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An engineer examining the oxidation of SO₂ in the manufacture of sulfuric acid determines that Kc = 1.7x10⁸ at 600. K:
2SO₂(g) + O₂(g) ⇄ 2SO₃(g)(b) The engineer places a mixture of 0.0040 mol of SO₂ (g) and 0.0028 mol of O₂ (g) in a 1.0-L container and raises the temperature to 1000 K. At equilibrium, 0.0020 mol of SO₃ (g) is present. Calculate Kc and PSO₂ for this reaction at 1000. K.

Respuesta :

Nitric oxide (NO) is the catalyst used for the oxidation of SO2​ to SO3​ in the lead chamber process for the manufacture of sulphuric acid.

Nitric oxide

The volume of flask =10 liter

(a)    2SO2​+O2​⇌2SO3​K=100

At an x       a

end   a/10  x/10    a/10

const KC​=(x/10)(a/10)2(a/10)2​=100

1001​=10x​⇒x=1/10

0.1 moles of O2​ are present .

(b)  2SO2​+O2​⇌2SO3​

At an x       2a

eq   a/10  x/10  2a/10

contact

KC​=(x/10)(a/10)2(102a​)2​⇒x/104​=100

x=4/10=0.4 moles of O2​.

To learn more about Nitric oxide visit the link

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