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Jlenok [28]
3 years ago
8

References Use the References to access important values if needed for this question A student ran the following reaction in the

laboratory at 1185 K: 2sO (g)+O2(8)2s05(8) When she introduced 8.19x102 moles of So,(g) and 8.10x10 moles of O2(g) into a 1.00 liter container, she found the equilibrium concentration of O2(g) to be 5.98x102 M. Calculate the equilibrium constant, Ke she obtained for this reaction. Ke Submit Answer
Chemistry
1 answer:
ANTONII [103]3 years ago
4 0

Answer:

19.27

Explanation:

Some values are corrected from correct source.Thus,

Moles of SO₂ = 8.19x10⁻² moles

Moles of O₂ = 8.10x10⁻² moles

Volume = 1 L

Molarity=\frac{Moles\ of\ solute}{Volume\ of\ the\ solution}

Concentration of SO₂ = 8.19x10² M

Concentration of O₂ = 8.10x10 M

Considering the ICE table for the equilibrium as:

                    2SO₂ (g) +    O₂ (g)     ⇔          2SO₃ (g)

t = o              8.19x10⁻²      8.19x10⁻²

t = eq                -2x                  -x                      2x

--------------------------------------------- --------------------------

neq:    8.19x10⁻² -2x       8.19x10⁻² -x                      2x

Given:  

Equilibrium concentration of  O₂ = 5.98x10⁻² M  = 8.19x10⁻² -x

Thus, x = 0.0212 M

[SO₂] = 8.19x10⁻² - 2*0.0212 = 0.0395 M

[SO₃] = 2*0.0212 = 0.0424 M

The expression for the equilibrium constant is:

K_c=\frac {[SO_3]^2}{[SO_2]^2[O_2]}  

K_c=\frac{{0.0424}^2}{{0.0395}^2\times 0.0598}  

K = 19.27

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150 gO_2*\frac{1molO_2}{32gO_2} *\frac{8molCO_2}{13molO_2} =2.8846molCO_2

Clearly, we see that 2.8846 < 2.8896, which means that oxygen is the limiting reactant. In other words, the most products can be made when the oxygen is all used up.

Now let's finally convert moles of carbon dioxide into grams by multiplying by its molar mass, which is 12.01 + 2 * 16 = 44.01 g/mol:

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Notice that we have 3 significant figures because we had 3 significant figures at the start with 150. grams of oxygen.

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