CHEMISTRY 102 HOMEWORK[set#5]
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CURRENT DATE and TIME

Dr. Kenneth M. Maloney

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Which of the following statements is true in a reaction system at equilibrium?

1. The number of collisions per unit time between reactants is equal to the number of     collisions per unit time between products.
2. Reactants are reacting to form products at the same rate as products are reacting to     form reactants.
3. The product of the concentrations of the products divided by the product of the     concentrations of the reactants is always a constant.

Your answer:
1 only
2 only
1 and 2 only
3 only
1, 2, and 3

The equilibrium constant, K_c, for the reaction

(1/2)N₂O₄(g) NO₂

is 3.3 at 100°C. The value for the equilibrium constant will be changed if

1. concentration sre given in atmosphers instead of moles per liter.
2. the temperature is change to 200°C.
3. the equation above is doubled.

Your answer:
1 and 2 only
2 only
2 and 3 only
1, 2, and 3
1 only

The equilibrium expression for K_c for the system

CaSO₃(s) CaO(s) + SO₂(g)

is

Your answer:
1/[SO₂]
[CaO][SO₂]
[SO₂]
[CaSO₃]/[CaO][SO₂]
[CaO][SO₂]/[CaSO₃]

A mixture of nitrogen and hydrogen was allowed to come to equilibrium at a given temperature.

H2(g) + I2(g) 2 HI(g)

at 460°C?

Your answer:
5.3
6.0
4.0
3.0
4.5

Sulfur dioxide combines with O₂ in the presence of a catalyst as represented by the equation

2SO₂(g) + O₂(g) 2SO₂

If the equilibrium is established by adding 0.10 mol each of SO₂ and O₂ to a 1-L vessel, then which of the following must be true at equilbrium?

Your answer:
[O₂] = 2[SO₃]
[SO₂] > [O₂]
[SO₂] < [O₂]
[SO₂] = [O₂]
[SO₂] = [O₂] = [SO₃]

For the reaction

CoO(s) + H₂(g) Co(s) + H₂O(g)

at 550°C, K = 67. The equilbrium constant expression is

Your answer:
[Co][H₂O]/[H₂].
[H₂]/[H₂O].
[H₂O]/[H₂].
[Co][H₂O]/[CoO][H₂].
[CoO][H₂]/[Co][H₂O].

If K = 0.145 for A₂ + 2B 2AB, then for 4AB 2A₂ + 4B, K would equal

Your answer:
-0.145.
47.6.
0.145.
2.63.
6.90.

For the following reaction systems at 500 K

   I. 2NOCl(g) 2NO(g) + Cl₂(g)         Kp = 1.7 x 10^-2
II. 2NO₂(g) 2NO(g) + O₂(g)             Kp = 5.9 x 10^-5
III. 2SO₃(g) 2SO₂(g) + O₂(g)            Kp = 1.3 x 10^-5

Your answer:
III<II<I.
II<I<III.
II<III<I.
III<I<II.
I<II<III.

Given the equilibrium constants for the following reactions

4Cu(s) + O₂(g) 2Cu₂O(s), K₁

2CuO(s) Cu₂O(s) + (1/2)O₂(g), K₂

what is K for the system

2Cu(s) + O₂(g) 2CuO(s)

equivalent to?

Your answer:
K₂^1/2 /K₁
K₁^1/2 K₂
K₁ x K₂ ^1/2
K₁ x K₂
K₁^1/2 /K₂

Which of the following equilibria would be affected by volume changes at constant temperature

1. 2NO(g) + 3F(g) 2F3NO(g)
2. 4NH₄(g) + 5O₂(g) 4NO(g) + 6H₂O(g)
3. SO₃(g) + NO(g) NO(g) + SO₂(g)

Your answer:
2 and 3 only
1 only
3 only
2 only
1 and 2 only

CS₂(g) + 3Cl₂(g) CCl₄(g) + S₂Cl₂(g)

At a given temperature the reaction above is at equilibrium when [CS₂] = 0.050 M, [Cl₂] = 0.25 M, [CCl₄] = 0.15 M, and [S₂Cl₂] = 0.35 M. What would be the direction of the reaction when the reactants and products have the following concentrations: CS₂ = 0.15 M, Cl₂ = 0.20 M, CCl₄ = 0.30 M, and S₂Cl₂ = 0.28 M?

Your answer:
to the right
to the left
no change
cannot predict unless we know the temperature
cannot predict unless we know whether the reaction is endothermic or exothermic

A state of dynamic equilibrium exists at constant temperature in

1. a stoppered flask half full of water.
2. a stoppered flask half full of an unsaturated sulfate solution.
3. an open pan of boiling water.

