5. If the concentration of the product NH3 was Increased from 1.0x 104 M to 5.6 x 10 M, calculate the reaction quotlent (Q) and determine which way the chemical system would shift by comparing the value of Q t K.
5. If the concentration of the product NH3 was Increased from 1.0x 104 M to 5.6 x 10 M, calculate the reaction quotlent (Q) and determine which way the chemical system would shift by comparing the value of Q t K.
Introduction to General, Organic and Biochemistry
11th Edition
ISBN:9781285869759
Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres
Publisher:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres
Chapter7: Reaction Rates And Chemical Equilibrium
Section: Chapter Questions
Problem 7.81P
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I need help with question 5!
![3. Consider the chemical reaction: N2+3H2ylelds 2NH3. If the concentratlon of the reactant H2 was increased
from 1.0x 102 M to 2.5x 101 M, calculate the reaction quotlent (Q) and determine which way the chemical
system would shift by comparlng the value of Q to K.
B IU E
E T T,
34 Word(s)
[NH3]^2/[N2]x[H2]^3 Q1 = (1.0x10^-4)^2/4.0x(1.0x10^-2)^3
= 0.25x10^-2
(1.0x10^-4)^2/(4.0)x2.5x10^-1^3
=10^-5/4x2.5^3x10^-3
Q2 =
=10^-6
Q will be less than K because the volume of Q will be decreased compared to the volume of k which will
create a forward reaction.
4. If the concentration of the reactant H, was decreased from 1.0 x 102 M to 2.7x 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.
BI U
T
T
18 Word(s)
(1.0x10^-4Y 2/4.0x2.7x10^-4)^3
= 092x10^4
=9.2x10^2
K will be less than Q. so the reaction with proceed in a reverse direction.
5. If the concentration of the product NH3 was Increased from 1.0x 104 M 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.
T
O Word(s)
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Transcribed Image Text:3. Consider the chemical reaction: N2+3H2ylelds 2NH3. If the concentratlon of the reactant H2 was increased
from 1.0x 102 M to 2.5x 101 M, calculate the reaction quotlent (Q) and determine which way the chemical
system would shift by comparlng the value of Q to K.
B IU E
E T T,
34 Word(s)
[NH3]^2/[N2]x[H2]^3 Q1 = (1.0x10^-4)^2/4.0x(1.0x10^-2)^3
= 0.25x10^-2
(1.0x10^-4)^2/(4.0)x2.5x10^-1^3
=10^-5/4x2.5^3x10^-3
Q2 =
=10^-6
Q will be less than K because the volume of Q will be decreased compared to the volume of k which will
create a forward reaction.
4. If the concentration of the reactant H, was decreased from 1.0 x 102 M to 2.7x 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.
BI U
T
T
18 Word(s)
(1.0x10^-4Y 2/4.0x2.7x10^-4)^3
= 092x10^4
=9.2x10^2
K will be less than Q. so the reaction with proceed in a reverse direction.
5. If the concentration of the product NH3 was Increased from 1.0x 104 M 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.
T
O Word(s)
hp
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