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Chemistry 12 > 5.4 > Flashcards

5.4 Flashcards

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1
Q

Reactions Not at Equilibrium

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2
Q

•For the reaction conditions shown;

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3
Q

Concentration (M)

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4
Q

equilibrium is not reached until NO

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concentration

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5
Q

reaches 0.0125 mol/L

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6
Q

0.08

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7
Q

0.06

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8
Q

0.04

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9
Q

0.02

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10
Q

line

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11
Q

Time

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12
Q

(a)

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13
Q

Chemical

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14
Q

Equilibrium

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15
Q

N

A

o

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16
Q

NO.

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17
Q

2NO

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18
Q

P2 (3)

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19
Q

0.08

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20
Q

0.06

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21
Q

0.04

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22
Q

The Reaction Quotient

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23
Q

Keg

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24
Q

0.02

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25
Q

eq

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26
Q

0

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27
Q

Q-lT[D

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28
Q

[A|[B

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29
Q

Time

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30
Q

(bl

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31
Q

Chemical

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32
Q

•Reaction quotient (Q): a numerical value

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33
Q

determined by using the same formula as the

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34
Q

equilibrium constant (using data for a reversible

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35
Q

reaction) that may or may not be at equilibrium.

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36
Q

For: aA + bB cC + dD:

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37
Q

3-4/ 20

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38
Q

NO

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39
Q

Determining the Direction of a Reaction

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40
Q

NO

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41
Q

•The symbols forQ and K are placed on a number

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42
Q

•The reaction will move in the direction from Q to K.

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43
Q

eg

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44
Q

Determining the Direction of a Reaction

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45
Q

Q>K:

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46
Q

Determining the Direction ofa Rea( 67 /20

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47
Q

ratio of products

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48
Q

to reactants is

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49
Q

too large

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50
Q

reaction will

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51
Q

proceed LEFT to

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52
Q

reach

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53
Q

equilibrium.

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54
Q

Q=

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55
Q

[products]

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56
Q

[reactants]

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57
Q

Reaction proceeds

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58
Q

toward right

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59
Q

forming products

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60
Q

Example 1:

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61
Q

eqilitriur is

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62
Q

Q> K

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63
Q

net reaction to left

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64
Q

Reactions Not at Equl lilbrium

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65
Q

ui

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66
Q

The Reaction Quotlent

A

C

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67
Q

•Reaxtion ouotiernt (Q) a numerical value

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68
Q

using the sane torry

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69
Q

Q=

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70
Q

uil NO

A

:6centretion

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71
Q

tormuls zs the

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72
Q

raactlcnl that may or may nat be at equi lari am.

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73
Q

erminlng the Dlrectlon of a Reaction

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74
Q

K

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75
Q

Q=K:

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76
Q

Qand K

A

are olkced ur a uribe

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77
Q

raler wll mnes in the cirertiar fon Qto K

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78
Q

the system is at

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79
Q

equilibrium.

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80
Q

K= Q=

A
81
Q

[products]

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82
Q

[reactants]

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83
Q

Q= K

A
84
Q

Reaction proceeds

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85
Q

toward left

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86
Q

forming reactants

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87
Q

no net reaction

A
88
Q

Q<K:

A
89
Q

Determining the Direction of a Reaction

A
90
Q

ratio of products

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91
Q

Calculate Q to determine the direction of reaction when

A
92
Q

the concentrations are: [CH

A

]=0.100 M

93
Q

M

A

[H

94
Q

AAnilibciun constant for the reaction below is 5.67.

A
95
Q

to reactants is to0

A
96
Q

small

A

reaction

97
Q

will proceed

A
98
Q

RIGHT to reach

A
99
Q

equilibrium.

A
100
Q

Q=

A
101
Q

[products]

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102
Q

[reactants]

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103
Q

Q<K

A
104
Q

net reaction to right

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105
Q

CHạ (e) + H

A

O) Coig + 3H2()

106
Q

Example 2:

A
107
Q

Determining the direction of a Reaction

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108
Q

In the Haber process for manufacturing ammonia

A
109
Q

nitrogen and hydrogen combine in the presence of a

A
110
Q

catalyst:

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111
Q

Nzte) + 3H (a) 2NHa (e)

A
112
Q

At 300 °C

A

the value of K._ for this reaction is 7.3.

