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A sample of gas contains 0.1900 mol of CO(g) and 0.1900 mol of NO(g) and occupies a volume of 22.0 L. The following reaction takes place: 2CO(g) + 2NO(g)2CO2(g) + N2(g) Calculate the volume of the sample after the reaction takes place, assuming that the temperature and the pressure remain constant.

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Answer:

V₂ = 16.5 L

Explanation:

To solve this problem we use Avogadro's law, which applies when temperature and pressure remain constant:

V₁/n₁ = V₂/n₂

In this case, V₁ is 22.0 L, n₁ is [mol CO + mol NO], V₂ is our unknown, and n₂ is [mol CO₂ + mol N₂].

  • n₁ = mol CO + mol NO = 0.1900 + 0.1900 = 0.3800 mol

We use the reaction to calculate n₂:

2CO(g) + 2NO(g) → 2CO₂(g) + N₂(g)

  • mol CO₂:

0.1900 mol CO * [tex]\frac{2molCO_{2}}{2molCO} =[/tex] 0.1900 mol CO₂

  • mol N₂:

0.1900 mol NO * [tex]\frac{1molN_{2}}{2molNO} =[/tex] 0.095 mol N₂

  • n₂ = mol CO₂ + mol N₂ = 0.1900 + 0.095 = 0.2850 mol

Calculating V₂:

22.0 L / 0.3800 mol = V₂ / 0.2850 mol

V₂ = 16.5 L

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