Answer:
C24H50
Explanation:
The empirical fomula's molar mass is 169.25 g/mol.
We know the molecular formula's molar mass is 338 g/mol.
338/169.25= 1.99 or approximately 2
From the given balanced equation we have find out the amount (in gm) of Ag formed from 5.50 gm of Ag₂O.
2Ag₂O(s) → 4Ag (s) + O₂ (g)
We know, molecular mass of Ag₂O= 231.7 g/mol, and atomic mass of Ag= 107.8 g/mol. Given, mass of Ag₂O=5.50 gm. Number moles of Ag₂O=
= 0.0237 moles.
From the balanced chemical reaction we get 2 (two) moles of Ag₂O produces 4 (four) moles of Ag. So, 0.0237 moles of Ag₂O produces
moles=0.0474 moles of Ag= 0.0474 X 107.8 g of Ag=5.11g Ag.
Therefore, 5.50 g Ag₂O produces 5.11 g of Ag as per the given balanced chemical reaction.
Molar mass CCl₄ = 12 + 35.5 x 4 = 154 g/mol
number of moles:
74.41 / 154 => 0.48318 moles
1 mole ------------------- 6.02 x 10²³ molecules
0.48318 moles ----------- ?
molecules = 0.48318 x ( 6.02x10²³) / 1
molecules = 2.908 x 10²³ / 1
= 2.908 x 10²³ molecules
hope this helps!