80if0100molo fpcl5 isaddedtoa500lflaskwhat

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Unformatted text preview: es of NOBr and NO are equal at equilibrium, what is the partial pressure of Br2? P 2 O P r2 N B K p = P 2 OBr N = 0.416 since PNOB r = P O N PBr2 = 0.416 atm 5. At 250°C, the reaction ˆˆ PCl5 (g) ‡ˆ† PCl3 (g) + Cl2 (g) has an equilibrium constant Kc= 1.80. If 0.100 mol o f PCl5 is added to a 5.00­L flask, what are the concentrations of PCl5, PCl3 and Cl2 at equilibrium at this temperature? [PCl 5 ] = 0 . 1 0 0 m o l = 0.0200 M 5.00 L ˆ ˆˆ PCl5 (g) ‡ˆ† PCl3 (g) + Cl2 (g) Initial D Equilibrium 0.0200 M – x 0.0200 –x 0 + x x 2 [PCl 3 ][Cl 2 ] x K C = = = 1.80 [PCl 5 ] 0.0200 ­x x 2 + 1.80 x ­ 0.0360 = 0 Solving the quadratic equation, ­1.80 ± (1.80)2 ­4(­0.0360) = 0.0198 2 [PCl 3 ]=[Cl 2 ]= 0.0198 M x = [PCl 5 ]= 0.0200 ­ 0.0198 = 0.0002 M 2 0 + x x 6. When 2.00 mo l each of hydrogen and iodine are mixed in a 1.00­L flask, 3.50 mo l of HI is produced at equilibrium: ˆˆ H2 (g) + I2 (g) ‡ˆ† 2 HI (g) Calculate the equilibrium constant Kc for this reactio n. ˆˆ H2 (g) + I2 (g) ‡ˆ† 2 HI (g) 2.00 M 2.00 M 0 – 1.75 – 1.75 + 3.50 0.25 0.25 3.50 Initial D Equilibrium 2 [HI]2 (3.50) K C = = = 196 2 [H 2 ] [I 2 ] (0.25) 7. The equilibrium constant for the reaction ˆˆ SO2 (g) + NO2 (g) ‡ˆ† SO3 (g) + NO (g) has a numerical value o f 3.00 at a given temperature. 1.50 mo...
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