Need Chemistry Help!!!! On finding liters in an equation using moles, etc. not that scary, though. please help.
How many liters of sulfur dioxide are formed when 4.68 g of sulfur tetrafloride reacts with 6.28 g of diiodine pentoxide to produce iodine pentafloride and sulfur dioxide? Balance equation:
I already balanced it :
Please show your work!!!!!!! and explain really really really thoroughly!!!! thanks:) so much!!!
For this question we need to know the mass of a mole of following substances.
`SF_4` = 108g/mol
`I_2O_2` = 286g/mol
`IF_5 ` = 222g/mol
`SO_2` = 64g/mol
Now lets see how many moles of each substance contain bofore the reaction starts.
number of `SF_4` moles = 4.68/108 mol = 0.043333 mol
Number of `I_2O_2` moles = 6.28/286 mol = 0.0219 mol
In the reaction as you found earlier;
Moles ratio of `SF_4:I_2O_2` = 5:2
So 5 moles of `SF_4` require 2 moles of `I_2O_2` to full reaction.
In our sample we need 0.043333/5*2 moles of I-2O-2 for reaction.
So required `I_2O_2` = 0.043333/5*2 = 0.0173 mol
We have 0.0219 moles but we need only 0.0173 moles. So the full reaction will takes place.
Moles ratio of `SF_4:SO_2` =1:1
So number of `SO_2` moles produced = 0.043333
If we assume standard temperature and pressure conditions and `SO_2` have ideal gas performance the volume of a mole is 22.414L
So Volume of `SO_2` = 22.414/1*0.04333