No 2 1. At 500°C, the reaction between N2 and H2 to form ammonia has Kc = 6.0 x 10-2. What is theKp for the reaction?N2(g) + 3H2(g) 5 2NH3(g)2. The value of Kp at 25°C for the reaction is 1.9 x 103 atm. Calculate the value of Ke at thesame temperature.2NO(g) + Cl2 (g) S 2NOCI(g)3. At equilibrium for the reaction, the concentrations of reactants and products at 727°C werefound to be SO2 0.27 molL-; O2 = 0.40 molL-1; SO3 = 0.33 molL-I. What is the value of theequilibrium constant, Ke, at this temperature?2SO2(g) + O2 (g) 2SO3 (g)4. Some nitrogen and hydrogen gases are pumped into an empty 5 litre glass bulb at 500°C.When equilibrium is established, 3.00 moles of N2, 2.10 moles of H2 and 0.298 mole of NH3 arefound to be present. Find the value of Kc for the reaction at 500°C.N2(g) + 3H2(g) 5 2NH3(g)

question no.2 ( as instructed) Kp and Kc both are equilibrium constant. Kp comes in terms of…

Answered: 2. The value of Kp at 25°C for the…

2. The value of Kp at 25°C for the reaction is 1.9 x 103 atm. Calculate the value of Ke at the same temperature. 2NO(g)+ Cl2 (g) 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

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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