Free Printable Chemistry - Chemical Quantities Practice Test

Worksheets

Chemistry - Chemical Quantities Practice Test

Total questions: 59

Worksheet time: 2hrs 47mins

Name

Class

Date

What number must we use to convert between particles and moles?

Avocado's Number

The speed of light

Avogadro's Number

The mass of the compound

What is the conversion factor from liters to moles?

$\frac{22.4\ L}{1\ mol}$

$\frac{1\ mol}{22.4\ L}$

Six grams of carbon combine chemically with 2 grams of hydrogen to produce combustible gas. What is the empirical formula of this gas?

$CH$

$CH_4$

$C_2H_2$

$C_4H$

The empirical formula of hydrazine, molecular mass 64 grams, is $NH_2$ . What is the molecular formula?

$N_4H_8$

$N_2H_2$

$N_4H_2$

$N_4H_4$

If 15 moles of $O_2$ gas are produced, what is its mass?

240 g

2.133 g

480 g

1.067 g

What is the percent composition of each element of the compound $N_4H_8$ ?

N: 87.4% H: 12.6%

N: 12.6% H: 87.4%

N: 50% H: 50%

N: 75% H: 25%

When calculating the percent composition, what should all of the percentages add up to?

75 %

The number of atoms in the molecule

It should equal the total mass of the molecule

100%

How many moles are in $5\ x\ 10^{23}$ particles?

$3.01\ x\ 10^{47}$ mol

0.83 mol

1.204 mol

none of the above

How many liters are in 3.4 moles of a gas?

0.15 L

6.59 L

3.4 L

76.16 L

10.

What is the mass of 5 moles of $C_6H_{12}O_6$ ?

180.18 g

900.9 g

36.036 g

0.028 g

11.

What is the name of the following compound: K₂SO₄

potassium sulfur

potassium sulfate

potassium (I) sulfate

potassium (II) sulfide

12.

What is the name of the following compound: Mn₂O₃

manganese oxide

manganese (II) oxide

manganese (III) oxide

magnesium oxide

13.

The name of the compound Ca₃(PO₄)₂

calcium phosphate

tricalcium diphosphate

calcium phosphorus oxide

calcium phosphide

14.

What is the formula for calcium carbonate?

CaCO

CaCO₂

CaCO3

Ca3CO3

15.

What is the name of K₃PO₄?

Tripotassium Phosphate

Tripotassium Phosphite

Potassium phosphide

Potassium phosphate

16.

What is the percent by mass of fluorine in CaF₂(gram-formula mass = 78 g/mol)? include one decimal place and the percent sign.

(a)

17.

Find the percent composition of Cu₂S?

%Cu= 67.987 %S= 32.013

%Cu= 79.854 %S= 20.145

%Cu= 35.946 %S= 64.054

18.

Calculate the % composition by mass of oxygen present in H₂SO₄. include two decimal places and the percent sign in your answer.

(a)

19.

A compound consists of 72.2% magnesium and 27.8% nitrogen by mass. What is the empirical formula? Capitalize element symbols as appropriate. You do not have to format subscripts.

(a)

20.

A sample contains 36.95 g of mercury (Hg) and 13.05 g of chlorine (Cl). What is the empirical formula for this compound? Capitalize element symbols as appropriate. You do not have to format subscrtipts.

(a)

21.

What is the molecular formula for a compound with the empirical formula: K₂SO₄and a molecular mass of 696g. Capitalize element symbols as appropriate, you do not have to format subscripts.

(a)

22.

Phenyl magnesium bromide is used as a reagent in organic synthesis. Determine its empirical formula if its molar mass is 181.31 g/mol and it contains 39.75% C, 2.78% H, 13.41% Mg, and 44.07% Br (these are in the correct order). Capitalize element symbols as appropriate, you do not have to format subscripts.

(a)

23.

How many atoms are present in a 13.5 gram sample of beryllium?

1.5 particles

9 particles

4.03 x10²³ particles

9.02 x10²³ particles

24.

A sample of silver contains 5.71 x 10²² atoms. How many moles of silver are present? Use significant figures. Units are not required for this question.

(a)

25.

How many molecules are present in a 135 g sample of Teflon, which has a formula of C₂F₄?

6.13 x 10²³ molecules

5.13 x 10²³ molecules

8.13 x 10 ²³ molecules

9.13 x 10²³ molecules

26.

What is the total mass in grams of 0.75 mole of SO₂? Use significant figures, units are not required for this question.

(a)

27.

What is the number of moles in 9.63 L of H₂S gas at STP? Use significant figures. Units are not required for this question.

(a)

28.

