00m 0 0 d x x x equilibrium 100x x x k c pcl3

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Unformatted text preview: N2 and O2 (fro m air): N2 (g) + ¾¾ ® O2 (g) ¬¾ ¾ 2 NO (g) Kc for this reaction equals 0.0025 at 2127 °C. If an equilibrium mixture at 2127 °C contains 0.023 mo l N2 and 0.031 mo l O2 per liter, what is the equilibrium concentration of NO? 2 [NO] K c = [NO]2 = K c [N 2 ][O 2 ] [N 2 ][O 2 ] [NO] = K c [N 2 ][O 2 ] = (0.0025)(0.023)(0.031) = 1.3x10­3 M Example 2: – The equilibrium shown below has a Kp value of 1.45x10 5 at 500 °C. In an equilibrium mixture of the three gases at this temperature, the partial pressure of H2 is 0.928 atm and that of N2 is 0.432 atm. What is the partial pressure of NH3 in this mixture? ¾¾ ® N2 (g) + 3 H2 (g) ¬¾ ¾ Kp = 17 2 NH3 (g) Chemistry 102 Chapter 14 Example 3: For the reaction shown below, init ially a mixture contains 0.850 mo l each of N2 and O2 in a 8.00 L vessel. Find the composit io n of the mixture when equilibrium is reached at 3900 °C. Kc = 0.0123 at 3900 °C ¾¾ ® N2 (g) + O2 (g) ¬¾ 2 NO (g) ¾ First: Obtain starting mo lar concentrations in mo l/L 0.850 mo...
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This document was uploaded on 03/18/2014 for the course CHEM 102 at Los Angeles Mission College.

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