Le Châtelier's Principle: Concentration Stress N2(g) + 3 H2(g) 2 NH3(g) Which way does the react proceed? A) Forward B) Reverse C) Neither D) Can't say • Add more N2 Which way does the react proceed? • Add more NH3 A) Forward B) Reverse C) Neither D) Can't say Which way does the react proceed? • Remove NH3 as its formed A) Forward B) Reverse C) Neither D) Can't say

Le Châtelier's Principle: Concentration Stress N2(g) + 3 H2(g) 2 NH3(g) Which way does the react proceed? A) Forward B) Reverse C) Neither D) Can't say • Add more N2 Which way does the react proceed? • Add more NH3 A) Forward B) Reverse C) Neither D) Can't say Which way does the react proceed? • Remove NH3 as its formed A) Forward B) Reverse C) Neither D) Can't say

Introductory Chemistry For Today

8th Edition

ISBN:9781285644561

Author:Seager

Publisher:Seager

Chapter8: Reaction Rates And Equilibrium

Section: Chapter Questions

Problem 8.56E

See similar textbooks

Similar questions

. 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?
Consider the equilibrium process depicted in Fig. 17.6. When does the equilibrium state occur?
Explain why the hydration process for concrete is exothermic by considering the chemical bonds in the reactants and products.
For a chemical reaction to take place, some or all chemical bonds in the reactants must break, and new chemical bonds must form among the participating atoms to create the products. Write a simple chemical equation of your own choice, and list the bonds that must be broken and the bonds that must form for the reaction to lake place.
Acetic acid is a weak acid that reacts with water according to this equation: CH3CO2H(aq)+H2O(aq)H3O+(aq)+CH3CO2(aq) Will any of the following increase the percent of acetic acid that reacts and produces CH3CO2 ion? (a) Addition of HCI (b) Addition of NaOH (c) Addition of NaCH3CO2
Explain that equilibrium is dynamic, and that at equilibrium the forward and backward reaction rates are equal.
For the simple reaction 2H2(g)+O2(g)2H2O(l)list the types of bonds that must be broken and the types of bonds that must form for the chemical reaction to take place.
The boxes shown below represent a set of initial conditions for the reaction: Draw a quantitative molecular picture that shows what this system looks like after the reactants are mixed in one of the boxes and the system reaches equilibrium. Support your answer with calculations.
According to the Resource Conservation and Recovery Act (RCRA), waste material is classified as toxic and must be handled as hazardous if the lead concentration exceeds 5 mg/L. By adding chloride ion, the lead ion will precipitate as PbCl2, which can be separated from the liquid portion. Once the lead has been removed, the rest of the waste can be sent to a conventional waste treatment facility. How many grams of sodium chloride must be added to 500 L of a waste solution to reduce the concentration of the Pb2+ ion from 10 to 5 mg/L?
What is the law of mass action? Is it true that the value of K depends on the amounts of reactants and products mixed together initially? Explain. Is it true that reactions with large equilibrium constant values are very fast? Explain. There is only one value of the equilibrium constant for a particular system at a particular temperature, but there is an infinite number of equilibrium positions. Explain.
. What does it mean to say that a state of chemical or physical equilibrium is dynamic?
When writing an equation, how is a reversible reaction distinguished from a nonreversible reaction?