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Test 1 Practice Questions - General Chemistry II | CHM 1046, Exams of Chemistry

Material Type: Exam; Professor: Landrum; Class: Gen Chemistry II; Subject: Chemistry; University: Florida International University; Term: Unknown 2001;

Typology: Exams

Pre 2010

Uploaded on 09/17/2009

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Exam I
General Chemistry I – CHM 1046
Spring 2001
Dr. Landrum
Name
SS#
Instructions: Always choose the best possible answer. Keep in mind that multiple
correct responses may be present. Answers may be very slightly different depending
on round-off and how many significant figures are carried between calculations.
Choose ‘None of the above’ only when no choice is a reasonable best answer.
R = 0.082 l atm/mol K
R = 8.3 J/mol K
First order
t1/2 = 0.693/k
ln([A]°/[A]t) = kt
Second order
t1/2 = 1/([A]°k)
((1/[A]t – 1/[A]°)) = kt
pf3
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Exam I General Chemistry I – CHM 1046 Spring 2001 Dr. Landrum

Name

SS#

Instructions: Always choose the best possible answer. Keep in mind that multiple correct responses may be present. Answers may be very slightly different depending on round-off and how many significant figures are carried between calculations. Choose ‘None of the above’ only when no choice is a reasonable best answer.

R = 0.082 l atm/mol K R = 8.3 J/mol K

First order

t (^) 1/2 = 0.693/k

ln ( [A]

/[A]t ) = kt

Second order

t 1/2 = 1 / ( [A]

k )

( (1/[A]t – 1/[A]

) ) = kt

  1. Which of the following is true for a solution? a) it is a mixture b) it is a special example of a suspension c) it contains only one solute d) it will always separate into its components on sitting
  2. The process of dissolving a solute into a solution is favored by a) increasing entropy b) solvation of the solute c) strong intermolecular attraction between the solute molecules d) a & b e) b and c f) a, b, & c g) none of the above
  3. Which is true for a solution prepared by dissolving 46.0 g of C 2 H 6 O in 100g of H 2 O if the final volume of the solution is 129 mL? a) the molarity will be 7.75 M b) the mole fraction of C 2 H 6 O is 0. c) the density fo the solution is 1.13 g/mL d) the molality is 10.0 m e) a & c f) b & d g) all are correct
  4. A solution has a density of 1.8g/mL and a molarity of 3.4 mole /L. What is the molality if the solvent is H 2 O and the molecular weight of the solute is 290 g/mole? a) 3.4 molal b) 6.12 molal c) 4.18 molal d) cannot be determined
  5. A freshwater lake is found to contain Hg 2+^ ion at a concentration of 4.7ppm. The lake has a uniform depth of 3 m and is circular having a diameter of 28 km. How many kg of Hg2+^ ion are present in the lake? a) 8.7 x 10-6^ kg b) 1.1 x 10^7 kg c) 2.3 x 10^9 kg d) 1.7 x 10^8 kg e) none of the above

a) [WI 3 ]/[W] [I 2 ] b) [W]^2 [I 2 ]^3 /[WI 3 ]^2 c) [WI 3 ]^2 /[W]^2 [I 2 ]^3 d) [WI 3 ]/[I 2 ]^3 e) [I 2 ]^3 /[WI 3 ]^2

  1. The reaction shown below has an equilibrium constant, Kc = 50.2. Is the system at equilibrium and is not which wa wil the reaction shift to reach equilibrium? [NO 2 ] = 0.25M ; [N 2 O 4 ] = 12.55M 2NO 2 (g) ⇄ N 2 O 4 (g) a) System is a equilibrium b) System is not at equilibrium and will shift right c) System is not at equilibrium and will shift left d) Can’t be determined
  2. What is the relationship between Kp and K (^) c for the reaction,

2NO (g) + O 2 (g) ⇄ 2NO 2 (g) a) Kc = Kp (1/RT) b) Kc = Kp (RT) c) Kc = Kp (1/RT) 2 d) Kc = Kp (1/RT) - e) None of the above

  1. Calculate the Kp from Kc for the following reaction; Kc = 2.5 x 10-3^ at T = 1400 K

CH 4 (g) + 2H 2 S (g) ⇄ CS 2 (g) + 4H 2 (g) a) 3.29 x 10^1 b) 3.78 x 10^3 c) 0. d) 1.65 x 10- e) 2.18 x 10-

