When Barium nitrate is heated it decomposes as follows:
Ba(NO3)2 (s) ? BaO (s) + 2NO2 (g) + 1/2O2 (g)
Calculate the mass of barium oxide which can be obtained by decomposing 5.00g of barium nitrate.
All help appreciated, thanks a lot.
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- Thread Starter
- 19-10-2015 19:08
- 19-10-2015 19:18
As moles =mass/ rfm, you can work out the moles of barium nitrate.
do 5/(the RFM of barium nitrate-which you can work out by adding all the mass numbers of the elements in it)= the moles of barium nitrate
The mole ratio is1:1 (which you can tell bc there is no number in front of the BaO, which means that there is one mole of that molecule.
Therefore, the mole number you just calculated = mass/(rfm of BaO)
So times (as you are rearranging the equation to get mass =)the mole number you calculated by the rfm of Bao to get the mass of BaO produced