50.0 L. Initially, there will be the same number of moles of each of the gases that were present at equilibrium. However, they are now in a larger volume, so their ooncentrations will change. a) Determine the new concentrations of N. H and NH. IN = INH. =. Using these new Initial concentrations, determine the value of Q. the reaction quotient b)
50.0 L. Initially, there will be the same number of moles of each of the gases that were present at equilibrium. However, they are now in a larger volume, so their ooncentrations will change. a) Determine the new concentrations of N. H and NH. IN = INH. =. Using these new Initial concentrations, determine the value of Q. the reaction quotient b)
Physical Chemistry
2nd Edition
ISBN:9781133958437
Author:Ball, David W. (david Warren), BAER, Tomas
Publisher:Ball, David W. (david Warren), BAER, Tomas
Chapter5: Introduction To Chemical Equilibrium
Section: Chapter Questions
Problem 5.19E: 5.19. Assume that a reaction exists such that equilibrium occurs when the partial pressures of the...
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1 N2 + 3H2 = 2NH3
![Starting with 0.500 M N; and 0.800 M Hz, the resction is allowed to
proceed until it resches equilibrium. The [NHa = 0.150 M at 250°C.
Determine K for this reaction at this temperature.
4.
Start by filling in the ICE table with the Initial concentrations.
Resction
[N] (M)
[H] (M)
[NH) (M)
Initial
0.500 M
0.800 M
Change
-3x
+2x
Equilibrium
0.500 M
0.800 M-3x
+2x
b)
Next, fill in the Changes in the system, in terms of x, which
will determined by the stoichiometry. Reactants are used
up (-) and products are formed (+).
c)
Next, write equilibrium expressions, in terms of initial
concentrations and the changes that occur (x).
d)
Solve for x from the information you have.
2x=0.150 M
x=0.150 M/2
0.075 M
e)
Determine the equilibrium concentrations of N and Hz-
[N:] = 0.500 M-x
= 0.500 M - 0.075 M
[N 0.425 M
[H] = 0.800 M - 3x
= 0.800 M - 3(0.075 M)
= 0.800 M - 0.225 M
[Hln=_0.575 M](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F1879c863-4338-45b6-a871-ee02c45f0c5b%2F8961cfef-65cb-4c54-9c1d-2fbb536ed60f%2F215crwy_processed.png&w=3840&q=75)
Transcribed Image Text:Starting with 0.500 M N; and 0.800 M Hz, the resction is allowed to
proceed until it resches equilibrium. The [NHa = 0.150 M at 250°C.
Determine K for this reaction at this temperature.
4.
Start by filling in the ICE table with the Initial concentrations.
Resction
[N] (M)
[H] (M)
[NH) (M)
Initial
0.500 M
0.800 M
Change
-3x
+2x
Equilibrium
0.500 M
0.800 M-3x
+2x
b)
Next, fill in the Changes in the system, in terms of x, which
will determined by the stoichiometry. Reactants are used
up (-) and products are formed (+).
c)
Next, write equilibrium expressions, in terms of initial
concentrations and the changes that occur (x).
d)
Solve for x from the information you have.
2x=0.150 M
x=0.150 M/2
0.075 M
e)
Determine the equilibrium concentrations of N and Hz-
[N:] = 0.500 M-x
= 0.500 M - 0.075 M
[N 0.425 M
[H] = 0.800 M - 3x
= 0.800 M - 3(0.075 M)
= 0.800 M - 0.225 M
[Hln=_0.575 M
![5.
Now, imagine that the volume of the container increases from 10.0 L to
50.0 L. Initially, there will be the same number of moles of each of the
gases that were present at equilibrium. However, they are now in a larger
volume, so their cancentrations will change.
a)
Determine the new concentrations of N., He and NH..
(N] =
[H] =
[NH.) =.
Using these new Initlal concentrations, detemine the value of Q,
the reaction quotient
Compare Q to K. Which way will the reaction proceed, under these
new experimental conditions?
c)
d)
Compare the number of moles of gas on the reactant and product
sides of the equation. Circle the correct answers in the statement
bekow.
Increasing the volume of the system shifts the equilibrium toward
the reactants / products, which has a larger / amaller number of
moles of gas](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F1879c863-4338-45b6-a871-ee02c45f0c5b%2F8961cfef-65cb-4c54-9c1d-2fbb536ed60f%2Fyw6h5yh_processed.png&w=3840&q=75)
Transcribed Image Text:5.
Now, imagine that the volume of the container increases from 10.0 L to
50.0 L. Initially, there will be the same number of moles of each of the
gases that were present at equilibrium. However, they are now in a larger
volume, so their cancentrations will change.
a)
Determine the new concentrations of N., He and NH..
(N] =
[H] =
[NH.) =.
Using these new Initlal concentrations, detemine the value of Q,
the reaction quotient
Compare Q to K. Which way will the reaction proceed, under these
new experimental conditions?
c)
d)
Compare the number of moles of gas on the reactant and product
sides of the equation. Circle the correct answers in the statement
bekow.
Increasing the volume of the system shifts the equilibrium toward
the reactants / products, which has a larger / amaller number of
moles of gas
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