Your answer:
1 only
3 only
1 and 2 only
2 only
1 and 3 only

For the reaction NO(g) + (1/2)O₂ NO₂(g) at 750°C, the equilibrium constant K_c equals

Your answer:
K_p(RT)^2/3.
K_p(RT)^-3/2.
K_p(RT)^1/2.
1.0.
K_p(RT)^3/2.

For the equilibrium system

CO₂(g) + H₂(g) CO(g) + H₂O(g) ΔH = +42 kJ/mol

K equals 1.6 at 1260 K. If 0.15 mol each of CO₂, H₂, CO, and H₂O(all at 1260 K) were placed in a 1.0-L thermally insulated vessel that was also at 1260 K, then when the system came to equilibrium,

Your answer:
the temperature would increase and the mass of CO would increase.
the temperature would increase and the mass of CO would decrease.
the temperature would remain constant and the mass of CO would increase.
the temperature would decrease and the mass of CO would decrease.
the temperature would decrease and the mass of CO would increase.

Carbon tetrachloride reacts with oxygen at high temperatures to produce chlorine and carbonyl chloride.

2CCl₄(g) + O₂(g) 2COCl₂(g) + 2Cl₂(g) K_c = 1.9 x 10¹⁹

What is K_c for the following?

COCl₂(g) + Cl₂(g) CCl₄(g) + (1/2)O₂(g)

Your answer:
5.3 x 10^-20
4.4 x 10⁹
2.3 x 10^-10
-1.9 x 10¹⁹
1.9 x 10¹⁰

**Important→To receive "credit" for your homework, complete the "following questions (e-mail format)" and submit(click here)! A Homework Exercise..for course details see... Dr. Kenneth M. Maloney

CHEMISTRY 102 HOMEWORK[set#5]{Tools/Aids}CURRENT DATE and TIME

Dr. Kenneth M. Maloney

The equilibrium constant, Kc, for the reaction (1/2)N2O4(g) NO2 is 3.3 at 100°C. The value for the equilibrium constant will be changed if 1. concentration sre given in atmosphers instead of moles per liter. 2. the temperature is change to 200°C. 3. the equation above is doubled.

The equilibrium expression for Kc for the system CaSO3(s) CaO(s) + SO2(g) is

A mixture of nitrogen and hydrogen was allowed to come to equilibrium at a given temperature. H2(g) + I2(g) 2 HI(g) at 460°C?

Sulfur dioxide combines with O2 in the presence of a catalyst as represented by the equation 2SO2(g) + O2(g) 2SO2 If the equilibrium is established by adding 0.10 mol each of SO2 and O2 to a 1-L vessel, then which of the following must be true at equilbrium?

For the reaction CoO(s) + H2(g) Co(s) + H2O(g) at 550°C, K = 67. The equilbrium constant expression is

If K = 0.145 for A2 + 2B 2AB, then for 4AB 2A2 + 4B, K would equal

For the following reaction systems at 500 K I. 2NOCl(g) 2NO(g) + Cl2(g) Kp = 1.7 x 10-2 II. 2NO2(g) 2NO(g) + O2(g) Kp = 5.9 x 10-5 III. 2SO3(g) 2SO2(g) + O2(g) Kp = 1.3 x 10-5

Given the equilibrium constants for the following reactions 4Cu(s) + O2(g) 2Cu2O(s), K1 2CuO(s) Cu2O(s) + (1/2)O2(g), K2 what is K for the system 2Cu(s) + O2(g) 2CuO(s) equivalent to?

Which of the following equilibria would be affected by volume changes at constant temperature 1. 2NO(g) + 3F(g) 2F3NO(g) 2. 4NH4(g) + 5O2(g) 4NO(g) + 6H2O(g) 3. SO3(g) + NO(g) NO(g) + SO2(g)

A state of dynamic equilibrium exists at constant temperature in 1. a stoppered flask half full of water. 2. a stoppered flask half full of an unsaturated sulfate solution. 3. an open pan of boiling water.

For the reaction NO(g) + (1/2)O2 NO2(g) at 750°C, the equilibrium constant Kc equals

For the equilibrium system CO2(g) + H2(g) CO(g) + H2O(g) ΔH = +42 kJ/mol K equals 1.6 at 1260 K. If 0.15 mol each of CO2, H2, CO, and H2O(all at 1260 K) were placed in a 1.0-L thermally insulated vessel that was also at 1260 K, then when the system came to equilibrium,

Carbon tetrachloride reacts with oxygen at high temperatures to produce chlorine and carbonyl chloride. 2CCl4(g) + O2(g) 2COCl2(g) + 2Cl2(g) Kc = 1.9 x 1019 What is Kc for the following? COCl2(g) + Cl2(g) CCl4(g) + (1/2)O2(g)