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# Kinetics and Equilibrium

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Kinetics and equilibrium
1- An aqueous solution containing 18.9g of an unknown molecular (nonelectrolyte) compound in 103.0g of water was found to have a freezing point of -1.7 ∘ C.Calculate the molar mass of the unknown compound.Express your answer using two significant figures and g/mol
delta Tf=i*m*kf
1.70C=1*(18.9g/M)/(0.103kg)*1.860C/m
M=200.77 g/mol

2- What is the osmotic pressure of a solution made by dissolving 25.0g of glucose, C 6 H 12 O 6 , in enough water to form 325.0mL of solution at 34.0 ∘ C ?.
Osmotic pressure: i*M*R*T=1*25.0g/(180g/mol)/(0.325L)*0.08206L.atm/(K.mol)*(34+273)K=10.77 atm.

3- A solution of water (K f =1.86 ∘ C/m ) and glucose freezes at − 2.75 ∘ C . What is the molal concentration of glucose in this solution? Assume that the freezing point of pure water is 0.00 ∘ C Express your answer to three significant figures and include the appropriate units.
Delta Tf=i*m*kf
2.750C=1*m*1.860C/m
Molality: m=1.48 m.
4- A solution of water (K b =0.512 ∘ C/m ) and glucose boils at 102.06 ∘ C . What is the molal concentration of glucose in this solution? Assume that the boiling point of pure water is 100.00 ∘ C .Express your answer to three significant figures and include the appropriate units.
Delta ...

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The solution discusses kinetics and equilibrium.

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## Reaction Kinetics, Rate Laws and Equilibrium

1. The isomerization of cyclopropane to form propene

CH3 - CH CH2CH2

is a first-order reaction. At 760 K, 15 percent of a sample of cyclopropane changes to propene in 6.8 minutes. What is the half-life of cyclopropane at 760 K?

2. Consider the two gaseous equilibria (K1 and K2):

SO2(g) + ½O2(g) SO3(g) K1

2SO3(g) 2SO2(g) + O2(g) K2

The values of the equilibrium constants K1 and K2 are related by ________.

3. The following reactions occur at 500 K. Arrange them in order of increasing tendency to proceed to completion (i.e., least completion greatest completion).
1. 2NOCl 2NO + Cl2 KP = 1.7 x 10-2
2. N2O4 2NO2 KP = 1.5 x 103
3. 2SO3 2SO2 + O2 KP = 1.3 x 10-5
4. 2NO2 2NO + O2 KP = 5.9 x 10-5

4. On analysis, an equilibrium mixture for the reaction

2H2S(g) 2H2(g) + S2(g)

was found to contain 1.0 mol H2S, 4.0 mol H2, and 0.80 mol S2 in a 4.0 L vessel. Calculate the equilibrium constant for this reaction.

5. At 35oC, the equilibrium constant for the following reaction is Kc = 1.6 x 10-5.

2NOCl(g) 2NO(g) + Cl2(g)

An equilibrium mixture was found to have the following concentrations of Cl2 and NOCl:

[Cl2] = 1.2 x 10-2 M; [NOCl] = 2.8 x 10-1 M. Calculate the concentration of NO(g) at equilibrium.

6. For the following reactions the equilibrium constants are defined.

A + 2B C K1
C D + E K2

Then for the reaction

A + 2B D + E Kc

the equilibrium constant must be equal to ________.

7. At 700 K, the reaction

2SO2(g) + O2(g) 2SO3(g)

has an equilibrium constant Kc = 4.3 x 106, and the following concentrations are present:

[SO2] = 0.10 M
[SO3] = 10 M
[O2] = 0.10 M

Is the mixture at equilibrium? If not at equilibrium, in which direction-left to right or right to left- will the reaction occur to reach equilibrium?

8. For the following reaction at equilibrium, which choice gives a change that will shift the position of equilibrium to favor formation of more products?

2NOBr(g) 2NO(g) + Br2(g) Horxn = 30 kJ

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