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Pam Owens

Columbia College
Other

Biography

I have a Bachelor's Degree in Chemistry and a Bachelor's Degree in Forensic Science. I was a College Chemistry Tutor for several years. I am currently a Crime Scene Investigator for a major metropolitan area. I am the Facilitator and Primary Instructor of our Crime Scene School.

Education

BA Chemistry
Columbia College
BS Forensic Science
Columbia College

Educator Statistics

Numerade tutor for 4 years
1333 Students Helped

Topics Covered

Unlocking the Power of Thermodynamics: A Comprehensive Guide
Unlocking the Power of Periodic Table Properties | Boost Your Knowledge
Periodic Table
Electromagnetic Waves
Understanding Electronic Structure: A Comprehensive Guide
Understanding Chemical Bonding: The Key to Molecular Structure
Understanding Structure and Bonding: A Comprehensive Guide
Exploring the Fascinating World of Thermochemistry | Learn More Today
Unlocking the Power of Composition: Tips and Techniques
Unlocking the Power of Chemical Reactions: A Comprehensive Guide
Energy in Thermal Processes
Energy of a System
Understanding Chemical Equilibrium: A Comprehensive Guide
Atoms, Molecules, and Ions: Understanding the Building Blocks of Matter
Mastering Chemical Reactions and Stoichiometry for Optimal Results
Explore the Fascinating World of Nuclear Chemistry
Discover the Wonders of Chemistry: Your Introductory Guide
Exploring the Chemistry of Nonmetals: Properties and Reactions
Exploring the Fascinating World of Transition Metals and Coordination Chemistry
Explore the Fascinating World of Molecular Geometry - Discover More!
Effective Solutions for Your Business Needs
Discover the Power of Liquids: Boost Your Health and Wellness Today!
Aqueous Solutions
Discover the Power of Solids for Your Everyday Needs
Unlock the Secrets of Organic Chemistry: Essential Guide
Discover the Power of Organic Compounds: Benefits and Uses
Acids and bases
Acid-Base Equilibria: Understanding the Balance
Understanding Acids and Bases: A Comprehensive Guide
Discover the Power of Gases: Benefits and Applications
Exploring the Fascinating World of Electrochemistry | Learn More Now

Pam's Textbook Answer Videos

06:18
Chemistry: Structure and Properties

Aspirin can be made in the laboratory by reacting acetic anhydride (C4H6O3) with salicylic acid (C7H6O3) to form aspirin (C9H8O4) and acetic acid (C2H4O2). The balanced equation is:
C4H6O3 + C7H6O3-C9H8O4 + C2H4O2

In a laboratory synthesis, a student begins with 3.00 mL of acetic anhydride (density = 1.08 g>mL) and 1.25 g of salicylic acid. Once the reaction is complete, the student collects 1.22 g of aspirin. Determine the limiting reactant, theoretical yield of aspirin, and percent yield for the reaction.

Chapter 7: Chemical Reactions and Chemical Quantities
Pam Owens
04:29
Chemistry Structure and Properties

Two substances $A$ and $B$ , initially at different temperatures, are thermally isolated from their surroundings and allowed to come into thermal contact. The mass of substance $A$ is twice the mass of substance B, but the specific heat capacity of substance $B$ is four times the specific heat capacity of substance A. Which substance will undergo a larger change in temperature?

Chapter 10: Thermochemistry
Pam Owens
06:26
Chemistry Matter and Change

Challenge Express each answer in scientific notation in the units indicated.
a. $\left(1.26 \times 10^{4} \mathrm{kg}\right)+\left(2.5 \times 10^{6} \mathrm{g}\right)$ in kg
b. $(7.06 \mathrm{g})+\left(1.2 \times 10^{-4} \mathrm{kg}\right)$ in $\mathrm{kg}$
c. $\left(4.39 \times 10^{5} \mathrm{kg}\right)-\left(2.8 \times 10^{7} \mathrm{g}\right)$ in $\mathrm{kg}$
d. $\left(5.36 \times 10^{-1} \mathrm{kg}\right)-\left(7.40 \times 10^{-2} \mathrm{kg}\right)$ in $\mathrm{g}$

Chapter 2: Analyzing Data
Pam Owens
07:31
Chemistry The Central Science

Write the chemical formula for each substance mentioned in the following word descriptions (use the front inside cover to find the symbols for the elements you do not know). (a) Zinc carbonate can be heated to form zinc oxide and carbon dioxide. (b) On treatment with hydrofluoric acid, silicon dioxide forms silicon tetrafluoride and water. (c) Sulfur dioxide reacts with water to form sulfurous acid. (d) The substance phosphorus trihydride, commonly called phosphine, is a toxic gas. (e) Perchloric acid reacts with cadmium to form
cadmium(II) perchlorate. (f) Vanadium(II) bromide is a colored solid.

