Free Printable Compound Stoichiometry

Worksheets

Compound Stoichiometry

Total questions: 56

Worksheet time: 2hrs 8mins

Name

Class

Date

What is the molar mass of Na₂CO₃?

22.99 g/mol

105.99 g/mol

96.00 g/mol

125.98 g/mol

What is the molar mass of of CO?

44.01 g/mol

16.00 g/mol

2.02 g/mol

28.01 g/mol

What is the molar mass of LiOH?

23.95 g/mol

18.02 g/mol

36.46 g/mol

112.15 g/mol

What is the molar mass of C₂H₄O₂?

Acetic Acid

100.09 g/mol

42.06 g/mol

60.06 g/mol

What is the molecular mass of fluorine gas, F₂?

What id the molar mass of UF₆?

101 g/mol

238 g/mol

257 g/mol

352 g/mol

Calculate the molar mass of Ba(C₂H₃O₂)₂

255.3 g/mol

237.3 g/mol

228.3 g/mol

196.3 g/mol

What is the percent by mass of oxygen in MgO?

20%

40%

50%

60%

What is the percent by mass of magnesium in MgO?

20%

40%

50%

60%

10.

What percent of CaF₂is Fluorine?

24%

49%

51%

65%

11.

Find the percent composition of Cu₂S?

%Cu= 67.987 %S= 32.013

%Cu= 79.854 %S= 20.145

%Cu= 35.946 %S= 64.054

12.

What is the percent composition of Benzene, C₆H₆?

C = 50%
H = 50%

C = 85.7 %
H = 14.3%

C = 92.2%
H = 7.8%

C = 71.9%
H = 28.1%

13.

Find the mass of 11.37 mol of BaO. Round to the nearest whole number.

1,354 g

1,740 g

17.40 g

1,684 g

14.

Determine the number of moles of AlNO₃ that are in 264 g of the compound.

2.97 mol

3.45 mol

2.73 mol

1.86 mol

15.

Which pair has the same empirical formula?

NaCrO₄ and Na₂Cr₂O₇

C₂H₄O₂ and C₆H₁₂O₆

C₃H₆O₃and C₂H₆O₂

CH₄ and C₂H₆

16.

A compound consists of 72.2% magnesium(Mg) and 27.8% nitrogen(N) by mass. What is the empirical formula?

Mg₄N₃

MgN₂

Mg₃N₂

MgN

17.

Which of the following is considered an empirical formula?

S₂O₄

C₆H₁₂O₆

H₂O

C₂H₄

18.

You are given the following percentages: 40.05% S and 59.95% O. Find the empirical formula for these elements.

SO₂

SO₃

SO₄

19.

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

Molecular Formula

Chemical Formula

Empirical Formula

Distance Formula

20.

Which pair has the same empirical formula?

NaCrO₄ and Na₂Cr₂O₇

C₂H₄O₂ and C₆H₁₂O₆

C₃H₆O₃and C₂H₆O₂

CH₄ and C₂H₆

21.

Glycerol has a molar mass of 92.09g/mol. Its percent composition is: 39.12% C, 8.75% H, and 51.12% O. What is the molecular formula for glycerol?

C₂H₃O₂

CH₂O

C₂H₄O₂

C₃H₈O₃

22.

A sample contains 36.95 g of mercury (Hg) and 13.05 g of chlorine (Cl). What is the empirical formula for this compound?

HgCl₂

Hg₃Cl

Hg₁₇Cl₃₆

HgCl

23.

What is the empirical formula if you have 36.84% nitrogen and 63.16% oxygen?

N₂O₄

N₂O₃

N₂O₅

24.

What is the empirical formula for P₂O₆?

P₂O₆

PO₃

P₃O

25.

What is the molecular formula for a compound with the empirical formula: K₂SO₄and a molecular mass of 696g.

K₂SO₄

K₈SO₁₆

K₈S₄O₈

K₈S₄O₁₆

26.

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

CH₂O

C₂H₄O₂

C₄H₈O₄

C₆H₁₂O₆

27.

Determine the empirical formula of a compound containing 63.50 % silver, 8.25 % nitrogen, and the remainder oxygen.

