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General Chemistry Quiz

Total questions: 85

Worksheet time: 2hrs 28mins

Name
Class
Date
1.
Chemical Formulas ...
a)
are written in alphabetical order 
b)
represent the destruction or creation of atoms 
c)
represent how atoms are arranged in a chemical reaction 
2.

The following data were measured for the reaction

BF3(g) + NH3(g) ⟶ F3BNH3(g)

What is the rate when [BF3] = 0.100 M and [NH3] = 0.500 M ?

a)

.01704 M/s

b)

.0852 M/s

c)

.1704 M/s

d)

.852 M/s

3.

A reaction is found to be second order with respect to carbon monoxide. If the concentration of carbon monoxide is doubled, the rate of reaction __________.

a)

doubles

b)

remains unchanged

c)

increases by a factor of 4

d)

is reduced by a factor of 2

4.

The first order rate constant for the decomposition of 0.5 M compound A at 100oC is 0.03 min-1. Calculate the half-life of A.

a)

1.5 min

b)

8.3 min

c)

23.1 min

d)

66.7 min

5.

In a series of reaction, which is the rate determining step

a)

The simplest reaction

b)

The slowest reaction

c)

The fastest reaction

d)

The main reaction involving the major reactant

6.

The unit of rate constant for first order reaction

(a)  

7.

In general, an increase in temperature of 10°C will have what effect on reaction rate:

A. Double the rate

B. Half the rate

C. Triple the rate

D. Increase the rate but not by a specific amount

a)

A

b)

B

c)

C

d)

D

8.

Which of the following statements is correct about order of a reaction.

a) The order of a reaction can be a fractional number.

b) Order of a reaction is experimentally determined quantity.

c) The order of a reaction is always equal to the sum of the stoichiometric coefficients of reactants in the balanced chemical equation for a reaction.

d) The order of a reaction is the sum of the powers of molar concentration of the reactants in the rate law expression.

a)

A, B

b)

A, B, C

c)

A, B, D

d)

B, C, D

9.

In the rate equation, when the concentration of reactants is unity then the rate is equal to

a)

specific rate constant

b)

average rate constant

c)

instantaneous rate constant

d)

None of the above

10.

The unit of rate constant for the second order reaction will be ___________

a)

a) s-1

b)

b) L mol-1 s-1

c)

c) Mol0.5 L-0.5 s-1

d)

d) Mol L-1 s-1

11.

For the elementary reaction the rate of

disappearance of M increases by a factor of 8 upon

doubling the concentration of M. The order of the reaction

with respect to M is:

a)

1

b)

3

c)

2

d)

4

12.

If the concentration of a reactant is increased, the reaction rate will ___________.

a)

increase

b)

decrease

c)

stay the same

13.

Determine order of reaction for the reactant A and B based on this rate law:

Rate = K [A]2[B]1

a)

[A] first order and [B] first order

b)

[A] first order and [B] second order

c)

[A] second order and [B] first order

d)

[A] second order and [B] second order

14.

The graph the rate of reaction below, refer to the:

a)

zero order

b)

first order

c)

second order

d)

third order

15.

Which of the following statements regarding the half-life of first order reaction is true?

a)

The half-life is affected by pressure.

b)

The half-life depends on the concem9of the reactant.

c)

The half-life is shorter at lower temperature.

d)

At the end of fourth half-life, the percentage of element left is 6.25% of the original quantity.

16.

Given: A + 3B -> 2C + D

This reaction is first order with respect to reactant A and second order with respect to reactant B. If the concentration of A is doubled and the concentration of B is halved, the rate of the reaction would __ by a factor of __.

a)

increase, 2

b)

decrease, 2

c)

increase, 4

d)

decrease, 4

e)

not change

17.

