Free Printable CIA #3 Review Units 7-9 Chemistry

Worksheets

CIA #3 Review Units 7-9 Chemistry

Total questions: 45

Worksheet time: 23mins

Name

Class

Date

How many moles of potassium oxide (K2O) will be formed when 1.52 moles of potassium reacts with oxygen according to the following reaction: 4 K + O2 → 2 K2O?

0.76 moles

1.52 moles

0.38 moles

3.04 moles

How many moles of copper are needed to react with sulfur to produce 120 grams of copper(I) sulfide according to the following reaction: 2 Cu + S → Cu2S?

0.5 moles

1 mole

2 moles

3 moles

What mass of iron is needed to react with sulfur in order to produce 96 grams of iron (III) sulfide according to the following equation? 2 Fe + 3 S → Fe2S3.

32 grams

56 grams

64 grams

112 grams

What mass of zinc is needed to react with 23.1 g of phosphoric acid according to the following equation? $3 \text{Zn} + 2 \text{H}_3\text{PO}_4 \rightarrow 3 \text{H}_2 + \text{Zn}_3(\text{PO}_4)_2$

6.5 g

9.5 g

13.0 g

19.5 g

If 85 g of NH₄Cl reacts with 130 g of Ca(OH)₂ according to the following reaction, what is the maximum mass of ammonia that can be formed? $2 \text{NH}_4\text{Cl} + \text{Ca(OH)}_2 \rightarrow \text{CaCl}_2 + 2 \text{NH}_3 + 2 \text{H}_2\text{O}$

30.5 g

34.0 g

28.0 g

32.5 g

If 25 g of NH₃ and 96 g of H₂S react according to the following reaction, what is the maximum mass of ammonium sulfide that can be formed? $2 \text{NH}_3 + \text{H}_2\text{S} \rightarrow (\text{NH}_4)_2\text{S}$

68 g

78 g

88 g

98 g

When all of the limiting reactant is used, the reaction _______.

stops

continues

accelerates

reverses

14. How much heat is required to raise the temperature of a 825 g block of wood (specific heat = 1.8 J/g°C) from 22.0°C to 155.0°C?

196,020 J

197,020 J

198,020 J

199,020 J

Calculate the heat of formation for the following reaction: CH₄ + 3 Cl₂ → CHCl₃ + 3 HCl. Given the following information: CH₄ ΔH = -74.8 kJ, Cl₂ ΔH = -132.1 kJ, HCl ΔH = -76.0 kJ, CHCl₃ ΔH = -92.0 kJ.

-151.1 kJ

-200.0 kJ

-100.5 kJ

-50.0 kJ

10.

How many electrons can each of the following sublevels hold: s, p?

s = 2, p = 6

s = 1, p = 3

s = 2, p = 4

s = 3, p = 6

11.

Which of the following is the correct longhand electron configuration for the element Chlorine (Cl)?

1s² 2s² 2p⁶ 3s² 3p⁵

1s² 2s² 2p⁶ 3s² 3p⁶

1s² 2s² 2p⁶ 3s² 3p⁴

1s² 2s² 2p⁶ 3s² 3p³

12.

An Exothermic Reaction is a type of chemical reaction that:

absorbs energy from the surroundings

releases energy to the surroundings

does not involve any energy change

requires a catalyst to proceed

13.

What is an Endothermic Reaction?

A reaction that releases heat

A reaction that absorbs heat

A reaction that occurs spontaneously

A reaction that produces light

14.

Mole ratio of Carbon Dioxide to Iron Oxide: 2Fe2O3 + C → Fe + 3CO2. Fill in the blank: The mole ratio is ____.

3:2

2:3

1:1

3:1

15.

5. If the quantity is insufficient, what is the limiting reagent (LR)?

The reactant that is completely consumed first

The reactant that is left over

The product formed

The catalyst used

16.

What happens to KE when temperature increases?

KE increases

KE decreases

KE remains constant

KE fluctuates

17.

9. What is the heat required for specific heat capacity?

The heat required to raise the temperature of a unit mass of a substance by one degree Celsius.

The heat required to change the state of a substance without changing its temperature.

The heat required to increase the volume of a substance by one cubic meter.

The heat required to decrease the pressure of a substance by one pascal.

18.

Calculate the energy absorbed by 35g of copper. Given: m = 35g, c = 0.17, ΔT = 65-50 = 15.

89.25 J

75.00 J

100.50 J

120.00 J

19.

Find the specific heat. Given: q = 45, m = 18, ΔT = 20.

0.125 J/g°C

0.150 J/g°C

0.100 J/g°C

0.200 J/g°C

20.

