Mark Brainliest please
Answer :
In my opinion , answer is A
Answer:
H2
Explanation:
CO2 + H2 → CO + H2O
↓ (-2). 0. (+2 )(-2). (+1)(-2)
↓ ·2 (+2)
+4 (-4)
Write down the oxidation number under each element, each molecule should equal 0 unless there is a charge shown.
Oxygen, always has an oxidation number of -2 unless in a peroxide.
Hydrogen, is -1 with metals,+1 with non-metals. Hydrogen loves non-metals!
H2 is zero because any standalone element has an oxidation number of zero
What is being oxidized? Whatever is being oxidized, loses electrons and becomes more positive, it will be a whole molecule, not just an element. In this case, the H in H2 goes from 0 to (+1) so it is the oxidized molecule.
Answer: 34.4 g
Explanation:
![\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}](https://tex.z-dn.net/?f=%5Ctext%7BNumber%20of%20moles%7D%3D%5Cfrac%7B%5Ctext%7BGiven%20mass%7D%7D%7B%5Ctext%7BMolar%20mass%7D%7D)
![\text{Number of moles of hydrogen}=\frac{5g}{2g/mol}=2.5moles](https://tex.z-dn.net/?f=%5Ctext%7BNumber%20of%20moles%20of%20hydrogen%7D%3D%5Cfrac%7B5g%7D%7B2g%2Fmol%7D%3D2.5moles)
As
is in excess,
is the limiting reagent and thus it will limit the formation of products.
![CO+2H_2\rightarrow CH_3OH](https://tex.z-dn.net/?f=CO%2B2H_2%5Crightarrow%20CH_3OH)
According to stoichiometry:
2 moles of hydrogen produce = 1 mole of ![CH_3OH](https://tex.z-dn.net/?f=CH_3OH)
2.5 moles of hydrogen produce =
of ![CH_3OH](https://tex.z-dn.net/?f=CH_3OH)
Mass of ![CH_3OH=moles\times {\text {Molar mass}}=1.25\times 32=40g](https://tex.z-dn.net/?f=CH_3OH%3Dmoles%5Ctimes%20%7B%5Ctext%20%7BMolar%20mass%7D%7D%3D1.25%5Ctimes%2032%3D40g)
But as % yield is 86%, mass of
produded is ![\frac{86}{100}\times 40=34.4g](https://tex.z-dn.net/?f=%5Cfrac%7B86%7D%7B100%7D%5Ctimes%2040%3D34.4g)
Thus 34.4 g of
is produced.
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