Q2. For a reaction A +B → C, the experimental rate law is found to be R=k[A]1[B]1/2. Find the rate of the reaction when [A] = 0.5 M, [B] = 0.01 M and k=0.03.

a)

a) 4.74 × 10-2 (L/mol)1/2 s-1

b)

b) 5.38 × 10-2 (L/mol)1/2 s-1

c)

c) 1.50 × 10-3 (L/mol)1/2 s-1

d)

d) 4.86 × 10-2 (L/mol)1/2 s-1

18.
Consider the following rate law: Rate = k[A]n[B]m
How are the exponents n and m determined?
a)
by using balanced chemical equation
b)
By using the subscripts for the formulas
c)
By educated guess
d)
By experiment 
19.
When you double the concentration of this reactant the rate of the reaction doesn't change.  It is ______ order
a)
First
b)
Second
c)
Zero
20.
What is the half-life of iodine-131?
a)
32 days
b)
8 days
c)
16 days
d)
24 days
21.

For an elementary reaction 2A + B →C + D, the molecularity is

a)

zero

b)

one

c)

two

d)

three

22.

The time taken for 10% completion of a first order reaction is 20 mins .Then for 19% completion ,the reaction will take

a)

50 mins

b)

30 mins

c)

40 mins

d)

60 mins

23.

What happened to the rate of reaction, if concentration of reactant is 'zero order'.

a)

rate of reaction will become double

b)

rate of reaction will become triple

c)

rate of reaction will become quadrapel

d)

No affect to the rate of reaction

24.

In a zero-order reaction for every 10° rise of temperature, the rate is doubled. If the temperature is increased from 10°C to 100°C, the rate of the reaction will become

a)

64 time

b)

128 times

c)

256 times

d)

512 times

25.

Radioactivity of a sample (z = 22) decreases 90% after 10 years. What will be the half-life of the sample?

a)

5 years

b)

2 years

c)

3 years

d)

10 years

26.

Which of these changes with time for a first-order reaction?

A. Rate of reaction

B. Rate constant

C. Half-life

a)

A only

b)

B only

c)

A & C only

d)

A & B only

27.

For a chemical reaction A → B, the rate of the reaction is

2 × 10–3 mol dm–3 s–1 when the initial concentration is 0.05 mol dm–3. The rate of the same reaction is 1.6 × 10–2mol dm–3 s–1 when the initial concentration is 0.1 mol dm–3. The order of the reaction is

a)

0

b)

3

c)

1

d)

2

28.

reaction rate constant also known as

a)

specific reaction rate

b)

reaction rate

c)

rate reaction

d)

none

29.
Basic buffer is made up of
a)
weak base and weak acid
b)
weak base and its conjugate salt
c)
weak base and its conjugate acid
d)
strong base and its conjugate acid
30.

Two beakers have liquids in them. When you add a base such as ammonia to beaker 1, the pH did not change. But when you add ammonia to beaker 2, the pH changes drastically. Choose the best explanation.

a)

Beaker 1 had only water and Beaker 2 contained a buffer.

b)

Beaker 1 contained a buffer and Beaker 2 contained only water.

c)

Beaker 2 contained an acid.

d)

The beaker that changed pH contained a buffer.

31.

What is the molarity of 4 g of NaCl (MM=58.45) in 3,200 mL of solution?

a)

0.021 M

b)

0.214 M

c)

0.315 M

32.

What is the molarity of a solution made by diluting 26.5 mL of 6.00M HNO3 to a volume of 250 mL?

a)

15.9 M

b)

0.636 M

c)

0.642 M

d)

1.59 M

33.

Molar mass of SO2 is

a)

64 a.m.u

b)

64 g

c)

48 a.m.u

34.

In reaction 2SO2+O2 →  2SO32SO_2+O_2\ \rightarrow\ \ 2SO_3  

 0.2 moles of  product will be formed by  

a)

3.2 g of Oxygen

b)

32 g of Oxygen

c)

1.6 g of Oxygen

d)

16 g of Oxygen

35.

Reactant that is left unreacted in a chemical reaction is called

(a)  

36.

Select all the correct options for chemical units of concentration

a)

Normality

b)

Mole fraction

c)

ppm

d)

weight percent

37.

For a given succinic acid solution

a)

Its Molarity and Formality are different

b)

Its Molarity is same as Formality

38.

Number of moles of HCl in 500 mL of 6.0 M solution

a)

1.2 moles

b)

3.0 moles

c)

0.8 moles

39.

Normality and Molarity are related as   (p is number of reaction units)

a)

Molarity p \frac{Molarity\ }{p}\  

b)

Molarity x p

40.

