What mass of hbo2 is produced from the
combustion of 96.9 g of b2h6?

11.0845g of is produced from the combustion of 96.9 g of

Explanation:

Given:

mass of   used in combustion= 96.9 g

To find:

amount  of   produced=?

Solution:

Let us find the molecular mass of

Atomic weight of Boron(B)=10.811

Atomic weight of Hydrogen(H)=1.007

Now the molecular mass of

=>2(10.811)+6(1.007)

=>21.622 x 6.042

=>27.664

In the given 96.9 g of , the number of moles of present is

So in 96.9 g of B2H6, 3.50  moles of   B2H6  is present  which is converted into 2 molecules of  

The molecular mass of   is

Atomic weight of Boron(B)=10.811

Atomic weight of Hydrogen(H)=1.007

Atomic weight of Oxygen(O)=15.9994

=> 10.811+1.007+2(15.9994)

=>10.811+1.007+31.998

=>43.816

Convert 3.50 moles of to HBO2  

=>

=>

=>

=>

=>11.0845