In: Chemistry

3. Molecular bromine is 24% dissociated at 1600K and 1.00 bar in the equilibrium:

Br2 (g)-------- 2Br(g)

Calculate:

a) the equilibrium constant K at 1600K (8)

b) the standard Gibbs energy of reaction 4)

C) K at 2000K , given that ∆r H = +112kj/mol over the temperature range. (6)

**Solution :-**

Given data

Br2 (g)-------- 2Br(g)

Br2 dissociate 24 % at 1600 K

a)the equilibrium constant K at 1600K (8)

dissociation is 24 % that means if we assume 1 mole of the Br2 then

1 mol * 24 % / 100 % = 0.24 mol Br2 will dissociate

Therefore at equilibrium moles of Br2 remain = 1 mol – 0.24 mol = 0.76 mol

Moles of Br formed = 0.24 mol * 2 = 0.48 mol Br

Lets write the Kc equation

Kc= [Br]^2 / [Br2]

Kc =[0.48]^2 /[0.76]

**Kc = 0.3032**

b)the standard Gibbs energy of reaction 4)

formula to calculate the Gibbs energy is as follows

Delta Go = - RT ln K

Lets put the values in the formula

Delta Go = - 8.314 J per K mol * 1600 K * ln 0.3032

Delta Go = 15874 J

Delta Go = 15874 J * 1 kJ / 1000 J =
**15.87 kJ**

C) K at 2000K , given that ∆r H = +112kj/mol over the temperature range. (6)

Now lets calculate the equilibrium constant at 2000 K

ln k2/k1 = delta H / R [(1/T1)-(1/T2)]

ln k2 /0.3032 = 112000 J per mol / 8.314 J per K . mol * [(1/1600)-(1/2000)]

ln K2 / 0.3032 = 1.689

k2/0.3032 = antiln 1.689

k2/0.3032 = 5.414

K2 = 5.414 * 0.3032

K2 = 1.64

**Therefore equilibrium constant at 2000 K =
1.64**

When 0.127 mol of NO and 17.80
g of bromine are placed in a 1.00-L reaction vessel and sealed, the
mixture is heated to 350 K and the following equilibrium is
established:
2NO(g) + Br2(g) ------> 2NOBr(g)
If the equilibrium concentration of nitrosyl bromide is
8.63X10^-2 M, what is Kc ?

Consider the following three-step mechanism for a
reaction:
Br2 (g) ⇌ 2 Br (g) Fast
Br (g) + CHBr3 (g) → HBr (g) + CBr3 (g)
Slow
Br (g) + CBr3 (g) → CBr4 (g) Fast
Based on this mechanism, determine the rate law for the overall
reaction.
Rate =

Consider the following equilibrium.
CS2(g) + 3 O2(g) equilibrium reaction arrow CO2(g) + 2 SO2(g)
If the reaction is started in a container with 5.59 atm CS2 and
13.3 atm O2, what is Kp if the partial pressure of CO2 is 3.76 atm
at equilibrium? (There is no change in temperature and the initial
partial pressures of the products are equal to 0.)

The following equilibrium reaction is investigated.
2 N2O(g) + N2H4(g) ⇆ 3 N2(g) + 2
H2O(g)
When 0.10 moles of N2O and
0.25 moles of N2H4 are placed in a 10.0-L container and allowed to
come to equilibrium, the equilibrium concentration of N2O is 0.0060
M. What is the equilibrium concentration of all four
substances?

1)
How many g/in^3 in 3.11 x 10^3 g/dm^3?
2) 1.00 in^3 (cubic inch) of a material has a mass of 0.240
lb. How many liters of this material would weigh 3.30 kg?
3) 1.00 in^3 of a metal weighs 0.544 pounds. What is the mass
in kg of 7.80 L of this metal?
4) When you perform the following operations, how many
significant figures should your answer have? (1.20000 x 10^4 g) +
(2.41 x 10^2)
5) When you...

How many oxygen atoms are in 1.00 g of the mineral
troegerite, (UO
2
)
3
(AsO
4
)
2
•12 H
2
O (
M
= 1304.0)?
(A)
6.47
×
10
21
(B)
8.31
×
10
21
(C)
1.20
×
10
22
(D)
1.39
×
10
22

The following reaction reaches equilibrium at 350 degree C and 2
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H subscript 3 C H O space left parenthesis g right parenthesis
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parenthesis space rightwards arrow space C subscript 2 H subscript
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N2 (g)+ 3 H2 (g)↔ 2 NH3
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ammonia gas (NH3) was
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volume was decreased?
nonreactive argon gas (Ar) was added
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A mixture of hydrogen gas and iodine
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[N2] = 0.0027 M
[H2] = 0.0045 M
[NH3] = 0.20 M
(a) Determine the ΔG of the reaction.
(b) Determine which direction the reaction will proceed in order
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Consider the following equilibrium:
2NOCl(g) 2NO(g)
+ Cl2(g)with K = 1.6 × 10–5. 1.00 mole of pure NOCl and 1.50 mole
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