The equilibrium constant (K) of the reaction below is K = 6.0 x 102, with initial concentrations as follows: [H2] = 1.0 x 102 M, [N2] = 4.0 M, and [NH3] = 1.0 x 10 M. N2(g) + 3H2(g) = 2NH3(g) 3. Consider the chemical reaction: N2 + 3H2yields 2NH3. If the concentration of the reactant H2 was increased from 1.0x 102 M to 2.5x 101 M, calculate the reaction quotient (Q) and determine which way the chemical system would shift by comparing the value of Q to K. B IU E T O Word(s) T II
The equilibrium constant (K) of the reaction below is K = 6.0 x 102, with initial concentrations as follows: [H2] = 1.0 x 102 M, [N2] = 4.0 M, and [NH3] = 1.0 x 10 M. N2(g) + 3H2(g) = 2NH3(g) 3. Consider the chemical reaction: N2 + 3H2yields 2NH3. If the concentration of the reactant H2 was increased from 1.0x 102 M to 2.5x 101 M, calculate the reaction quotient (Q) and determine which way the chemical system would shift by comparing the value of Q to K. B IU E T O Word(s) T II
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Answer 3 please
![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 10 M.
N2(g) + 3H2(g) = 2NH3(g)
3. Consider the chemical reaction: N2+ 3H2yields 2NH3. If the concentration of the reactant H2 was increased from
1.0x 102 M to 2.5x 101 M, calculate the reaction quotient (Q) and determine which way the chemical system would
shift by comparing the value of Q to K.
B IU E E T
T
O Word(s)
4. If the concentration of the reactant H2 was decreased from 1.0 x 10-2 M to 2.7 x 10-4 M, calculate the reaction
quotient (Q) and determine which way the chemical system would shift by comparing the value of Q to K.
B
T'
T
O Word(s)
5. If the concentration of the product NH3 was increased from 1.0x 104M to 5.6 x 103 M, calculate the reaction
quotient (Q) and determine which way the chemical system would shift by comparing the value of Q to K.
O Word(s)
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Transcribed Image Text: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 10 M.
N2(g) + 3H2(g) = 2NH3(g)
3. Consider the chemical reaction: N2+ 3H2yields 2NH3. If the concentration of the reactant H2 was increased from
1.0x 102 M to 2.5x 101 M, calculate the reaction quotient (Q) and determine which way the chemical system would
shift by comparing the value of Q to K.
B IU E E T
T
O Word(s)
4. If the concentration of the reactant H2 was decreased from 1.0 x 10-2 M to 2.7 x 10-4 M, calculate the reaction
quotient (Q) and determine which way the chemical system would shift by comparing the value of Q to K.
B
T'
T
O Word(s)
5. If the concentration of the product NH3 was increased from 1.0x 104M to 5.6 x 103 M, calculate the reaction
quotient (Q) and determine which way the chemical system would shift by comparing the value of Q to K.
O Word(s)
80
888
DII
FB
F11
23
&
2
3
4
5
6
7
8
9
-
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R
Y
U
{
P
D
G
H
J
K
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