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 %

A 3.27 g sample of iron ore is transformed to a solution of iron(II) sulfate, FeSO4. This solution is titrated with 0.110 M K2CT20, (potassium dichromate). If it requires 58.3 ml of potassium dichromate solution to titrate the iron(II) sulfate solution, what is the percentage of iron in the ore? The reaction is 6FESO, (aq) + K, Cr2O; (aq) + 7H;SO4 (aq) + 3Fe; (SO,)a (aq) + Cr2 (SO4)a (ag) + 7H2O(1) + K2SO, (ag) Percentage =

1.45-g sample of oxalic acid, H2C2O4, is dissolved in distilled water to make 50.00 mL of aqueous solution. This solution is called “Solution A”. The 5.00 mL of Solution A is added to 20.00 mL of distilled water to make “Solution B”.H2C2O4(aq) reacts with MnO4–(aq) to produce CO2(g) and Mn2+(aq).When 19.41 mL of H2C2O4(aq) (Solution B) is mixed with 21.59 mL of 0.0400 M MnO4–(aq), the mass of CO2(g) obtained is 0.0990 g.(a) In this chemical reaction, which substance is the oxidizing agent? Why?(b) Calculate the percentage yield of CO2(g).(c) Determine the molarity of the excess reactant at the end of the chemical reaction.

What mass of precipitate (in g) is formed when 45.5 mL of 0.300 M Na₃PO₄ reacts with 64.0 mL of 0.200 M Cr(NO₃)₃ in the following chemical reaction? Na₃PO₄(aq) + Cr(NO₃)₃(aq) → CrPO₄(s) + 3 NaNO₃(aq)

A sample of limestone and other soil materials was heated, and the limestone decomposed to give calcium oxide and carbon dioxide. CACO3 (s) → Ca0(s) + CO2 (g) A 5.483 g sample of limestone-containing material gave 2.14 g of CO2, in addition to CaO, after being heated at a high temperature. What was the mass percent of CACO3 in the original sample? %

What mass of Mg, in g, is required to react with 63.4 mL of 0.269 M AgNO3 solution? Mg(s) + 2AgNO3(aq) → 2Ag(s) + Mg(NO3)2(aq) g Mg

One way the U.S. Environmental Protection Agency (EPA) tests for chloride contaminants in water is by titrating a sample of silver nitrate solution. Any chloride anions in solution will combine with the silver cations to produce bright white silver chloride precipitate.Suppose an EPA chemist tests a 250.mL sample of groundwater known to be contaminated with cadmium chloride, which would react with silver nitrate solution like this: CdCl2(aq)+2AgNO3(aq)→2AgCl(s)+CdNO32(aq).  The chemist adds 51.0mM silver nitrate solution to the sample until silver chloride stops forming. She then washes, dries, and weighs the precipitate. She finds she has collected 8.9mg of silver chloride. Calculate the concentration of cadmium chloride contaminant in the original groundwater sample. Be sure your answer has the correct number of significant digits.

Look at the balanced chemical equation for the reaction between copper and nitric acid: Cu(s) + 4HNO3(aq) → Cu(NO3)2(aq) + 2H2O(l) + 2NO2 (g) How many grams of nitrogen dioxide would be produced if 2.47 g of copper were reacted with excess of nitric acid?

Suppose 0.0350 g Mg is reacted with 10.00 mL of 6 M HCI to produce aqueous magnesium chloride and hydrogen gas. Mg(s) + 2HC1(aq) → MgCl2(aq) +H2(g) What is the limiting reactant in this reaction? Select one: Magnesium metal Hydrochloric acid Magnesium chloride Hydrogen gas

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