Question

How many milliliters of sodium metal, with a density of 0.97 g/mL, would be needed to produce 53.2 grams of hydrogen gas in the single-replacement reaction below? Show all steps of your calculation as well as the final answer.

Na + H2O → NaOH + H2

Answer 1

can u plz explain to me how to solve this i am really confused?

Answer 2

1) Balance
Write down the number of atoms that you have on each side of the equation.
Na + H2O → NaOH + H2
On the reactant Side: Na:1 H:2 O:1
On the Product Side : Na:1 H:3 O:1
Add a coefficient of 2 to H2O
Na + 2H2O →NaOH + H2
On the reactant Side: Na:1 H:4 O:2
On the Product Side: Na:1 H:3 O:1
Add a coeffcient of 2 to both Na and NaOH
2Na + 2H2O →2NaOH + H2
On the reactant Side: Na:2 H:4 O:2
On the Product Side: Na:2 H:4 O:2

Number of Moles=Mass(g)/Molar Mass(g/mol)
53.2/2=26.6
Look at the Mole Ratio of Na:H2
2:1
x:26.6
26.6*2/1=53.2 moles
Mass(g)=Molar Mass(g/mol)*Number of moles
53.2*23.0=1223.6 grams of Sodium
Density=Mass/Volume
1223.6/V=0.97
0.97V=1223.6
V=1261.4 ml

Answer 3

WOW thank for explaining this to me!!