GIZMOS: Inclined Plane – Simple Machine Answer Key Feel the Heat Gizmos Answer Key with complete solution Gizmos_Student Exploration: MolesSE_2020 | Gizmos_MolesSE_Graded A GIZMO - Lab 22: Student Exploration Reaction Energy Answers


2019

Name: Date:

Student Exploration: Moles

Vocabulary: atomic mass, Avogadro constant, conversion factor, dimensional analysis, mole,

molar mass, molecular mass, scientific notation, significant figures, unified atomic mass unit

Prior Knowledge Questions (Do these BEFORE using the Gizmo.)

1. In the image to the right, note a dozen eggs, a dozen donuts and

a dozen roses. How many of each item do you have?

2. Would a dozen of each object have the same mass?

3. Suppose you have a dozen carbon atoms, a dozen gold atoms, and a dozen iron atoms.

Even though you have the same number of each, would you expect them all to have the

same mass? Explain.

Gizmo Warm-up

When counting roses, eggs, or donuts, a dozen is a good unit to

use. If you are counting atoms, however, a dozen is not much help.

In the Moles Gizmo, you will learn about a unit used to count atoms.

On the AVOGADRO CONSTANT tab, place the copper (Cu) atom

on the nano-balance on the left, which will show the average atomic

mass of copper rather than the mass of a single copper atom.

1. What is the average mass of a copper atom?

The unit “u” refers to unified atomic mass units. A single proton or neutron has a mass of

approximately one atomic mass unit. (Officially, 1 u is one-twelfth the mass of a C-12 atom.)

2. To gain an idea as to how many atoms are in a gram or so of copper, use the larger balance

on the right. Press Add atoms to put a scoop of atoms in the weighing dish, and keep

adding until the balance registers between 1 and 2 grams. If you don’t seem to be making

much progress, adjust the exponent using the slider, which will make the scoop size bigger.

How many atoms did you need to add?

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2019

Activity A:

Molar Mass

Get the Gizmo ready:

 Select the AVOGADRO CONSTANT tab.

 Turn on Show hints and check that Copper (Cu)

is selected.

Introduction: Since atoms are so tiny, chemists have devised a unit known as the mole. A

mole represents a macroscopic quantity of matter that can be used in the laboratory. One mole

of any element has the same mass in grams as its atomic mass in u.

Question: How many particles are in a mole?

1. Explore: Note the average atomic mass of copper on the nano-balance. Add atoms to the

larger balance until it registers the same number (in g) as the reading on the nano-balance

(in u). Use the Exponent slider to help get the correct amount. Stop adding atoms when the

readings on both balances match exactly (to the nearest 0.001 g).

How many atoms did you need to add?

2. Explore: Repeat the same procedure with carbon, then sulfur and aluminum.

A. For each element, how many atoms did you need to add?

B. What do you notice about the number of atoms in one mole?

3. Discover: In each case, you measured out one mole of atoms, since the mass of one mole

of any element, in grams, is equal to its atomic mass, in u. One mole of any element

contains the same number of atoms, a number known as the Avogadro constant.

What is the exact value of the Avogadro constant?

4. Illustrate: The Avogadro constant is so large it is normally written in scientific notation. To

get an idea of the enormity of the Avogadro constant, write it out in standard form. (You will

need to move the decimal place to the right 23 times, so you will need to add a lot of zeros!)

5. Compare: While the number of atoms in a mole is constant, the number of grams in a mole

changes based on the element. The number of grams in a mole (g/mol) is known as its

molar mass, and has the same numerical value as an element’s atomic mass (in u). Use

the Gizmo to find the atomic and molar mass of the following elements. Use proper units.

S: Atomic mass Molar mass

Al: Atomic mass Molar mass

(Activity A continued on next page)

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Name: Date:
Lab 22: Student Exploration: Reaction Energy
Directions: Follow the instructions to go through the simulation. Respond to the questions and
prompts in the orange boxes.
Vocabulary: calorimeter, chemical bond, endothermic, enthalpy, exothermic, Hess’s law
Prior Knowledge Questions (Do these BEFORE using the Gizmo.)
1. Two magnets are stuck together. What might you have to do to get them to separate?
Pull them apart
2. Suppose you held two magnets a short distance apart, then let go. What would happen?
Depends on which poles of the magnets were facing each other. If one was positive and
one was negative, they would be attracted to each other. If they were either both
positive or negative, they would repel.
3. Think about the magnets in terms of energy. In which case do you increase the potential energy of the
magnets? In which case do you increase the kinetic energy of the magnets?
Kinetic energy increases if you were to move magnets with the same charge towards
each other because they are going to repel. Potential energy would increase if they
were different poles because they are attracted to each other.
Gizmo Warm-up
Just like magnets, atoms of different elements are
attracted together to form chemical bonds. Breaking
these bonds requires energy. When a new bond forms,
energy is released and temperatures rise. In the Reaction
Energy Gizmo, you will explore how the energy of
chemical bonding relates to temperature changes that
occur during chemical reactions.
To begin, check that Reaction 1 and Forward are selected. In this reaction, hydrogen (H2) and oxygen (O2)
react to form water (H2O). The reaction takes place inside a device called a calorimeter. Inside the
calorimeter, a small chamber holds the reactants. The rest of the calorimeter is filled with water.
1. Click Play ( ). What happens?
Temperature increases, moving molecules.
2. How does the temperature change?
Increases
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Activity A:
Energy of
chemical bonds
Get the Gizmo ready:
● Check that Reaction 1 and Forward are selected.
● Select the INVESTIGATION tab.
Introduction: The heat energy stored in a chemical system is called the enthalpy (H) of the system. When
atoms are joined by a chemical bond, energy must be added to pull them apart. This increases the enthalpy of
the system. When a chemical bond forms, energy is released as shared electrons move into lower-energy
orbitals. This causes the enthalpy to decrease.
Question: How can you predict how much energy is released in a chemical reaction?
1. Predict: In the warm-up activity, you observed how the reaction inside the chamber affected the
temperature of the surrounding water. Based on what happens to the surrounding water, do you think heat
energy (enthalpy) is absorbed in the reaction or released? Explain.
Heat is released because the surrounding water is absorbing the heat (which we know
because the temperature increases).
2. Observe: In the Gizmo, the energy required to break a chemical bond is modeled by placing a molecule
into a set of mechanical claws. Place one of the hydrogen (H2) molecules between the claws, and press the
Break bond.
A. What happens? The bond between the atoms is broken and energy is absorbed.
B. Look under the Energy absorbed column of the table. How much energy was required to break this
bond?
436kJ/mol
Note: The energy is given here in units of kilojoules per mole (kJ/mol). This is the energy, in
kilojoules, required to break all of the H–H bonds in one mole of H2 gas.
C. Remove the hydrogen atoms from the claws and then break apart the other H–H molecule.
What is the total energy absorbed so far? 872kJ/mol
3. Measure: Notice that the oxygen atoms are connected by a double covalent bond. This is because the
oxygen atoms share two pairs of electrons. Place the oxygen molecule in the claws and press the Break
bond.
A. How much energy is required to break the first O–O bond? 349kJ/mol
Reproduction for educational use only. Public sharing or posting prohibited. © 2020 ExploreLearning™ All rights reserved
This study source was downloaded by 100000826990473 from cnn.com on 06-16-2021 15:38:01 GMT -05:00
https://www.cnn.com/file/87674338/GIZMO-Reaction-Energy-Answerspdf/
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