Write a balanced ionic equation showing elemental iron reacting with H^+ to form

Question

Write a balanced ionic equation showing elemental iron reacting with H^+ to form the iron (III).icon and hydrogen gas. If your equation has fractional coefficients, re-write it with whole number coefficients. Using the reaction above, what is the ratio of moles of Fe to moles of H_2? Suppose in the experiment that 1.647 times 10^-3 moles of H_2 are collected. How many moles of iron reacted? 4. The iron used in this example weighed 0.0609 g. What would you calculate as the atomic weight iron (g/mol)? Compare this to the value taken from a periodic table.

Explanation / Answer

1)

balanced ionic equation:
Fe (s) + 6 H+ (aq) ------------------> Fe+3 (aq) + 3 H2 (g)

2)

moles of Fe = 1

moles of H2 = 3

ratio of moles of Fe and H2 = 1 : 3

3)

1 mol Fe ---------------> 3 mol H2

y mol Fe --------------> 1.647 x 10^-3 mol H2

y = 1.647 x 10^-3 / 3 = 5.49 x 10^-4

moles of Fe = 5.49 x 10^-4

4)

moles = 5.49 x 10^-4

mass = 0.0609 g

moles = mass / molar mass

5.49 x 10^-4 = 0.0609 / molar mass

molar mass = 111 g / mol

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