Use this information to answer Questions 3, 4, and 5: The equilibrium constant (K) of the reaction below is K = 6.0 x 10-2, with initial concentrations as follows: [H2] = 1.0 x 102 M, [N2] = 4.0 M, and [NH3] = 1.0 x 104M. N2(g) + 3H2(g) = 2NH3(g) 3. Consider the chemical reaction: N2 + 3H2yields 2NH3. If the concentration of the reactant H2 was increased from 1.0 x 102 M to 2.5 x 10²M, calculate the reaction quotient (Q) and determine which way the chemical system would shift by comparing the value of Q to K. T' T. O Word(s) III !!!

Use this information to answer Questions 3, 4, and 5: The equilibrium constant (K) of the reaction below is K = 6.0 x 10-2, with initial concentrations as follows: [H2] = 1.0 x 102 M, [N2] = 4.0 M, and [NH3] = 1.0 x 104M. N2(g) + 3H2(g) = 2NH3(g) 3. Consider the chemical reaction: N2 + 3H2yields 2NH3. If the concentration of the reactant H2 was increased from 1.0 x 102 M to 2.5 x 10²M, calculate the reaction quotient (Q) and determine which way the chemical system would shift by comparing the value of Q to K. T' T. O Word(s) III !!!

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter17: Equilibrium

Section: Chapter Questions

Problem 7ALQ: The value of the equilibrium constant, K, is dependent on which of the following? (There may be more...

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. Explain what it means that a reaction has reached a state of chemical equilibrium. Explain why equilibrium is a dynamic state: Does a reaction really “stop” when the system reaches a state of equilibrium? Explain why, once a chemical system has reached equilibrium, the concentrations of all reactants remain constant with time. Why does this constancy of concentration not contradict our picture of equilibrium as being dynamic? What happens to the rates of the forward and reverse reactions as a system proceeds to equilibrium from a starting point where only reactants are present?
Explain that equilibrium is dynamic, and that at equilibrium the forward and backward reaction rates are equal.
During an experiment with the Haber process, a researcher put 1 mol N2 and 1 mol H2 into a reaction vessel to observe the equilibrium formation of ammonia, NH3. N2(g)+3H2(g)2NH3(g) When these reactants come to equilibrium, assume that x mol H2 react. How many moles of ammonia form?
In Section 13.1 of your text, it is mentioned that equilibrium is reached in a closed system. What is meant by the term closed system. and why is it necessary to have a closed system in order for a system to reach equilibrium? Explain why equilibrium is not reached in an open system.
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