Answer:
K = 3.3
Explanation:
Nitric acid, HNO3, reacts with nitrogen monoxide, NO, to produce nitrogen dioxide, NO2 and water H2O as follows:
2HNO3(g) + NO(g) → 3NO2(g) + H2O(g)
Where equilibrium constant, K, is:
K = [NO2]³[H2O] / [HNO3]²[NO]
<em>[] is the molar concentration of each species at equilibrium.</em>
To solve this question we need to find molarity of each gas and replace these in the equation as follows:
<em>[NO2] -Molar mass NO2-46.0g/mol-</em>
18.6g * (1mol/46.0g) = 0.404mol / 7.7L = 0.0525M
<em>[H2O] -Molar mass:18.01g/mol- </em>
236.7g * (1mol/18.01g) = 13.14 moles / 7.7L = 1.707M
<em>[HNO3] -Molar mass:53.01g/mol-</em>
16.2g * (1mol/53.01g) = 0.3056 moles / 7.7L = 0.0397M
<em>[NO] -Molar mass: 30.0g/mol-</em>
11.0g * (1mol/30.0g) = 0.367 moles / 7.7L = 0.0476M
Replacing:
K = [NO2]³[H2O] / [HNO3]²[NO]
K = [0.0525M]³[1.707M] / [0.0397M]²[0.0476M]
<h3>K = 3.3</h3>
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