When 440.23 grams of iron(III) oxide are reacted with hydrogen gas, the amount of iron produced will be 307.66 grams
<h3>Stoichiometric calculation</h3>
From the equation of the reaction:
The mole ratio of iron(III) oxide to produced iron is 1:2.
Mole of 440.23 iron(III) oxide = 440.23/159.69 = 2.76 moles
Equivalent mole of produced iron = 2.76 x 2 = 5.52 moles
Mass of 5.52 moles of iron = 5.52 x 55.8 = 307.66 grams
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Answer:
The volume will be 6, 67 L
Explanation:
We use the gas formula, which results from the combination of the Boyle, Charles and Gay-Lussac laws. According to which at a constant mass, temperature, pressure and volume vary, keeping constant PV / T:
P1xV1/T1 = P2 x V2/T2
V2= ((P1xV1/T1)xT2)/P2
V2=((1,5 atm x5 L/300K)x400K)/1,5 atm
V2=6, 67 L
Depending on what you need to round it to, it’s
1.9565
Or
1.957
Or
1.96
Density is mass/volume so it’s simply 4.8/2.3
Which equals
1.95652174
Hope this helped, good luck!
Answer:
Outermost
Covalent
Two
One
Two
Two
Covalent
One
Explanation:
A covalent bond is formed when an atom shares two electrons with another atom. These shared electrons could be contributed by each of the bonding atoms or by only one of the bonding atoms.
Hydrogen has the electronic configuration of 1s1. This implies that it has only one electron in its valence shell although the 1s shell can accommodate two electrons. When the atomic orbitals of carbon and hydrogen overlap, they share two electrons and hydrogen is now associated with two electrons in a covalent bond.
Since hydrogen possesses only one valence electron, it can not be bonded to two atoms.
I do believe the answer would be physical