Ca+2 → Ca Ca^{+2\ }\rightarrow\ Ca\  value of 'p'  for this reaction is  _____ and hence its equivalent weight is _________its molar mass

(a)  

41.

molality is a temperature dependent concentration unit

a)

True

b)

False

42.

For a redox reaction involving KMnO4 in presence of H2SO4, equivalent wt. of KMnO4 will be

a)

One fifth of its Molecular weight

b)

Same as its molecular weight

c)

One third of its molecular weight

d)

5 times its molecular weight

43.

0.1 ppm solution means

a)

0.1 moles of solute dissolved per litre of solution

b)

0.1 moles of solute dissolved per 1000L of solution

c)

0.1 millimoles of solute dissolved per 1000L of solution

d)

0.1 mg of solute per litre of solution

44.

Amount of CaCl2 required to prepare 1 L of 10 ppm solution w.r.t Ca2+ ions is (At. wt of Ca = 40, Cl= 35.5)

a)

44 mg

b)

10 mg

c)

27.75 mg

45.

A substance that gives solution of exact known concentration is called

(a)  

46.
When does a chemical reaction stop?
a)
When the lab is finished
b)
When the excess reactant is used up
c)
When the limiting reactant is used up
d)
Chemical reactions never stop
47.

The coefficients in a chemical equation represent the

a)

masses, in grams, of all reactants and products.

b)

relative numbers of moles of reactants and products.

c)

number of atoms in each compound in a reaction.

d)

number of valence electrons involved in the reaction.

48.
Calculate mol fraction of H2O in 1.33 molal NaOH solution.
a)
0.56
b)
0.76
c)
0.98
d)
0.84
49.

8 g of sugar is dissolved in 42g of water. What is the concentration (%w/w) of the solution formed?

a)

16%

b)

14%

c)

18%

d)

20%

50.

A bottle of concentrated nitric acid, HNO3 solution has a label of "85.00% by mass" and density of 0.8362 gmL-1. Calculate the molarity and molality of the concentrated nitric acid solution.

a)

11.28 M and 98.95 molal

b)

10.18 M and 85.95 molal

c)

11.28 M and 89.95 molal

d)

10.18 M and 86.95 molal

51.
N2 +  3H2 −->  2NH3 
How many moles of hydrogen are needed to react with 2 moles of nitrogen?
a)
6
b)
2
c)
3
d)
1
52.

To convert liters of a solution to moles, one should:

a)

divide by the molarity

b)

multiply by the molarity

c)

multiply by the molar mass

d)

divide by the molar mass then multiply by the speed of light squared

53.

The buffer solution is able to maintain pH by some events, except . . .

a)

The addition of a little acid

b)

The addition of a little base

c)

Dilution

d)

Addition of water

e)

The addition of excess acid

54.

The pH solution that consist of CH3COOH 0.01 M and CH3COONa 0.01 M with Ka = 10-5 is . . .

a)

4

b)

5

c)

6

d)

8

e)

9

55.

a buffer solution is made by mixing HA, a weak acid, with salts containing A- ions.


HA ↔ H+ + A-


a formula that can be used for the calculation of the pH of this buffer solution is

a)
b)
c)
d)
56.

Ionic product of water increases if

a)

Pressure is reduced

b)

H + is added

c)

OH - is added

d)

Temperature is increased

57.

PH of 10-8M NaOH solution is

a)

8

b)

6.8

c)

7

d)

4

58.

Identify the order from the following rate constant : k =9.3×10-3 L mol-1s-1

a)

second order

b)

first order

c)

zero order

d)

third order

59.
Which of the following is true about acids and bases?
a)
The lower the pH, the stronger the acid
b)
the higher the pH, the stronger the acid
c)
The lower the pH, the more neutral the acid
d)
The higher the pH, the weaker the base
60.
Basic buffer is made up of
a)
weak base and weak acid
b)
weak base and its conjugate salt
c)
weak base and its conjugate acid
d)
strong base and its conjugate acid
61.