What is the volume (in liters) of 3.20 moles of H₂O? Use significant figures, units are not required for this question.

(a)

29.

What is the SI unit for the amount of a substance?

meter

mass

molecule

mole

30.

What is the percent composition of nitrogen in NH₃?

25%

14%

28%

82%

31.

Which pair has the same empirical formula?

NaCrO₄ and Na₂Cr₂O₇

C₂H₄O₂ and C₆H₁₂O₆

C₃H₆O₃and C₂H₆O₂

CH₄ and C₂H₆

32.

A formula with the lowest whole # ratio of elements in a compound is called

Molecular Formula

Chemical Formula

Empirical Formula

Distance Formula

33.

What is the molecular formula if the empirical formula is CH₂O and the molecular molar mass is 180.18?

CH₂O

C₂H₄O₂

C₄H₈O₄

C₆H₁₂O₆

34.

C₆H₁₂O₆has how many total atoms?

35.

What is STP?

States of Temperature and Pressure, 1 $1\degree C$ 0 atm

Standard Tire Pressure, 65 psi

Standard Temperature and Pressure, $0\degree C$ 1 atm

Standard Timing and Pressure, 273 K 0 atm

36.

Diatomic molecules are __________ found in nature as their single element: I, O, N, H, Br, Cl, or H.

often

never

sometimes

always

37.

What is the molar mass of table salt (NaCl)?

116.886 g/mol

35.453 g/mol

22.990 g/mol

58.443 g/mol

38.

What is the molar mass of CO₂?

39.

Calculate the molar mass of Ba(C₂H₃O₂)₂

255.3 g/mol

237.3 g/mol

228.3 g/mol

196.3 g/mol

40.

What is the mass of one mole of Helium?

4 g

2 g

8 g

There is no way to know

41.

36.0 g of Be contains how many moles?

0.25 mol

4.0 mol

45 mol

320 mol

42.

How many grams are in 88.1 moles of magnesium?

2141 g

0.3 g

30 g

3.6 g

43.

How many hydrogen atoms are in the compound: (NH₄)₂CO₃

44.

What is Avogadro's Number?

6.02 x 10²³

- 6.02 10²³

6.02 x 10²²

6,020,000,000,000

45.

How many atoms of iodine are in 1 mole of iodine?

63.55

126.9

6.02 x 10²³

46.

How many molecules would be in 8.4 moles of Octane (C₈H₁₈)?

5.77 x 10²³

5.04 x 10²⁴

5.77 x 10²⁶

5.04 x 10²³

47.

Which has more molecules?

1 mole H₂O

1 mole Al(OH)₃

1 mole NaCl

They all contain the same number of molecules

48.

How many atoms of carbon are in 6.00g of carbon?

1.20x10²⁴atoms C

6.02x10²³atoms C

3.01x10²³atoms C

1.50x10²³atoms C

49.

What is the mass of 1.0 x 10¹² molecules of O₂?

1.9 x 10¹³ g

6.0 x 10¹¹ g

5.3 x 10^-11 g

1.7 x 10^-12 g

50.

What is the SI unit for a count of atoms?

meter

mass

molecule

mole

51.

Which of the following is an empirical formula?

C₃H₃

Li₂CO₃

Na₂O₂

C₆H₁₂O₆

52.

How many moles are contained in 45 grams of aluminum?

27 mol

1215 mol

1.7 mol

57 mol

53.

How many moles of chlorine gas are contained in 45 grams of pure sample?

35 mol

0.64 mol

1.3 mol

2.6 mol

54.

How many atoms of are contained in a mole of sodium?

6.02 x 10²³ atoms

11 atoms

23 atoms

2 atoms

55.

If the empirical formulas is CH and the molar mass is 78g/mol, what is the molecular formula?

C₆H₆

C₅H₁₈

6CH

56.

You have 55.0 g of CH₄. How many moles of hydrogen atoms would it contain? Enter you answer with the correct sig figs, and no units.

(a)

57.

You have 7.71 x 10²⁴ atoms of carbon that you got from Cr₂(CO₃)₃. How many moles of this compound did you start with?

4.27 moles

12.8 moles

38.4 moles

1.42 moles

58.

You have 4.82 moles of strontium nitrate (Sr(NO₃)₂). How many nitrogen atoms are there?

2.90 x 10²⁴ atoms N

6.02 x 10²³ atoms N

5.80 x 10²⁴ atoms N

3.61 x 10²⁴ atoms N

59.

You have 5.31 moles of Sn₃(PO₄)₄. How many moles of oxygen are there?

5.31

21.2

3.01

85.0

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Chemistry - Chemical Quantities Practice Test

Total questions: 59

Worksheet time: 2hrs 47mins

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