113
Q

eq

A
114
Q

The following concentrations of gases are present in

A
115
Q

a container at 300°C: [N

A

] = 0.10 mol/L

116
Q

mol/L

A

and [NH

117
Q

gases at equilibrium? If not

A

in which direction will

118
Q

the reaction go to reach equilibrium?

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119
Q

Example 3: Calculating Equilibrium

A
120
Q

Concentrations from Initial Concentration

A
121
Q

Carbon monoxide reacts with water vapour to

A
122
Q

produce carbon dioxide and hydrogen. At 900 °d

A
123
Q

K = 4.200. Calculate the concentrations of all

A
124
Q

entities at equilibrium if 4.000 mol of each entity

A
125
Q

are initially placed in a 1.000 L closed container.

A
126
Q

eo

A
127
Q

Step 1: Calculate concentrations given c=nv

A
128
Q

Step 2: Calculate the value of Q

A
129
Q

Example 3 Continued

A
130
Q

Step 3: Set up an ICE chart

A
131
Q

Determining the Direction of a Reactinn

A
132
Q

ERample

A
133
Q

Initial conc. (mol/L)

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134
Q

Determining the Direction of a

A
135
Q

pTcHad LEFT

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136
Q

ceullbdurh.

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137
Q

|Change in conc. (mol/4)

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138
Q

ratio of aradu.cti tha systam Is at rato of praeucts

A
139
Q

snall reacrior

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140
Q

BISHT OrE8th

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141
Q

ing the Direction af a neaction

A
142
Q

M. EH

A

O| 0.200 M and J]=0200 M

143
Q

onc.

A
144
Q

co(g)

A
145
Q

4

A
146
Q

= 4.000 mol/1.000 L

A
147
Q

= 4.000 M

A
148
Q

blve for X

A
149
Q

Q = [C0

A

][H

150
Q

= (4.000)(4.000)/(4.000)(4.

A
151
Q

= 1.000.. NOT at equilibril

A
152
Q

+ H

A

ole)

153
Q

4

A
154
Q

co

A

(e)

155
Q

4

A
156
Q

H

A

(e)

157
Q

4

A
158
Q

Step 1. Write the balanced equation for the reaction.

A
159
Q

Step 2. Under the balanced equation

A

make a table that lists for each substance

160
Q

involved in the reaction:

A
161
Q

(a) The initial concentration

A
162
Q

the

A
163
Q

(b) The change in concentration on going to equilibrium

A
164
Q

(c) The equilibrium concentration

A
165
Q

In constructing the table

A

define x as the concentration (mol/L) of one of

166
Q

he substances that reacts on going to equilibrium

A

then use the

167
Q

stoichiometry of the reaction to determine the concentrations of the other

A
168
Q

substances in terms of x.

A
169
Q

Step 3. Substitute the equilibrium concentrations into the equilibrium equation for

A
170
Q

the reaction and solve for x. If you must solve a quadratic equation

A
171
Q

choose the mathematical solution that makes chemical sense.

A
172
Q

Step 4. Calculate the equilibrium concentrations from the calculated value of x.

A
173
Q

Example 4

A
174
Q

Step 5. Check your results by substituting them into the equilibrium equation.

A
175
Q

Calculations with Imperfect Squares

A
176
Q

•The “thousand rule” is an assumption made to

A
177
Q

simplify problems:

A
178
Q

If the ratio of:

A
179
Q

[initial concentration of reactant]/Keq> 1000

A
180
Q

then x is very small compared to initial

A
181
Q

concentration

A

so it is considered negligible with

182
Q

respect to the change from the initial

A
183
Q

concentration

A

and x may be removed from that

184
Q

part of the calculation.

A
185
Q

**Note: this is nota great rule

A

but acceptable for high school

186
Q

chemistry

A
187
Q

Carbon monoxide is a primary starting material in the

A
188
Q

synthesis of many organic compounds

A

including

189
Q

methanol

A

CH

190
Q

13-14/ 20

A
191
Q

At 2000°C

A

K is 6.40 x 10 for the decomposition of

192
Q

carbon dioxide into carbon monoxide and oxygen.

A
193
Q

Calculate the concentrations of all entities at

A
194
Q

equilibrium if 0.250 mol/L of COo

A

lel is placed in a

195
Q

closed container and heated to 2000 °C.

A
196
Q

2C02 (8)

A
197
Q
  • 2C0e + Oz(e)
A

Chemistry 12 (6 decks)

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