1. Consider the reaction A(g) + B(g) ↔ C(g) + D(g) at 300°C. What is the equilibrium concentration of D if the initial concentrations are [A] = [B] = 1.25 x 10-2 M and [C] = [D] = 3.50 x 10-3 M? The value of the equilibrium constant for the reaction is 55.9 at 300°C.
|1.41 x 10-2 M|
|4.39 x 10-2 M|
|8.34 x 10-2 M|
|6.62 x 10-2 M|
|5.76 x 10-2 M|
|9.18 x 10-3 M
2. The equilibrium constant for the following reaction is 4.66 x
10-3 at 25°C. The system at equilibrium has
[N2O4] = 0.208 M. What is [NO2] in
the equilibrium mixture?
N2O4(g) ↔ 2 NO2(g)
4.51 x 10-2 M
4.01 x 10-2 M
5.79 x 10-2 M
3.11 x 10-2 M
2.21 x 10-2 M
5.26 x 10-2 M
3.The reaction 2 A(g) + B(g) ↔ C(g) + 3 D(g) has an equilibrium constant of 2.55 x 10-3 at 85°C. If the initial concentrations are [A] = 1.50 M, [B] = 3.15 M, [C] = 0.0425 M, and [D] = 0.725 M, which of the following statements is true?
|The system is not at equilibrium and will shift to the left to establish equilibrium.|
|The system is not at equilibrium and will shift to the right to establish equilibrium.|
|The system is at equilibrium and will not shift in either direction.|
|Cannot be predicted.|
1. For the reaction
Initial concentration of reactants (A and B) are more than product (C and D) therefore reaction will proceed forward.
At equilibrium if x mole/L of A and B react to produce x moles of C and D
Final concentration of A= Final Concentration of B =
Final Concentration of C= Final Concentration of D=
Final concentration of
For the reaction
The system is at equilibrium and will not shift in either direction.
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