. What is the mass percentage of Fe in the original mixture? Choose the closest answer. Fe(s) + 2 HCI(aq) FeCl2(aq) + H2(g) → 2 AICI3(aq) + 3 H2(g) 2 Al(s) + 6 HCl(aq) 96 % 69 % 47 % 33 % 17 %
Chemistry & Chemical Reactivity
10th Edition
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter4: Stoichiometry: Quantitative Information About Chemical Reactions
Section: Chapter Questions
Problem 4PS: The balanced equation for the reduction of iron ore to the metal using CO is Fe2O3(s) + 3 CO(g) 2...
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![Remaining Time! 02:29:4.
Consider the balanced chemical equations shown below. When a 6.00 g sample of a mixture of iron (Fe) and
aluminum (Al) is treated with excess HCl(aq), 0.177 moles of H2 are obtained. What is the mass percentage of
Fe in the original mixture? Choose the closest answer.
Fe(s) + 2 HCI(aq) FeCl2(aq) - + H2(g)
2 Al(s) +6 HC((aq) 2 AICI3(aq) + 3 H2(g)
96 %
69 %
47 %
33 %
17 %
Rack
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Transcribed Image Text:Remaining Time! 02:29:4.
Consider the balanced chemical equations shown below. When a 6.00 g sample of a mixture of iron (Fe) and
aluminum (Al) is treated with excess HCl(aq), 0.177 moles of H2 are obtained. What is the mass percentage of
Fe in the original mixture? Choose the closest answer.
Fe(s) + 2 HCI(aq) FeCl2(aq) - + H2(g)
2 Al(s) +6 HC((aq) 2 AICI3(aq) + 3 H2(g)
96 %
69 %
47 %
33 %
17 %
Rack
Question Menu -
O O
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