Consider the reaction of NO and O, described by the chemical reaction below. Determine the equilibrium constant for this reaction by constructing an ICE table, writing the equilibrium constant expression, and solving it. Complete Parts 1-2 before submitting your answer. 2 N₂O(g) + 3 O₂(g) = 4 NO₂(g) NEXT A 1.00 L reaction vessel was filled with 0.0560 mol O₂ and 0.200 mol N₂O and allowed to react at 298 K. At equilibrium, there were 0.0200 mol of NO, present. Fill in the ICE table with the appropriate value for each involved species to determine concentrations of all reactants and products.. Initial (M) Change (M) Equilibrium (M) 1 2N₂O(g) + 30₂(g) 2 4NO₂(g) >

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Consider the reaction of N,O and O, described by the chemical reaction below. Determine the
equilibrium constant for this reaction by constructing an ICE table, writing the equilibrium
constant expression, and solving it. Complete Parts 1-2 before submitting your answer.
2 N₂O(g) + 3 O₂(g) = 4 NO₂(g)
2
NEXT
A 1.00 L reaction vessel was filled with 0.0560 mol O, and 0.200 mol N₂O and allowed to react at 298 K. At
equilibrium, there were 0.0200 mol of NO, present. Fill in the ICE table with the appropriate value for each involved
species to determine concentrations of all reactants and products..
Initial (M)
Change (M)
Equilibrium (M)
0.0100
0
-0.0100
1
2N₂O(g)
Question 34 of 40
0.0560
-0.0050
0.200
0.0050
+
-1.00
0.0150
30₂(g)
-0.0560
-0.0150
0.0200
0.210
4NO₂(g)
RESET
-0.0200
>
0.190
Transcribed Image Text:Consider the reaction of N,O and O, described by the chemical reaction below. Determine the equilibrium constant for this reaction by constructing an ICE table, writing the equilibrium constant expression, and solving it. Complete Parts 1-2 before submitting your answer. 2 N₂O(g) + 3 O₂(g) = 4 NO₂(g) 2 NEXT A 1.00 L reaction vessel was filled with 0.0560 mol O, and 0.200 mol N₂O and allowed to react at 298 K. At equilibrium, there were 0.0200 mol of NO, present. Fill in the ICE table with the appropriate value for each involved species to determine concentrations of all reactants and products.. Initial (M) Change (M) Equilibrium (M) 0.0100 0 -0.0100 1 2N₂O(g) Question 34 of 40 0.0560 -0.0050 0.200 0.0050 + -1.00 0.0150 30₂(g) -0.0560 -0.0150 0.0200 0.210 4NO₂(g) RESET -0.0200 > 0.190
Consider the reaction of NO and O, described by the chemical reaction below. Determine the
equilibrium constant for this reaction by constructing an ICE table, writing the equilibrium
constant expression, and solving it. Complete Parts 1-2 before submitting your answer.
2 N₂O(g) + 3 O₂(g) = 4 NO₂(g)
<
PREV
Based on the data from your ICE table, construct the expression for Kc. Each reaction participant must be
represented by one tile. Do not combine terms.
Once the expression is constructed, solve for Kc.
[0.200]
[0.200]²
0.0643
[0.0560]
[0.0560]³
2.57
1
Kc =
[0.0200]
Question 34 of 40
[0.0200]*
15.6
[0.190]
[0.1901²
0.390
[0.0410]
[0.0410³³
2
[0.0710]
[0.0710]³
[0.0360]
[0.0360]³
RESET
[0.180]
[0.180]²
Transcribed Image Text:Consider the reaction of NO and O, described by the chemical reaction below. Determine the equilibrium constant for this reaction by constructing an ICE table, writing the equilibrium constant expression, and solving it. Complete Parts 1-2 before submitting your answer. 2 N₂O(g) + 3 O₂(g) = 4 NO₂(g) < PREV Based on the data from your ICE table, construct the expression for Kc. Each reaction participant must be represented by one tile. Do not combine terms. Once the expression is constructed, solve for Kc. [0.200] [0.200]² 0.0643 [0.0560] [0.0560]³ 2.57 1 Kc = [0.0200] Question 34 of 40 [0.0200]* 15.6 [0.190] [0.1901² 0.390 [0.0410] [0.0410³³ 2 [0.0710] [0.0710]³ [0.0360] [0.0360]³ RESET [0.180] [0.180]²
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