No 5 5. The reaction was studied at 25°C. The partial pressures at equilibrium were found to bePNOCI = 1.2 atm; PNO = 5.0 x 10-2 atm; Pc12 = 3.0 × 10-' atm; Calculate Kp for the reaction at%3D25°C.2NO(g) + Cl2(g) 5 2NOCI(g)6. Consider the following system at 100 °CN2O4 5 2NO2 Kp=11Predict the direction in which reaction will occur to reach equilibrium, starting with 0.10 atm ofN204 and 0.20 atm NO2 in a 2.0 L container.

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5. The reaction was studied at 25°C. The partial pressures at equilibrium were found to be PNOCI = 1.2 atm; PNO = 5.0 x 10 ² atm; Pc12 = 3.0 × 10-' atm; Calculate Kp for the reaction at %3D %3D 25°C. 2NO(g)+ Cl2(g) 5 2NOCI(g)

5. The reaction was studied at 25°C. The partial pressures at equilibrium were found to be PNOCI = 1.2 atm; PNO = 5.0 x 10 ² atm; Pc12 = 3.0 × 10-' atm; Calculate Kp for the reaction at %3D %3D 25°C. 2NO(g)+ Cl2(g) 5 2NOCI(g)

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

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Question

No 5

5. The reaction was studied at 25°C. The partial pressures at equilibrium were found to be
PNOCI = 1.2 atm; PNO = 5.0 x 10-2 atm; Pc12 = 3.0 × 10-' atm; Calculate Kp for the reaction at
%3D
25°C.
2NO(g) + Cl2(g) 5 2NOCI(g)
6. Consider the following system at 100 °C
N2O4 5 2NO2 Kp=11
Predict the direction in which reaction will occur to reach equilibrium, starting with 0.10 atm of
N204 and 0.20 atm NO2 in a 2.0 L container.

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