Answer:
(A) is 0.0773 mol B2H6
(C) is 2.79 x 10^23 H atoms
Explanation:
Questions (A) and (B) are the same.
2.14 g B2H6 x (1 mol B2H6/27.668g B2H6) = 0.0773 mol B2H6 (A)
<u>27.668 is the molar mass of B2H6 calculated from the period table: </u>
(2 x 10.81) + (6 x 1.008) = 27.668
1.008 is the mass of H and 10.81 is the mass of B
(C)
0.0773 mol B2H6 x (6 mol H/ 1 mol B2H6) x (6.022 x 10^23 H atoms/1 mol H)
= 2.79 x 10^23 hydrogen atoms
Further Explanation:
- For every 1 mol of B2H6, there are 6 moles of H (indicated by the subscript)
- 6.022 x 10^23 is Avogrado's number and it equals to 1 mol of anything
- Avogrado's number can be in units of atoms, molecules, or particles
I’m sorry if I wasted your time but I think it’s alkali metals but I’m
Not sure
Answer:
H2-1
H2+-1/2
H22- zero
Explanation:
Bond order= Bonding electrons-antibonding electrons/2
In H2, there are two bonding electrons and no antibonding electrons. In H2+ there is only one bonding electron and no antibonding electron while in H22- there are two bonding and two antibonding electrons respectively.
Explanation:
nH2O=35/18
xH2O=35/18x6.02x10 powered by 23
so, the answer is
im sry if im wrong
Answer:
5.56 moles H₂O
Explanation:
moles = mass of substance / formula weight of substance
∴moles H₂O = 100 grams / 18 grams/mole = 5.56 moles H₂O
