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alekssr [168]
3 years ago
12

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 t

he single-replacement reaction below? Show all steps of your calculation as well as the final answer. Mn + H2O → MnO + H2 (5 points)
Chemistry
1 answer:
Alla [95]3 years ago
3 0
First compute the number of grams of manganese metal required to make 21.7 grams of H2. 
21.7 g H2 x (1 mole H2/ 2 g H2) x (1 mole Mn/1 mol H2) x (55 grams Mn/1 mol Mn) = 596.75 grams 
Now density = mass/volume 
7.43 = 596.75/volume 
volume = 596.75/7.43 = 80.31 mL 
80.31 mL is the amount of manganese needed.
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3 years ago
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The reaction will  shift toward the reactants if the volume is cut in half.

<h3 /><h3>Reactants </h3>

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8 0
1 year ago
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