10.07.2022 - 14:42

An alloy of iron and carbon was treated with sulfuric acid, in which only iron reacts. 2Fe(s) + 3H_2SO_4(aq) to Fe_2(SO_4)_3(aq) + 3H_2(g) If a sample of alloy weighing 2.358 g gave 0.1067 g of hydrogen, what is the percentage of iron in the alloy?

Question:

An alloy of iron and carbon was treated with sulfuric acid, in which only iron reacts.

{eq}rm 2Fe(s) + 3H_2SO_4(aq) to Fe_2(SO_4)_3(aq) + 3H_2(g) {/eq}

If a sample of alloy weighing 2.358 g gave 0.1067 g of hydrogen, what is the percentage of iron in the alloy?

Answers (0)
  • Gwenda
    April 11, 2023 в 21:56
    We can use the given balanced chemical equation to determine the amount of iron present in the alloy. From the equation, we see that 2 moles of Fe reacts with 3 moles of H2SO4, producing 3 moles of H2. This means that the mole ratio of Fe to H2 is 2:3. To find the moles of H2 produced from the given mass of alloy, we can use the following formula: moles of H2 = mass of H2 / molar mass of H2 The molar mass of H2 is 2 g/mol. Substituting the values given in the problem: moles of H2 = 0.1067 g / 2 g/mol = 0.05335 mol Since the mole ratio of Fe to H2 is 2:3, we can calculate the moles of Fe that reacted: moles of Fe = (2/3) x moles of H2 = (2/3) x 0.05335 mol = 0.03557 mol To find the mass of Fe in the sample of alloy, we can use its molar mass: mass of Fe = moles of Fe x molar mass of Fe The molar mass of Fe is 55.845 g/mol. Substituting the values: mass of Fe = 0.03557 mol x 55.845 g/mol = 1.980 g Therefore, the percentage of iron in the alloy is: % iron = (mass of Fe / mass of alloy) x 100% Substituting the values: % iron = (1.980 g / 2.358 g) x 100% = 83.9% Therefore, the alloy contains 83.9% iron.
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