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CHEM2 Finals

Total questions: 50

Worksheet time: 54mins

Name
Class
Date
1.
Is the combustion of gasoline endothermic or exothermic?
a)
Endothermic
b)
Exothermic
2.

Consider the reaction: 2 H2O + energy --> 2H2 + O2

a)

exothermic because releasing energy

b)

exothermic because absorbing energy

c)

endothermic because absorbing energy

d)

endothermic because releasing energy

3.

A 500g piece of aluminum has a temperature of 7°C. What is the heat energy produced? Specific heat of Aluminum is 0.900 J/gºC.

a)

3000 J

b)

3000 g

c)

3150 J

d)

3150 g

4.

How much heat does an aluminum block absorb if 10.00 grams is heated from 25.0oC to 50.0oC? *Specific heat of aluminum is 0.900 J/goC

a)

450 J

b)

-450 J

c)

225 J

d)

-225 J

5.

A 24.0 gram sample of copper was heated from 25.0oC to 500.0oC, 4378 J of heat were absorbed, what is the specific heat of copper?

a)

0.384 J/g°C

b)

49909200 J/g°C

c)

2.60 J/g°C

d)

8.77 J/g°C

6.

Endothermic:_________:__________

Exothermic:_________:__________

a)

positive:warm

negative:cold

b)

positive:warm

negative:warm

c)

positive:cold

negative:cold

d)

positive:cold

negative:warm

7.
Using the table of average bond energies below the image, the ΔH for the reaction in kJ is.....
a)
+ 160 kJ
b)
-63 kJ
c)
- 160 kJ
d)
-217 kJ
8.

Use the Hf values provided below to calculate Hrxn for the reaction. (Exclude units in your answer)

CO2(g) + N2(g) ⟶ NO(g) + CO(g) ΔH = ?

Data:

CO(g) = -110 kJ/mol

CO2(g) = -394 kJ/mol

NO(g) = +90 kJ/mol

(a)  

9.

How will a rate of reaction be altered if temperature is increased?

a)

reaction rate decreases (goes slower)

b)

reaction rate increases (goes faster)

c)

reaction rate is constant (stays the same)

10.

When a sugar cube is crushed up, the particles get smaller. How has the surface area of the particles changed?

a)

the surface area increases

b)

the surface area decreases

c)

the surface area remains constant

11.

A reaction between which of the following would increase the rate of a reaction and make it occur the fastest? What variable is being manipulated?


10 g of aluminum strip and 0.5 M hydrochloric acid at 20°C

10 g of aluminum strip and 0.5 M hydrochloric acid at 60°C

a)

10 g of aluminum strip and 0.5 M hydrochloric acid at 20°C; concentration is being altered

b)

10 g of aluminum strip and 0.5 M hydrochloric acid at 60°C; concentration is being altered

c)

10 g of aluminum strip and 0.5 M hydrochloric acid at 20°C; temperature is being altered

d)

10 g of aluminum strip and 0.5 M hydrochloric acid at 60°C; temperature is being altered

12.

You have a solution of 0.1 M silver nitrate reacting with a 5 g chunk of salt at room temperature. If you crush/pulverize the salt chunk, how will this alter the reaction rate?

a)

it will make the reaction faster because you are increasing the surface area of the salt

b)

it will make the reaction slower because you are increasing the surface area of the salt

c)

it will make the reaction faster because you are decreasing the surface area of the salt

d)

it will make the reaction slower because you are decreasing the surface area of the salt

13.

How does increasing concentration increase the rate of a reaction?

a)

fewer collisions occur among reactants

b)

more kinetic energy is provided to the reactants

c)

more collisions occur among reactants

d)

less kinetic energy is provided to the reactants

14.

How can you increase the concentration of a reactant?

a)

crush/pulverize the reactant into smaller pieces

b)

increase the molarity of a reactant

c)

add more water to the test tube

d)

increase the temperature of the reacting solutions

15.

