Sulfur dioxide gas (so2) reacts with excess oxygen gas (o2) and excess liquid water (h2o) to form liquid sulfuric acid (h2so4). in the laboratory, a chemist carries out this reaction with 67.2 l of sulfur dioxide and gets 250 g of sulfuric acid. • write a balanced equation for the reaction. • calculate the theoretical yield of sulfuric acid. • calculate the percent yield of the reaction. (one mole of any gas occupies 22.4 l under certain conditions of temperature and pressure. assume those conditions for this question.)

The balanced equation is as below

2SO₂ +O₂ +2H₂O →  2 H₂SO₄

 The theoretical yield of H₂SO₄  is   294 grams

   calculation

step 1 :find the  moles of SO₂

 That is at STP  1  moles = 22.4 L

                           ? moles = 67.2 L

by cross  multiplication

= (67.2 L  x 1  moles) / 22.4 L  = 3  moles

step 2: use  the  mole ratio to determine the  moles of H₂SO₄

from equation above the  mole ratio  of SO₂:H₂SO₄  is  2:2 = 1:1 therefore the moles of H₂SO₄  is also 3 moles

step 3: find the theoretical yield

theoretical yield= moles x  molar  mass

from periodic table the  molar mass of H₂SO₄  = (1 x2) + 32 + (16 x4) =98 g/mol

Theoretical yield = 3 moles x 98 g/mol = 294 grams

percent yield =  actual yield/ theoretical yield x 100

=( 250g / 294 g) x 100 = 85.03%

you need to take a look at the periodic system in order to sort these elements into pairs that would most likely exhibit similar chemical properties. first, you need to find elements that are found in the same group (groups are vertical in the periodic system), and then to see whether they have the same valence number. if they meet these criteria, they will have similar properties.

the first pair: ne (neon) and kr (krypton), are noble gases found in group 8

the second pair: li (lithium) and k (potassium), found in group 1

the third pair: s (sulfur) and te (tellurium), found in group 6

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