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Select all the true statements regarding chemical equilibrium.
1) the concentrations of reactants and products remain constant.
2) reactants are still being converted to products (and vice versa).
3) the concentrations of reactants and products are equal.
4) the rates of the forward and reverse reactions are equal.
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the concentrations of reactants and products remain constant. reactants are still being converted to products (and vice versa). the rates of the forward and reverse reactions are equal.
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Write the equilibrium-constant expression for the reaction
[A]s + [B] l = 2[C] aq + [D]aq
in terms of [A], [B], [C], and [D] as needed.
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kc= [C]2 [D] ignore both A and B because they are not aqueous.
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For the reversible reaction
[A]g = [B] g
which K values would indicate that there is more B than A at equilibrium?
K = 1× 109, 1× 10-9
K = K = 0.2, K = 2000
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YES : K = 1× 109, K = 2000 NO: K = 1× 10-9, K = 0.2
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In which direction will the net reaction proceed
X+Y=Z kp= 1.0 @ 300K
for each of these sets of initial conditions?
a) [X] = [Y] = [Z] = 1.0 M
b) PX = PZ = 1.0 atm, PY = 0.50 atm
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a) net reaction goes to the right b) net reaction goes to the left
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Consider the following system at equilibrium.
2CO + O2 = 2CO2
a) How will increasing the concentration of CO shift the equilibrium?
b) How will increasing the concentration of CO2 shift the equilibrium?
c) How will decreasing the the volume of the container shift the equilibrium?
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a) to the right b) to the left c) to the right
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Consider this system at equilibrium.
[A]aq = [B]aq ΔH.= +450 kJ/mol
a) What can be said about Q and K immediately after an increase in temperature?
b) How will the system respond to a temperature increase?
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a) Q< K because K increased ΔH. For endothermic reactions, K increases when T increases. For exothermic reactions, K decreases when T increases. b) Shift right
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Rearrange this expression into quadratic form, ax2 bx c=0
.20= x2/35*x
where a = 1, and identify the values of b and c.
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a) 1 b) .2 c) -7 (-.2*35)
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Consider the following system at equilibrium.
S(s) + O2(g) = SO2(g)
a) How will adding more S(s) shift the equilibrium?
b) How will removing some SO2(g) shift the equilibrium?
c) How will decreasing the volume of the container shift the equilibrium?
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a) no effect b) to the right c) no effect
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Consider this system at equilibrium.
[A]aq = [B]aq ΔH.= -750kJ/mol
a) What can be said about Q and K immediately after an increase in temperature?
b) How will the system respond to a temperature increase?
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a) Q>K because K decreased b) shift left
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