  1. For the reaction below which statement is true if the system is initially @ equilibrium? H 2 (g) + I 2 (g) ⇄ 2HI (g) + q

a) If the volume is doubled the reaction shifts left b) If the pressure is doubled the reaction shifts left c) If the moles of I 2 are increased the reaction shifts left d) If the moles of H 2 are increased the reactions shifts right e) When the temperature is lowered the reaction shifts left

  1. Which statement is true about equilibria shown below

I H 2 O (g) + 1/2O 2 (g) ⇄ H 2 O 2 (g) K

II H 2 O 2 (g) + HCO 2 H (g) ⇄ HCO 3 H (g) + H 2 O (g) K

III 1/2O 2 + HCO 2 H (g) ⇄ HCO 3 H (g) K

a) K3 = K1 + K b) K3 = K2– K c) K3 = K1 x K d) K3 = K2/K e) K3 = K1/K

  1. Consider the equilibrium

2O 3 (g) ⇄ 3 O 2 (g) Kp = 1.3 x 10^57 at sea level the partial prssure of O 2 is 150 mmHg. Calculate the equilibrium partial pressure of O 3 at in air at sea level if the O 2 as is given is at equilibrium with O 3. a) 1.73 x 10-53^ mmHg b) 5.1 x 10-26^ mmHg c) 5.78 x 10^52 mmHg d) 8.67 x 10^54 mmHg

  1. At a temperature of 1500K the Kp for the dissociation of F 2 into atomic fluorine is 7.83. If a 1 L container is filled with 0.01 mole of F 2 (0.244 atm) at room temperature what will the partial pressure of fluorine atoms be after the system is heated to 1500K and equilibrium has been reached. (Remember: you must use units of Pressure!) F 2 (g) ⇄ 2F (g)

a) 0.856 atm b) 1.53 atm c) 1.39 atm d) 1.55 atm

  1. What is Kp for the following reaction if the equilibrium pressures of the reactants are: PPCl5 = 0.2 atm, P (^) Cl2 = 5.0 atm, PPCl3 = 4.64 atm PCl (^5) (g) + Cl (^2) (g) ⇄ PCl (^3) (g)

a) 8.62 x 10- b) 2.16 x 10- c) 1856 d) 116

c) 0.046 molar d) 3.5 x 10-4^ molar e) 0.395 molar

  1. For the reaction 2H 2 O 2 Æ 2H 2 O + O 2 (g) Which of the following must be true? a) R = k[H 2 O 2 ] 2 b) –1/2 d[H 2 O 2 ]/dt = d[O 2 ]/dt c) 1/2d[O 2 ]/dt = d[H 2 O 2 ]/dt d) d[H 2 O 2 ]dt = d[O 2 ]/dt
  2. Determine the Rate law for the following reaction using the method of initial rates and the data below.

Exp # [A] [B] Initial rate of C formation 1 0.011 0.071 0.041 M -1^ s - 2 0.011 0.142 0.020 M -1^ s - 3 0.022 0.071 0.164 M -1^ s -

a) R = k[A]^2 [B] b) R = k[A]^1 [B]^2 c) R = k[A]^2 [B]- d) R = k[A]-1^ [B]^2 e) R = k[A]^2 [B]-

  1. Use the graph below to determine the half-life of a reaction which obeys the following rate law, Rate = k[A]. [A] °

= 0.5M.

a) 408 s b) 177 s c) 511 s d) 588 s

  1. The rate constant of a reaction is dependent upon which of the following? a) Ea, activation energy b) The concentration of the reactants c) The temperature of the reaction d) The Arrhenius constant e) a & b f) a & c g) b & c h) a, b, & c i) a, c, & d j) None of the above
  2. Which statement is entirely correct about the following rate law, Rate = k[H+]^2 [O 3 ] a) the reaction is 1st^ order b) the reaction is 2nd^ order c) the reaction involves a single ternary step d) the reaction is 2nd^ order in H+^ and 1 st^ order in O 3
  3. A catalyst a) alters the activation energy b) influences the reaction mechanism c) must be insoluble d) a & b e) all of the above
  4. If a reaction is 1st^ order and the reaction is 7% complete after 2 hrs when will the reaction reach 99% completion. a) 28.3 hrs

t ln[A] 0 -0. 100 -0. 200 -1. 300 -1. 400 -1. 500 -1. 600 -1. 700 -1. 800 -2. 900 -2. 1000 -2.393 (^) -

-2.

-

-1.

-

-0.

0

0 200 400 600 800 1000 1200 time (seconds)

ln [A]t