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...

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:

5SF4+2I2O2-->4IF5 +5SO2

Please show your work!!!!!!! and explain really really really thoroughly!!!! thanks:) so much!!!

jeew-m | College Teacher | (Level 1) Educator Emeritus

Posted on

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

= 0.9711L

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