Question

SO2 + Cl2 = SO2Cl2 If 8g of SO2 is mixed with 14.2g of Cl2, and one mole of SO2Cl2 is 135g, What is the number of moles in Cl2 (chlorine) and SO2 (sulfur dioxide)?

I don't understand how does knowing the mole for one of the products or reactants show the moles of things on the other side.

Thank you in advance.

Answer 1

We use the quotient....`"mass of stuff"/"molar mass of stuff"="number of moles of stuff"`

Explanation:

And certainly this is consistent dimensionally....for the given problem the quotient gives....

`(8.0*cancelg)/(64.07*cancelg*mol^-1)=0.125*mol`..with respect to sulfur dioxide, because `1/(mol^-1)=1/(1/(mol))=mol` as required....

And with respect to dichlorine, we got `(14.2*g)/(70.9*g*mol^-1)=0.197*mol`

And thus, with respect to the given stoichiometric equation....

`SO_2(g) + Cl_2(g) rarr SO_2Cl_2(g)`

....sulfur dioxide is present in DEFICIENCY, and there is a molar excess of `Cl_2`.

And so AT MOST we can form `0.125*mol` of `"sulfuryl chloride"`, a mass (given 100% yield) of ............

`0.125*molxx134.96*g*mol^-1=16.9*g`

Do you follow this treatment? The relationship between moles AND mass is quite explicit.

Is the given equation an example of a redox equation; why or why not?