Who invented the pH scale?

a)

S.P.L.Sorenson

b)

Benjamin Franklin

c)

Henry Moseley

d)

Wilhelmina Rontgen

62.
Which of these pH values would indicate that a solution is a weak base?
a)
4
b)
5.6
c)
8
d)
13
63.
Which solution A and B of equal volume and concentration mixed together to form a buffer?
a)
Nitric acid and potassium hydroxide
b)
Nitric acid and potassium nitrate
c)
Propanoic acid and potassium hydroxide
d)
Propanoic acid and potassium propanoate
64.

pH change from 6.5 to 4.2 would indicate that a ___________ solution was added

a)

basic

b)

acidic

c)

buffer

65.

What is the Half life of this isotope?

a)

5 seconds

b)

10 seconds

c)

15 seconds

d)

20 seconds

66.
If one-fourth of the carbon-14 is remaining then how many half-lives have passed?
a)
1
b)
2
c)
3
d)
4
67.

After the third half-life, how much of the sample is left?

a)

1/2

b)

1/3

c)

1/16

d)

1/8

68.
The half-life of strontium-90 is 25 years. How much strontium-90 will remain after 100 years if the initial amount is 4.0 g?
a)
3.0g
b)
0.25mg
c)
0.3g
d)
0.25g
69.
The half-life of Zn-71 is 2.4 minutes. If one had 100.0 g at the beginning, how many grams would be left after 7.2 minutes has elapsed?
a)
100.0g
b)
50.0g
c)
12.5g
d)
8.5g
70.

it quantifies the ability of a solution to resist changes in pH by either absorbing or desorbing H+ and OH- ions.

a)

Buffer Capacity

b)

Buffer Solution

c)

Buffer Index

d)

Buffer Value

71.

What is the change in pH upon adding 0.024M of NaOH to a liter of a buffer containing 0.04M sodium bicarbonate and 0.04M acetic acid? (Ka = 1.75 X 10- 5M)

(a)  

72.

What is the pH of a buffer solution prepared with 0.05 M ammonia and 0.05 M ammonium chloride. The Kb value of ammonia is 1.80 × 10–5 at 25°C.

(a)  

73.

Molarity is measured in _____.

a)

moles per g.

b)

mols per L.

c)

moles per mm.

d)

moles per mL.

74.
What is the mass of 0.75 moles of (NH4)3PO4?
a)
101.75 g
b)
121.75 g
c)
111.75 g
d)
131.75 g
75.
How many moles of NaCl are present in a solution with a molarity of 8.59 M and a volume of 125 mL?
a)
1074 mol
b)
0.069 mol
c)
1.07 mol
d)
62.7 mol
76.

What do molarity and molality have in common?

a)

Both have "moles solute" in the numerator

b)

Both have "kg solvent" in the denominator

c)

Both have "L solution" in the denominator

d)

Both have "moles solution" in the denominator

77.
Total number of mol fraction for all component in the solution is equal to
a)
1.0
b)
0.95
c)
0.50
d)
2.0
78.

suppose a hydrochloric acid solution contains 36 g of HCl and 64 g of H2O.what is the mole fraction of HCl?

a)

0.78

b)

0.99

c)

0.22

d)

3.6

79.
How many moles of NaCl are present in a solution with a molarity of 8.59 M and a volume of 125 mL?
a)
1074 mol
b)
0.069 mol
c)
1.07 mol
d)
62.7 mol
80.

When calculating molality, Kg of the following are included in the calculation?

a)

solvent

b)

solute

c)

none of these

d)

solvent & solute

81.

40 grams of NaOH = ________ moles

a)

1

b)

2

c)

160

d)

1600

82.

If 1 mole of solute is dissolved in 1 liter of water, what is the molarity?

a)

2M

b)

.5M

c)

1M

d)

It can't be determined unless you know the solute

83.

When you make a dilution, which of these values remains constant?

a)

The molarity (M)

b)

The total moles of solute

c)

The volume (V)

d)

The concentration

84.

As we dilute a solution.....

a)

The volume increases and the molarity (M) increases

b)

The volume increases and the molarity (M) decreases

c)

The volume decreases and the molarity (M) increases

d)

The volume decreases and the molarity (M) decreases

85.

When a solution is heated until it boils, the molarity...

a)

Doesn't change because everything evaporates

b)

Decreases

c)

Increases

d)

Will become 1M

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