Free Printable Stoichiometry

1.

What is the mole ratio of H2O to H3PO4 in the following chemical equation?

a)

1 to 6

b)

3 to 2

c)

4 to 6

d)

2 to 3

2.

Knowing the mole ratio of a reactant and product in a chemical reaction would allow you to determine:

a)

the energy released in the reaction.

b)

the speed of the reaction.

c)

whether the reaction is reversible.

d)

the mass of the product produced from a known mass of reactant.

3.

In the reaction represented by the equation CH4(g) + O2(g) ----> CO2(g) + H2O(g), a mass of 125 g CH4 is reacted with excess oxygen. The expression:

a)

mass of oxygen redacted.

b)

mass of carbon dioxide produced.

c)

mass of water produced.

d)

none of the above.

4.

In the equation $6CO_2+6H_2O\ \rightarrow\ C_6H_{12}O_6+6O_2$ the mole ratio of water to oxygen is:

a)

2 : 1

b)

1 : 1

c)

3 : 2

d)

6 : 8

5.

The blue numbers in the image below represent ________

a)

I don't know, and don't want to try

b)

coefficients

c)

subscripts

d)

none of the answers are correct

6.

A number written in front of a chemical formula is called a(n)

a)

subscript

b)

superscript

c)

yield

d)

coefficient

7.

What is a coefficient?

a)

The small number on the right of the chemical symbol.

b)

The large number to the left of a formula.

8.

In the equation $Al_2\left(SO_4\right)3+3Ca\left(OH\right)_2\ \rightarrow\ 3CaSO_4\ +2Al\left(OH\right)_3$ , , the mole ratio of calcium hydroxide to aluminum hydroxide is:

a)

1 : 3

b)

2 : 3

c)

1 : 1

d)

3 : 2

9.

For the reaction represented by the equation N_2+3H_{2 ightarrow ext{2NH}_3}, how many moles of nitrogen (N2) are required to produce 18 grams of ammonia (NH3)?

a)

0.9 mol

b)

18 grams

c)

0.53 mol

d)

36 grams

10.

The most steps are required to solve stoichiometry problems when the reactant is given in grams and the product is sought in

a)

moles.

b)

grams.

c)

liters.

d)

number of atoms.

11.

Fill in the steps required to find the number of grams of substance B produced from the number of grams of substance A:

grams of A $\rightarrow$ ________ $\rightarrow$ _______ $\rightarrow$ ______= grams of B.

a)

$\frac{1\ mol\ of\ A}{Molar\ Mass\ of\ A^3};\ \frac{Molar\ Mass\ of\ B}{1\ mol\ of\ B};\ \frac{Moles\ of\ B}{Moles\ of\ A}$

b)

$\frac{1\ mol\ of\ A}{Molar\ Mass\ of\ A^3};\ \frac{Moles\ of\ B}{Moles\ of\ A};\ \frac{Molar\ Mass\ of\ B}{1\ mol\ of\ B}$

12.

For the reaction represented by the equation Pb\left(NO_3\right)_2+2KI\ \rightarrow\ PbI_2+2KNO_3 how many moles of lead iodide\left(PbI_2\right)are produced of 300 grams potassium iodide\left(KI\right) when Pb\left(NO_3\right)_2 is in excess?

a)

114.78 mol PbI₂

b)

0.904 grams PbI₂

c)

0.904 mol PbI₂

d)

114.78 grams PbI₂

13.

For the reaction represented by the equation $2KClO_3\rightarrow\ 2KCI+30_2$ how many grams of potassium chlorate are required to produce 160. g of oxygen?

a)

408 g KClO₃

b)

804 g KClO₃

c)

598 g KClO₃

d)

There is not enough information.

14.

___KNO₃ → ___KNO₂ + ___O₂

What coefficients are needed to balance the reaction?

a)

2, 2, 1

b)

2, 3, 2

c)

1, 2, 2

d)

1, 3, 1

15.

What is the first thing you must do to solve a stoichiometry problem?

a)

Write a Balanced Equation

b)

Write an Unbalanced Equation

c)

Panic

d)

Avogadro's Number

16.

2H₂ + O₂ --> 2H₂O

12 grams of H₂ are reacted with 36 grams of O₂.

What is the limiting reactant?

a)

Hydrogen

b)

Oxygen

c)

Water

d)

There is not a limiting reactant

17.

What is the excess reactant?

a)

Hydrogen

b)

Oxygen

c)

Water

d)

There is no excess reactant

18.

2H₂ + O₂ --> 2H₂O

12 grams of H₂ are reacted with 36 grams of O₂.

Calculate the amount of excess reactant.

a)

4.5 grams

b)

7.5 grams

c)

12.5 grams

d)

36.5 grams

19.

From the reaction: B₂H₆ + 3O₂ -->2 HBO₂ + 2 H₂O

What mass of O₂ will be needed to burn 36.1 g of B₂H₆?

B₂H₆ = 27.68 g/mol

a)

13.8 g O₂

b)

3.91 mol of O₂

c)

125 g O₂

d)

41.7 g O₂

20.

Balance this reaction: ____ RbNO₃ + ____ BeF₂ ----> ____ Be(NO₃)₂ + ____ RbF

a)

1,1,1,1

b)

1,2,1,1

c)

2,1,1,2

d)

2,1,2,1

21.

What is a Excess Reagent?

a)

amount you end with

b)

what you run out of first

c)

what you have left over

d)

what you start with

22.

In the reaction represented by the equation $2H_2 + O_2 \rightarrow 2H_2O$ , how many moles of water are produced from 4 moles of hydrogen gas?

a)

A) 2 moles

b)

B) 4 moles

c)

C) 6 moles

d)

D) 8 moles

23.

What is the molar mass of water (H2O)?

a)

A) 16 g/mol

b)

B) 18 g/mol

c)

C) 20 g/mol

d)

D) 22 g/mol

24.

In a stoichiometric calculation, if you start with 10 grams of carbon dioxide (CO2), how many grams of carbon (C) can be obtained? (Molar mass of CO2 = 44 g/mol, Molar mass of C = 12 g/mol)

a)

A) 2.73 grams

b)

B) 3.18 grams

c)

C) 4.55 grams

d)

D) 5.00 grams

25.

Which of the following best describes the concept of a limiting reactant in a chemical reaction?

a)

A) The reactant that is left over after the reaction is complete

b)

B) The reactant that determines the amount of product formed

c)

C) The reactant that reacts the fastest

d)

D) The reactant that has the highest molar mass

Stoichiometry

Total questions: 25

Worksheet time: 25mins

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