CHEM 112 Lecture Notes - Lecture 8: Gas Constant, Quadratic Formula, Dihydrogen Cation

44 views2 pages

periwinklegoose372

12 Feb 2017

School

Department

Course

Professor

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

Document Summary

Note that r= . 08205 when in terms of gas constant. Comparison to see whether it is at equilibrium. If q does not equal k it is not in equilibrium reactants must be converted to product for reaction to obtain equilibrium. If q is less than k: reaction is in forward direction, reactants still need to be converted to product to reach equilibrium. If q is equal to k: the reaction is in equilibrium. If q is larger than k: reaction is in reverse direction, products still need to be converted to reactants to reach equilibrium. To find equilibrium concentrations use the formula: k= products/reactants. Don"t forget to raise products and reactants to the coefficient in front of them. To solve: take square root of both sides. When you find what x equals, this is not the answer. Must plug x back in, in order to find the equilibrium concentration.

Related Questions

Consider the following reaction where K_c = 77.5 at 600 K.

CO(g) + Cl₂(g) <---->COCl₂(g)

A reaction mixture was found to contain 2.42Ã10^-2 moles of CO(g), 3.94Ã10^-2 moles of Cl₂(g) and 0.116 moles of COCl₂(g), in a 1.00 liter container.

Is the reaction at equilibrium?
If not, what direction must it run in order to reach equilibrium?

The reaction quotient, Q_c, equals________ .

The reaction________
A. must run in the forward direction to reach equilibrium.
B. must run in the reverse direction to reach equilibrium.
C. is at equilibrium.

1) If the temperature of an endothermic reaction at equilibriumcould be increased instantaneously, what would be the instantaneouseffect on Q and K before equilibrium was againachieved?

a.	Q would increase and K would stay thesame.
b.	Q would decrease and K would stay thesame.
c.	Q would stay the same and K wouldincrease.
d.	Q would stay the same and K woulddecrease.
e.	Both Q and K would stay the same.

2) Which of the following is true regarding the effect of acatalyst on chemical equilibrium?

a.	Only the forward rate increases so the quantity of productsincreases.
b.	Only the forward rate increases but the quantity of productsremains the same.
c.	Both the forward and reverse rates increase and the quantity ofproducts increases.
d.	Both the forward and reverse rates increase but the quantity ofproducts is unchanged.
e.	The effect varies depending on whether the reaction isendothermic or exothermic.

3) The equilibrium constant for a given reaction __________

a.	does not change with temperature.
b.	always increases with temperature.
c.	always decreases with temperature.
d.	increases with temperature for exothermic reactions only.
e.	increases with temperature for endothermic reactions only,

Fill in the blanks

1) Chemical equilibrium arises from the __________ of chemicalreactions and is defined when the __________ of the forwardreaction is equal to the __________ of the reverse reaction.

2) Students often write expressions for the equilibrium constantK_c and reaction quotient Q_cin exactly the same way. To avoid confusion, you must rememberthatK_c uses concentrations under __________conditions while Q_c uses concentrations under__________ conditions.

3) If Q for a reaction is greater than K, thereaction will be __________. If Q for a reaction is lessthan K, the reaction will be __________. If Q fora reaction is equal to K, the reaction will be__________.

4) How and why are the expressions for homogeneous equilibriumconstants different from the expressions for heterogeneousequilibrium constants?

CHEM 112 Lecture Notes - Lecture 8: Gas Constant, Quadratic Formula, Dihydrogen Cation

Document Summary

Get access

Related textbook solutions

Chemistry: Structure and Properties

Basic Chemistry

Principles of Chemistry Molecular Approach

Chemistry: Structure and Properties

Principles of Chemistry Molecular Approach

Chemistry: A Molecular Approach

Chemistry: A Molecular Approach

Principles of Chemistry: A Molecular Approach

Chemistry: The Central Science

Related Documents

CHEM 112 Chapter 15: Chem 112 chapter 15

CHEM 112 Study Guide - Final Guide: Reaction Rate, Ideal Gas, Reagent

CHEM 112 Lecture Notes - Lecture 7: Equilibrium Constant

Related Questions