18. All orbitals of equal energy are filled according to which rule?

Pauli Exclusion Principle

Hund's Rule

Aufbau Principle

Heisenberg Uncertainty Principle

21.

Endothermic reaction (a) energy.

22.

Solid to liquid to gas is an ________ process.

Endothermic

Exothermic

Isothermal

Adiabatic

23.

Burning is an (a) process.

24.

What is the electron configuration of Oxygen?

1s2 2s2 2p4

1s2 2s2 2p3

1s2 2s2 2p5

1s2 2s2 2p6

25.

What is the electron configuration of Chlorine?

1s2 2s2 2p6 3s2 3p5

1s2 2s2 2p6 3s2 3p6

1s2 2s2 2p6 3s2 3p4

1s2 2s2 2p6 3s2 3p3

26.

33. If you had 134.6g of calcium nitrate, calculate the theoretical yield in grams. Use the following calculation: 134.6g Ca(NO₃)₂ x 1mol/164.1g x 1mol/1mol x 293.8/1mol = 241.04g

241.04g

200.00g

150.00g

300.00g

27.

In the reaction below, what is the mole ratio of Carbon Dioxide to Iron Oxide? 2Fe_2O_3 + C → Fe + 3CO_2

3:2

3:1

2:3

2:1

28.

For the reaction FeNO3 + NaCl → NaNO3 + FeCl, how many moles of Iron Chloride, FeCl, are produced from 9 mole of Iron Nitrate, FeNO3?

4.5

29.

For the reaction Cl2 + 2CaBr → 2CaCl + Br2, how many moles of calcium chloride are produced from 130g of calcium bromide?

.54 mole

1.08 mole

2.16 mole

30.

For the reaction 2MgClO3 → 2MgCl + 3O2, how many grams of magnesium chlorate are required to produce 315 g of oxygen?

1413g

471g

235g

707g

31.

For the reaction CO3 + H2O → H2SO4, how many grams of sulfuric acid can be produced from 250g of carbon trioxide and 100g of water?

408g

544g

315g

289g

32.

The temperature of a substance increases as (a) .

Choose from the below words

the substance expands

the average kinetic energy of its particles increases

the substance's volume increases

the substance's mass increases

33.

The heat required to raise the temperature 1°C for every gram is called (a) ?

Choose from the below words

Thermal Energy

Specific Heat

Temperature

Kinetic Energy

34.

When the Limiting Reactant runs out, the reaction continues.

False

True

35.

Find the specific heat of an 18 g substance that absorbs 45 J when it is heated from 60°C to 80°C.

0.125 J

0.125 J/g °C

.04 J

.04 J/g °C

36.

How many electrons can the s sublevel hold?

The s sublevel can hold a maximum of 2 electrons.

The s sublevel can hold a maximum of 4 electrons.

The s sublevel can hold a maximum of 6 electrons.

The s sublevel can hold a maximum of 8 electrons.

37.

How many electrons can the p sublevel hold?

The p sublevel can hold a maximum of 6 electrons.

The p sublevel can hold a maximum of 2 electrons.

The p sublevel can hold a maximum of 8 electrons.

The p sublevel can hold a maximum of 10 electrons.

38.

How many electrons can the d sublevel hold?

39.

How many electrons can the f sublevel hold?

The f sublevel can hold a maximum of 14 electrons.

The f sublevel can hold a maximum of 10 electrons.

The f sublevel can hold a maximum of 8 electrons.

The f sublevel can hold a maximum of 12 electrons.

40.

All orbitals of equal energy are occupied by one electron before any single orbital is occupied by a second electron.

Aufbau principle

Pauli exclusion principle

Hund's rule

Core Notation

41.

In an endothermic reaction, energy is (a) .

Choose from the below words

absorbed

released

42.

27. In an exothermic reaction, energy is (a) .

Choose from the below words

absorbed

released

43.

What atom matches this electron configuration? 1s²2s²2p⁶3s²3p⁶4s²3d¹⁰

Zinc

Copper

Nickel

Germanium

44.

What electron configuration matches an oxygen atom?

1s²2s²2p⁶, 3p⁶4s²3d¹⁰4p⁵

1s²2s²2p⁴

1s²2s²2p⁶

1s²2s²2p⁶3s²3d¹⁰4s²3d¹

45.

Which electron configuration belongs to Chlorine (Cl)?

1s²2s²2p⁶3s²3p⁵

1s²2s²2p⁶3s²3p⁶

1s²2s²2p⁶3s²3p⁷

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CIA #3 Review Units 7-9 Chemistry

Total questions: 45

Worksheet time: 23mins

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