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For each of the following unbalanced equations, calculate how many grams of each product would be produced by complete reaction of 10.8 g of the second reactant. (a) S(s) + H2SO4(aq) → SO2(g) + H2O(l) SO2 WebAssign will check your answer for the correct number of significant figures. g H2O WebAssign will check your answer for the correct number of significant figures. g

User Belial
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1 Answer

4 votes

Answer:


10.6g of
SO_(2)


2.0g of
H_(2)O

Step-by-step explanation:

First we are going to balance the reaction:


S+_(2)H_(2)SO{4}=_(3)SO_(2)+_(2)H_(2)O

Then we are going to find the quantities with the stoichiometry:

-For
SO_(2):


10.8gH_(2)SO_(4)*(1molH_(2)SO_(4))/(98.079gH_(2)SO_(4))*(3molesSO_(2))/(2molesH_(2)SO_(4))*(64.066gSO_(2))/(1molSO_(2))=10.6gSO_(2)

-For
H_(2)O:


10.8gH_(2)SO_(4)*(1molH_(2)SO_(4))/(98.079gH_(2)SO_(4))*(2molesH_(2)O)/(2molesH_(2)H_(2)O)*(18.015gH_(2)O)/(1molH_(2)O)=10.6gH_(2)O=2.0gH_(2)O

User Mozes Ong
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