Chapter 2: Atoms, Molecules, and lons
Pam Owens
04:40
Chemistry The Central Science

Consider the unit cells shown here for three different structures that are commonly observed for metallic elements.
(a) Which structure(s) corresponds to the densest packing of atoms? (b) Which structure(s) corresponds to the least dense packing of atoms?

Chapter 12: Solids and Modern Materials
Pam Owens
04:24
Chemistry

Variations in average atomic mass may be observed for elements obtained from different sources. Lithium provides an example of this. The isotopic composition of lithium from naturally occurring minerals is 7.5% $^{6} Li$ and 92.5% $^{7} Li,$ which have masses of 6.01512 amu and 7.01600 amu, respectively. A commercial source of lithium, recycled from a military source, was 3.75% $^{6} Li$ (and the rest $^{7} Li$). Calculate the average atomic mass values for each of these two sources.

Chapter 2: Atoms, Molecules, and Ions
Pam Owens
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Pam's Quick Ask Videos

05:30
Chemistry 101

1. A balloon with a volume of 15.0 L at 25°C and 1.0 atm is released. It rises to a height of 5,000 feet where the pressure is 632 mmHg and the temperature is 5°C. What is the new volume of the balloon?
2. A balloon with a volume of 550 mL at 1.0 atm rises to a height of 6.5 km where the pressure is 305 mmHg. Assuming the temperature remains constant, what is the new volume of the balloon?
3. A sample of oxygen gas occupies a volume of 1.2 L at 22°C. Calculate the temperature (in °C) at which the volume will reduce to 254 mL.

Pam Owens
02:54
Chemistry 101

1. When H2(g) reacts with C2H4(g) to form C2H6(g), 137 kJ of energy are evolved for each mole of H2(g) that reacts.
Write a balanced thermochemical equation for the reaction with an energy term in kJ as part of the equation. Note that the answer box for the energy term is case sensitive.
Use the SMALLEST INTEGER coefficients possible and put the energy term (including the units) in the last box on the appropriate side of the equation. If a box is not needed, leave it blank.

2. When NO(g) reacts with H2(g) to form N2(g) and H2O(l), 376 kJ of energy are evolved for each mole of NO(g) that reacts.
Write a balanced thermochemical equation for the reaction with an energy term in kJ as part of the equation. Note that the answer box for the energy term is case sensitive.
Use the SMALLEST INTEGER coefficients possible and put the energy term (including the units) in the last box on the appropriate side of the equation. If a box is not needed, leave it blank.

Pam Owens
03:51
Chemistry 101

Part A
The highest recorded temperature in the world was 46.0 °C in El Azizia, Libya, on September 13, 1922. Calculate this temperature in degrees Fahrenheit.
Express your answer using three significant figures.

Part B
The highest recorded temperature in the world was 46.0 °C in El Azizia, Libya, on September 13, 1922. Calculate this temperature in kelvins.
Express your answer using three significant figures.

Part C
The lowest recorded temperature in the world was -83.0 °C in Vostok, Antarctica, on July 21, 1983. Calculate this temperature in degrees Fahrenheit.
Express your answer using three significant figures.

Part D
The lowest recorded temperature in the world was -83.0 °C in Vostok, Antarctica, on July 21, 1983. Calculate this temperature in kelvins.
Express your answer using three significant figures.

Pam Owens
08:21
Chemistry 101

Convert 66.3 grams of SiS2 to molecules.
Convert 7.41 x 10^23 molecules of C2H2 to grams.
Convert 4.36 x 10^23 molecules of CH3OH to moles.
How many molecules are in 25 grams of water?
How many molecules are in 25 grams of NH3?
How many grams are in 8.2 x 10^23 molecules of N2I6?

Pam Owens
06:16
Chemistry 101

1. How many moles of Ba3(PO4)2 are in a sample containing 7.7*10^25 formula units of Ba3(PO4)2? Use dimensional analysis and show all your work.
2. What is the mass in grams of exactly one atom of mercury? Use dimensional analysis and show all your work.
3. A single atom of an element has a mass of 1.792*10^-22g. What is the atomic mass of this element? Use dimensional analysis and show all your work.
4. Given a bag containing 76.5 grams of calcium phosphate, how many moles of phosphorus does it contain? Use dimensional analysis and show all your work.

Pam Owens
05:26
Chemistry 101

a) Calculate the formula mass of methyl bromide, CH3Br. (Enter an unrounded value. Retain the number of decimal places from the periodic table.)
b) What is the molar mass of methanol if 1.556 mol methanol has a mass of 48.28 g?
c) What number of moles is equivalent to 7.12 × 10^21 atoms of Hg?
d) How many atoms are there in 38.7 g of tin (Sn)?

Pam Owens
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