Question

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

Answer 1

Answer:

$10.6g$ of $SO_{2}$

$2.0g$ of $H_{2}O$

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 $SO_{2}$:

$10.8gH_{2}SO_{4}*\frac{1molH_{2}SO_{4}}{98.079gH_{2}SO_{4}}*\frac{3molesSO_{2}}{2molesH_{2}SO_{4}}*\frac{64.066gSO_{2}}{1molSO_{2}}=10.6gSO_{2}$

-For $H_{2}O$:

$10.8gH_{2}SO_{4}*\frac{1molH_{2}SO_{4}}{98.079gH_{2}SO_{4}}*\frac{2molesH_{2}O}{2molesH_{2}H_{2}O}*\frac{18.015gH_{2}O}{1molH_{2}O}=10.6gH_{2}O=2.0gH_{2}O$