You have a 0.2 M aqueous solution of copper (II) sulfate reacting with powdered iron at room temperature. If you put the solution of copper (II) sulfate in an ice water bath, how will this alter the reaction rate when combined with the iron?

a)

it will make the reaction faster because you are increasing the temperature of the solution

b)

it will make the reaction slower because you are increasing the temperature of the solution

c)

it will make the reaction faster because decreasing the temperature of the solution

d)

it will make the reaction slower because you are decreasing the temperature of the solution

16.

You have 1 M HCl reacting with 5 g of granular magnesium at room temperature. If you add water to the 1 M HCl, how will this alter the reaction rate?

a)

it will make the reaction faster because you are increasing the concentration

b)

it will make the reaction slower because you are increasing the concentration

c)

it will make the reaction faster because you are decreasing the concentration

d)

it will make the reaction slower because you are decreasing the concentration

17.

You have a solution of 0.1 M silver nitrate reacting with a 5 g chunk of salt at room temperature. If you crush/pulverize the salt chunk, how will this alter the reaction rate?

a)

it will make the reaction faster because you are increasing the surface area of the salt

b)

it will make the reaction slower because you are increasing the surface area of the salt

c)

it will make the reaction faster because you are decreasing the surface area of the salt

d)

it will make the reaction slower because you are decreasing the surface area of the salt

18.

Which best describes a catalyst?

a)

decreases reaction rate by raising activation energy

b)

increases reaction rate by lowering activation energy

c)

prevents reaction

d)

raises activation energy no matter what

19.

Calculate the equilibrium constant (Kc) for the given reaction

N2 (g) + 3H2 (g) ↔ 2NH3 (g)

At equilibrium [N2] = 0.34 M, [H2] = 0.13 M, and [NH3] = 0.19 M.

a)

48

b)

33

c)

48.0

d)

33.07

20.

Calculate the equilibrium constant (Kc) for the given reaction and tell whether equilibrium lies to the left or the right.

2NO (g) + Br2 (g) ↔ 2NOBr (g)

At equilibrium [NO] = 0.5 M, [Br2] = 0.25 M, and [NOBr] = 3.5 M.

a)

56 lies to the right

b)

200 lies to the right

c)

196 lies to the left

d)

56 lies to the left

21.

Consider the following system at equilibrium:

CH4(g) + 2H2O (g) ↔ CO2 (g) + 4H2O (g)

Suppose the concentration of CH4 decreased, in which direction does the reaction shift to reestablish equilibrium?

a)

The reaction shifts to the left

b)

The reaction shifts to the right

22.

What is the Kc expression for this reaction?    2 NO(g)  +  O2(g) ⇌  2 NO2(g)

a)

Kc = [NO2]2 / [NO]2 [O2]

b)

Kc =  [NO]2 [O2] / [NO2]2

c)

Kc = [NO]2 [O2] [NO2]2

d)

Kc = [NO2]2 / [NO]2 +  [O2]

23.

Consider the following reaction: 2SO2(g) + O2(g) <=> 2SO3(g):  ΔΗ = - 197 kJ mol -1 Which of the following will NOT shift the equilibrium position to the right?

a)

Adding more O2

b)

Adding a catalyst

c)

increasing the pressure

d)

Lowering the temperature

24.

CO2 (g) + C (s) ↔ 2CO (g)CO_2\ \left(g\right)\ +\ C\ \left(s\right)\ \leftrightarrow\ 2CO\ \left(g\right)  
An increase in carbon dioxide shifts 

a)

Left (towards reactants)

b)

Right (towards products)

c)

Does not affect equilibrium

25.

CO2 (g) + C (s) ↔ 2CO (g)CO_2\ \left(g\right)\ +\ C\ \left(s\right)\ \leftrightarrow\ 2CO\ \left(g\right)  
An increase in carbon monoxide shifts 

a)

Left (towards reactants)

b)

Right (towards products)

c)

Does not affect equilibrium

26.

