How many milliliters of manganese metal, with a density of 7.43 g/mL, would be needed to produce 21.7 grams of hydrogen gas in the single-replacement reaction below? Show all steps of your calculation as well as the final answer.

Mn + H2O → MnO + H2

Question

How many milliliters of manganese metal, with a density of 7.43 g/mL, would be needed to produce 21.7 grams of hydrogen gas in the single-replacement reaction below? Show all steps of your calculation as well as the final answer.

Mn + H2O → MnO + H2

dtan5457 · Answer

You know that the molar mass of H2 is basically 2...so you gotta realize that the ratio here is 1:10. In other words, 21.7 grams of hydrogen means that multiplied the original equation by 10 moles.

Knowing that, you gotta multiply Mn's formula mass by 10.

10Mn=591 grams (rounded)

Now, reverse the density mass of 

d=mass/volume

you know the density (given in the problem ) is 7.43 g/ml and that the mass is 591 grams.

to get volume, you would do mass/density

591/7.43=about 80 ml of Mn

anonymous · Answer

thank you!

dtan5457 · Answer

Welcome. Feel free to fan and medal and tag me onto more questions.