No 3 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) S 2NH3(g)2. The value of Kp at 25°C for the reaction is 1.9 x 10 atm. Calculate the value of Ke at thesame temperature.2NO(g) + Cl2 (g) 5 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-!. 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)

Answered: Image /qna-images/answer/97e84af2-64de-4805-8d50-e540ba7278f4.jpg

3. At equilibrium for the reaction, the concentrations of reactants and products at 727°C were found to be SO2 0.27 molL-I; O2 = 0.40 molL-; SO3 = 0.33 molL-I. What is the value of the equilibrium constant, Kc, at this temperature? %3D 2SO2(g) + O2 (g) = 2SO3 (g)

3. At equilibrium for the reaction, the concentrations of reactants and products at 727°C were found to be SO2 0.27 molL-I; O2 = 0.40 molL-; SO3 = 0.33 molL-I. What is the value of the equilibrium constant, Kc, at this temperature? %3D 2SO2(g) + O2 (g) = 2SO3 (g)

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 12.79PAE

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Question

100%

No 3

1. At 500°C, the reaction between N2 and H2 to form ammonia has Kc = 6.0 x 10-2. What is the
Kp for the reaction?
N2(g) + 3H2(g) S 2NH3(g)
2. The value of Kp at 25°C for the reaction is 1.9 x 10 atm. Calculate the value of Ke at the
same temperature.
2NO(g) + Cl2 (g) 5 2NOCI(g)
3. At equilibrium for the reaction, the concentrations of reactants and products at 727°C were
found to be SO2 0.27 molL-; O2 = 0.40 molL-1; SO3 = 0.33 molL-!. What is the value of the
equilibrium 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 are
found to be present. Find the value of Kc for the reaction at 500°C.
N2(g) + 3H2(g) 5 2NH3(g)

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