Consider the equilibrium system described by the chemical reaction below. A 1.00 L reaction vessel was filled 0.0560 mol O: and 0.200 mol N:O and allowed to react at 298 K. At equilibrium, there were 0.0200 mol of NO: present. Determine the concentrations of all species and then calculate the value of Kc for this reaction. 2 N:O(g) + 3 O:(g) = 4 NO:(g) PREV Based on the set up of your ICE table, construct the expression for Kc and then evaluate it. Do not combine or simplify terms. K. = 2 RESET [0.200] [0.0560] [0.0200] [0.190] [0.0410] |0.0710] [0.0360] [0.180] (0.200F [0.0560] [0.0200]* [0.190 [0.0410]" 10.0710 [0.0360)" [0.180) 0.0643 2.57 15.6 0.390
Consider the equilibrium system described by the chemical reaction below. A 1.00 L reaction vessel was filled 0.0560 mol O: and 0.200 mol N:O and allowed to react at 298 K. At equilibrium, there were 0.0200 mol of NO: present. Determine the concentrations of all species and then calculate the value of Kc for this reaction. 2 N:O(g) + 3 O:(g) = 4 NO:(g) PREV Based on the set up of your ICE table, construct the expression for Kc and then evaluate it. Do not combine or simplify terms. K. = 2 RESET [0.200] [0.0560] [0.0200] [0.190] [0.0410] |0.0710] [0.0360] [0.180] (0.200F [0.0560] [0.0200]* [0.190 [0.0410]" 10.0710 [0.0360)" [0.180) 0.0643 2.57 15.6 0.390
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![Consider the equilibrium system described by the chemical reaction below. A 1.00 L reaction vessel was filled 0.0560 mol O: and 0.200 mol N:O and
allowed to react at 298 K. At equilibrium, there were 0.0200 mol of NO: present. Determine the concentrations of all species and then calculate the
value of Kc for this reaction.
2 N:O(g) + 3 O:(g) = 4 NO:(g)
PREV
2
Based on the set up of your ICE table, construct the expression for Kc and then evaluate it. Do not combine or simplify terms.
K. =
%3D
2 RESET
[0.200]
[0.0560]
[0.0200]
[0.190]
[0.0410]
[0.0710]
[0.0360]
[0.180]
[0.200]"
(0.0560]"
[0.0200]*
[0.190
(0.0410]"
[0.0710]"
[0.0360]
(0.180]
0.0643
2.57
15.6
0.390](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F1199fdc2-4d26-4f2c-8b62-c411e8b4637a%2F02450009-86e6-48fa-ad78-4c25caec7b75%2F6umqp2p_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Consider the equilibrium system described by the chemical reaction below. A 1.00 L reaction vessel was filled 0.0560 mol O: and 0.200 mol N:O and
allowed to react at 298 K. At equilibrium, there were 0.0200 mol of NO: present. Determine the concentrations of all species and then calculate the
value of Kc for this reaction.
2 N:O(g) + 3 O:(g) = 4 NO:(g)
PREV
2
Based on the set up of your ICE table, construct the expression for Kc and then evaluate it. Do not combine or simplify terms.
K. =
%3D
2 RESET
[0.200]
[0.0560]
[0.0200]
[0.190]
[0.0410]
[0.0710]
[0.0360]
[0.180]
[0.200]"
(0.0560]"
[0.0200]*
[0.190
(0.0410]"
[0.0710]"
[0.0360]
(0.180]
0.0643
2.57
15.6
0.390
Transcribed Image Text:Consider the equilibrium system described by the chemical reaction below. A 1.00 L reaction vessel was filled 0.0560 mol O: and 0.200 mol N:O and
allowed to react at 298 K. At equilibrium, there were 0.0200 mol of NO: present. Determine the concentrations of all species and then calculate the
value of Kc for this reaction.
2 N:O(g) + 3 O:(g) = 4 NO:(g)
NEXT
Based on the given values, fill in the ICE table to determine concentrations of all reactants and products.
2 N:O(g)
3 0:(g)
4 NO:(g)
Initial (M)
Change (M)
Equilibrium (M)
5 RESET
0.0560
0.200
-1.00
-0.0560
0.0200
-0.0200
0.0150
-0.0150
0.210
0.190
0.0100
-0.0100
-0.0050
0.0050
0.0410
0.0710
0.0360
0.180
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