AgNO₃

Ag₂NO₃

AgNO₂

Ag₂N₂O₅

28.

What is the empirical formula for Si₂F₆?

SiF

Si₂F₆

SiF₃

Si₆F₂

29.

What is the molecular formula for a compound with the empirical formula: K₂SO₄and a molecular mass of 696g.

K₂SO₄

K₈SO₁₆

K₈S₄O₈

K₈S₄O₁₆

30.

A chemical formula that shows the actual # and kinds of atoms present in one molecule of a compound is called_________

ionic formula

covalent formula

empirical formula

molecular formula

31.

Which of the following could be a molecular formula with the empirical formula of CH₂O?

CH₂O₂

CHO

C₃H₅O₃

C₂H₄O₂

32.

What is the empirical formula of Na₂SO₄?

Na₂SO₄

NaSO₂

Na₂SO₂

NaSO₈

33.

Match the following

The actual number of atoms in a compound.

MOLECULAR FORMULA definition

The simplest reduced ratio of elements in a compound.

EMPIRICAL FORMULA defintion

$N_2O_4$

MOLECULAR FORMULA example

$NO_2$

EMPIRICAL FORMULA example

34.

MATCH THE EMPIRICAL AND MOLECULAR FORMULAS.

$N_2O_8$

$NO_4$

35.

A compound is found to be 69.6% iron (Fe) and 30.4% oxygen (O) by mass. What is the empirical formula of the compound?

FeO

Fe₂O₃

Fe₃O₄

FeO₂

36.

Match the following

The actual number of atoms in a compound.

MOLECULAR FORMULA definition

The simplest reduced ratio of elements in a compound.

EMPIRICAL FORMULA defintion

$N_2O_4$

MOLECULAR FORMULA example

$NO_2$

EMPIRICAL FORMULA example

37.

What is the molarity of 3 mole of hydrochloric acid in 3 L of water.

38.

What is the molarity of 4 grams of sodium chloride in 3,800 mL of solution?

0.018 M

0.018 mol

1.052 M

1.052 mol

39.

Molarity is measured in

moles per kg

mols per L

moles per kJ

moles per mL

40.

The ___ is the thing being dissolved

solute

solvent

41.

50 ml of a 1 M solution is diluted until the final volume is 80ml. How much water was added?

50 ml

1.3 ml

30 ml

130 ml

42.

Which sweet tea would you expect to taste the sweetest?

3.1M

2.5M

43.

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

The molarity (M)

The total moles of solute

The volume (V)

The concentration

44.

As we dilute a solution.....

The volume increases and the molarity (M) increases

The volume increases and the molarity (M) decreases

The volume decreases and the molarity (M) increases

The volume decreases and the molarity (M) decreases

45.

When Na₂O is added to water it reacts violently instead of making a solution. What is the molar mass of Na₂O?

62 g/mol

39 g/mol

55 g/mol

100 g/mol

46.

The term molar which is used to describe a solution's concentration, is written as?

mol

g/L

47.

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

Doesn't change because everything evaporates

Decreases

Increases

Will become 1M

48.

Molarity is ...

grams of solute/deciliters of solvent.

grams of solute/liters of solution.

moles of solute/liters of solution.

moles of solute/milliliters of solvent.

49.

2 moles of H₂O would weigh ____ grams

18 grams

9 grams

36 grams

2 grams

50.

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

15.9 M

0.636 M

0.642 M

1.59 M

51.

What is the molarity of a solution made by adding 1.565 moles of PbNO₃ to 500 mL?

300. M

31.3 M

3.13 M

1.56 M

52.

Which sweet tea would you expect to taste the least sweet?

3.1M

2.5M

53.

If you have 34 mL of a 0.5 M NaBr solution, what will the concentration be if 56 mL of water is added to it?

.188 M

3.78 M

.389 M

1.76 M

54.

The units "M" can also be written as:

mol/L

moles

g/L

g/mol

55.

40 grams of NaOH = ________ moles

160

1600

56.

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

.5M

It can't be determined unless you know the solute

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Compound Stoichiometry

Total questions: 56

Worksheet time: 2hrs 8mins

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