Question

If 0.500 moles of carbon disulfide reacts with oxygen completely according to the following reaction what would the total volume of the products be at 25°C and 4.23 atm?

Answer 1

$CS_2 + 3O_2 → CO_2 + 2SO_2$

Here we are given that 0.5 moles of carbon disulphide is given and lets assume that oxygen is in excess

As the stochiometric coefficient ratio of carbon disulphide to carbondioxide is 1:1 and to that of sulphur dioxide is 1:2

Then moles of carbondioxide formed will be 0.5 moles and sulphur dioxide formed will be 1 moles

Then total moles formed will be (0.5+1)moles=1.5 moles

$pV=nRT\\4.23\times V=1.5\times0.082\times298\\\\V=8.67 \ litres$