N2O4 → 2NO2N_2O_4\ \rightarrow\ 2NO_2  

Write the equation for the equilibrium constant:

a)

K = [NO2][N2O4]K\ =\ \frac{\left[NO_2\right]}{\left[N_2O_4\right]}  

b)

K = [N2O4][NO2]K\ =\ \frac{\left[N_2O_4\right]}{\left[NO_2\right]}  

c)

K = [NO2]2[N2O4]K\ =\ \frac{\left[NO_2\right]^2}{\left[N_2O_4\right]}  

d)

K = [N2O4][NO2]2K\ =\ \frac{\left[N_2O4\right]}{\left[NO_2\right]^2}  

27.
Balance the following equation:
146C --> 0-1e + ________
a)
145B
b)
146C
c)
147N
d)
42He
28.
What is the missing isotope that will balance the following nuclear equation?
94Be  +  11H →  _____  +  42He
a)
105B
b)
105Ne
c)
63Li
d)
63C
29.

If an atom of potassium-40 (K) goes through gamma decay, what would you have at the end?

a)

Potassium-40

b)

Calcium-40

c)

Argon-35

d)

Potassium-39

30.
What element is the ?
a)
Ag-115
b)
Cd-115
c)
Pd-115
d)
Not Listed
31.

When the isotope 5024X releases a beta particle we get another element, Y, that looks like

a)

5023Y

b)

4622Y

c)

5025Y

d)

5024Y

32.

Complete the nuclear equation and determine the type of decay that is occurring in this reaction.

a)

alpha, 42He

b)

beta, 0-1e

c)

gamma

d)

none

33.
What type of decay is this?
7534Se + 0-1e --> 7533As
a)
Electron Capture
b)
Positron Emission
c)
Alpha Decay
d)
Beta Decay
34.
What is the equation for the positron emission by oxygen-16?
a)
168O + 0+1e --> 169F
b)
168O --> 42He + 126C
c)
168O --> 0-1e + 169F
d)
168O --> 0+1e + 167N
35.
Name the organic family for this structure:
a)
alkanes
b)
alkenes
c)
alkynes
d)
aromatics
36.

What functional group is shown?

a)

amino

b)

hydroxyl

c)

carboxyl

d)

sulfhydryl

37.

What functional group is shown?

a)

carboxyl

b)

carbonyl

c)

hydroxyl

d)

amino

38.

Identify the functional group.

a)

Benzene ring

b)

Carbon-carbon double bond

c)

Carbonyl

d)

Carboxyl

39.

Identify the functional group.

a)

Carbonyl

b)

Carboxyl

c)

Hydroxyl

d)

Carboalkoxy

40.

Identify the functional group.

a)

Carboalkoxy

b)

Carbon-carbon double bond

c)

Halogen

d)

Acyl chloride

41.

Identify the functional group.

a)

Halogen

b)

Amino group

c)

Anhydride

d)

Nitro group

42.

Neutral solutions have a pH of:

a)

0

b)

1

c)

7

d)

14

43.

Acid or Base?

Ca(OH)2 → Ca2+ + OH-

a)

Base

b)

Acid

44.

What is the pH of 0.0004M HF?

a)

4

b)

3.39

c)

3.40

45.

What is the pH of a solution with a concentration of 2.6 x 10-4 KOH solution?

a)

3.59

b)

14

c)

10.41

d)

4

46.

TRUE OR FALSE?

Bronsted-Lowry Base accept the proton (H+)

a)

TRUE

b)

FALSE

47.

Identify the Bronsted-Lowry Acid-Base in the given equation.

HNO3 + CH3OH → NO3- + CH3OH2

a)

Base + Acid → Acid + Base

b)

Acid + Base → Base + Acid

c)

Acid + Base → Acid + Base

48.

A solution has a pOH of 10.34

Is it an Acid or a Base?

a)

Acid

b)

Base

49.

Which of the following represents an Acid?

a)

pH = 12

b)

pOH = 3

c)

pOH = 12

d)

[H+] = 2.3 x 10-10

50.

In the equation below, OH- would be considered a ______

NH3 + H2O --> NH4+ + OH-

a)

Conjugate Acid

b)

Conjugate Base

c)

Salt

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