HomeTextbook Notes300,000US110,000

CHEM 105bL Chapter 14: Chapter 14 - Chemical Equilibrium

64 views1 pages

2 Feb 2017

School

Department

Course

Professor

For unlimited access to Textbook Notes, a Class+ subscription is required.

Document Summary

A reversible rxn is a rxn that can proceed in the forwards and reverse directions. When the rate of the reverse rxn = the rate of the forwards rxn, dynamic equilibrium is reached. The equilibrium constant (k) for the rxn is defined as a ratio (at equilibrium) of the concentration of the products raised to their stoichiometric coefficients divided by the concentrations of the reactants raised to their stoichiometric coefficients. [(cid:3002)](cid:3276)[(cid:3003)](cid:3277) (for (cid:1853)(cid:1827)+(cid:1854)(cid:1828) (cid:1855)(cid:1829)+(cid:1856)(cid:1830)) constant means that the reactants are favored (left, reverse rxn) A large equilibrium constant means that the products are favored (right, forward rxn); a small equilibrium. Relationships between the equilibrium constant and the chem eqn. If you reverse the eqn, the equilibrium constant is inverted. If you multiply the coefficients in the eqn by a factor, raise the equilibrium constant to the same factor.

Related textbook solutions

Chemistry: Structure and Properties

ISBN: 9780134293936

Basic Chemistry

ISBN: 9780134138046

Principles of Chemistry Molecular Approach

ISBN: 9780134112831

Principles of Chemistry Molecular Approach

3rd Edition, 2014

ISBN: 9780321971944

Chemistry: Structure and Properties

ISBN: 9780134293936

Chemistry: A Molecular Approach

ISBN: 9780321809247

Chemistry: A Molecular Approach

ISBN: 9780134874371

Principles of Chemistry: A Molecular Approach

ISBN: 9780134895741

Chemistry: The Central Science

14th Edition, 2017

ISBN: 9780134414232

Related Documents

CHEM 105bL Lecture Notes - Lecture 7: Equilibrium Constant, Reversible Reaction, Dynamic Equilibrium

CHEM 105bL Lecture Notes - Lecture 3: Reversible Reaction, Rate Equation, Dynamic Equilibrium

cerisegiraffe538

CHEM 1032 Chapter Notes - Chapter 14: Inert Gas, Reaction Quotient, North American Racing Team

burgundyherring290

Related Questions

Calculate K at 298 K for the following reactions. Delta Gf kj/mol = NOg...... 86.60 NO2g........... 51 O2.....0 Part A : NO(g) + 1/2 O2(g)......>> NO2(g) ..(.I know the answer is 1.7 x 10^6) Part B) Use the equilibrium constant ( K= 3.89 x 10^-34 at 298K ) to calculate Delta G (in kJ) at 298 for the following reaction: 2HCL (g)....> H2 (g) + CL2 (g) answer delta G in kJ and in scientific notation please.... NOTE:... the answer to part a is correct, the answer to part b is NOT.-1.90 x 10^2 it said HInt: For any state function (G, H, or S) the change in the state function, F, for a reaction can be calculated from Delta F rxn= (sideways M)n x delta F (products) minus (sideways M) n x delta F (reactants), when n are the stoichiometric coefficients from the balanced chemical equation. Use this expression to calculate Delta G rxn. Use the expression that relates change in fuel energy of a reaction, Delta G rxn, to the equilibrium constant K. I just need part B.....thanks. View comments ...part of the answer to part B is ............10^2 Comments You commented it said ^2 not ^-2 in the answer.......sorry

ENT ives To determine equilibrium concentrations for species in solution . Examine temperature effects on reaction equilibrium Investigate the shift in equilibrium from different stresses on a system kills . Use colorimeter to determine unknown solution concentrations ced .Preparing temperature baths to change reaction conditions tionEquilibrium is defined as a state in which the concentrations of both the reactants and products have no tendency to change with time. We can restate this by saying that the rate of the forward reaction is equal to the rate of the reverse reaction. Recall that with rate we are simply defining how fast a reaction is proceeding, a speed at which the reaction proceeds. Take note that when writing an equilibrium expression, pure liquids (denoted by l or 2) and pure solids (denoted by s) are omitted. Typically we express the equilibrium by K or Kp where c and p denote either concentration or partial pressure respectively. We refer to this value of K, or Kp as an equilibrium constant For any reaction, Kc can be written as the product of the concentration of products, raised to their stoichiometric coefficients, divided by the product of the concentration of the reactants raised to their stoichiometric coefficients. See Equation (5-1) below for an example: aA(aq) + bB(aq-cC(aq) + dD(aq) (5-1) A] [B]b As mentioned before, K, or K, are equilibrium constants meaning that they will have the same value unless temperature is changed. This brings in two important ideas 1) We can perturb the equilibrium concentrations of a reaction, say [A] for instance which will cause the other concentrations to shift so that K for the reaction remains constant. 2) If we change temperature, we will either increase or decrease our value of K depending on the specific reaction we are examining. Determining K, and Equilibrium Concentrations During lecture we often discuss the idea of using ICE tables as a method for organizing and calculating concentrations of reactions as they proceed towards equilibrium. In a typical ICE table you need to know initial concentrations and the magnitude of K to determine the equilibrium concentrations. Alternatively, if you know the equilibrium concentrations for a reaction you can calculate K. For this experiment we will be examining a complex ion formation, when iron(III) ion

1) Express the equilibrium constant for the following reaction?

2) For the reaction of carbon with carbon dioxide to make carbon monoxide, the reaction is as follows.

Write the equilibrium constant expression for the K_c?

3) Which of the following statements is FALSE?

a) When K is very large, the forward reaction is favored and essentially goes to completion.

b) None of the answers are correct.

c) If K is very large it implies that the reaction is very fast at producing products.

d) When K is very small, the reverse reaction is favored and the forward reaction does not proceed to a great extent.

4)The equilibrium constant for the production of carbon dioxide from carbon monoxide and oxygen is 2 x 10¹¹.

This means that the reaction mixture at equilibrium is likely to consist of

a) mostly starting materials.

b) twice as much starting material as a product.

c) mostly products.

d) twice as much product as starting material.