Given the balanced equation below, calculate the moles of aluminum that are needed to react completely with 17.5 moles of feo? you must show all of your work. 2al + 3feo à 3fe +al2o3 sodium and water react according to the following equation. if 51.5g of sodium are added to excess water, how many liters of hydrogen gas are formed at stp? show all work for credit. 2na + 2h2o à 2naoh + h2
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Ответ:
The moles off Al that are needed to react completely with 17.5 moles of FeO is 11.67 moles
calculation
2Al + 3 FeO→ 3 Fe + Al₂O₃
From equation above Al: FeO is 2:3
therefore the moles of Al = 17.5 moles x 2 /3 = 11.67 moles
Question 2
The number of liters of hydrogen gas that are formed at STP 25.088 L
calculation
2Na + 2H₂O → NaOH +H₂
Step 1 : calculate the moles of Na
moles = mass÷ molar mass
from the periodic table the molar mass of Na = 23 g/mol
moles= 51.5 g÷ 23 g/mol =2.24 moles
Step 2: use the mole ratio to determine the moles of H₂
Na:H₂ is 2:1 therefore the moles of H₂ = 2.24 moles x 1/2 =1.12 moles
Step 3: calculate the number of liters of H₂ at STP
that is at STP 1 mole of a gas = 22.4 L
1.12 moles = ? L
by cross multiplication
=( 1.12 moles x 22.4 L) / 1 mole = 25.088 L
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