I-C-E Worksheet
1. In a 4.00 L closed container, 2.50 mol of carbon dioxide gas is decomposed.
(a) Calculate the theoretical yield for this system. I.e. Calculate [O2(g)] and [CO(g)] if the
reaction was quantitative.
(b) At equilibrium, [CO2(g)]eq = 0.125 mol/L. Use an ICE table to find [O2(g)]eq and [CO(g)]eq.
2CO2(g)
2CO(g)
+
1O2(g)
Initial (mol/L)
Change (mol/L)
Equilibrium
(mol/L)
(c) Determine the percent reaction for this system under these conditions.
2. 0.500 mol of NOCl(g) is decomposed in a closed 2.00 L container.
(a) Calculate the theoretical yield for this system.
(b) [NO(g)]eq = 0.040 mol/L. Find [Cl2(g)]eq and [NOCl(g)]eq.
2NOCl(g)
2NO(g)
+
Initial (mol/L)
Change (mol/L)
Equilibrium
(mol/L)
(c) Determine the percent reaction for this system under these conditions.
1Cl2(g)
3. When 2.00 mol of ethene gas and 1.50 mol of bromine vapour come to equilibrium in a
closed 1.00 L container, the equilibrium concentration of bromine vapour is measured at
0.150 mol/L.
(a) Calculate the theoretical yield for this system.
(b) Find [C2H4(g)]eq and [C2H4Br2(g)]eq
1C2H4(g)
+
1Br2(g)
1C2H4Br2 (g)
Initial (mol/L)
Change (mol/L)
Equilibrium (mol/L)
(c) Determine the percent reaction for this system under these conditions.
(d) Graph the equilibrium reaction for the addition of bromine to ethene.
Concentration-time graph for addition reaction
equilibrium
Concentration
2.500
2.000
1.500
1.000
0.500
Reaction Progess
Practice: p. 437 #6,7 & #1-5,7-9