Daniel Gosser

University of Toledo
Teacher

Biography

I'm an Education Specialist in Curriculum and Instruction with a focus in Chemistry. I have taught Chemistry and other sciences at the high school level for 14 years, and have taught college-level chemistry courses at my high school through Ohio's College Credit Plus program for the last 5 years.

Education

BS AYA Education
University of Toledo
MS Educational Technology
Bowling Green State University
MS Curriculum and Instruction
University of Toledo

Educator Statistics

Numerade tutor for 3 years
899 Students Helped

Topics Covered

Atoms, Molecules, and Ions: Understanding the Building Blocks of Matter
Exploring the Fascinating World of Thermochemistry | Learn More Today
Unlocking the Power of Thermodynamics: A Comprehensive Guide
Discover the Wonders of Chemistry: Your Introductory Guide
Understanding Chemical Equilibrium: A Comprehensive Guide
Unlocking the Power of Chemical Reactions: A Comprehensive Guide
Discover the Power of Kinetics: Unleash Your Potential
Exploring the Fascinating World of Electrochemistry | Learn More Now
Mastering Chemical Reactions and Stoichiometry for Optimal Results
Discover the Power of Liquids: Boost Your Health and Wellness Today!
Discover the Power of Solids for Your Everyday Needs
Understanding Electronic Structure: A Comprehensive Guide
Aqueous Equilibria: Understanding the Balance of Solutions
Unlocking the Power of Composition: Tips and Techniques
Explore the Fascinating World of Molecular Geometry - Discover More!
Find Your Dream Job: Discover the Best Work Opportunities
Unlock the Power of Kinetic Energy: Boost Your Efficiency Today
Save Energy and Money with Effective Conservation Techniques
Electromagnetic Waves
Periodic Table

Daniel's Textbook Answer Videos

01:17
Chemistry: Structure and Properties

Make a drawing of each unit cell: simple cubic, body-centered cubic, and face-centered cubic.

Chapter 12: Crystalline Solids and Modern Materials
Daniel Gosser
02:15
Chemistry The Central Science

Consider the combustion of liquid methanol, $\mathrm{CH}_{3} \mathrm{OH}(l) :$
$$\begin{aligned} \mathrm{CH}_{3} \mathrm{OH}(l)+\frac{3}{2} \mathrm{O}_{2}(g) \longrightarrow \mathrm{CO}_{2}(g)+2 \mathrm{H}_{2} \mathrm{O}(l) & \\ \Delta H &=-726.5 \mathrm{kJ} \end{aligned}$$ (a) What is the enthalpy change for the reverse reaction? (b) Balance the forward reaction with whole-number coefficients. What is $\Delta H$ for the reaction represented by this equation? (c) Which is more likely to be thermodynamically favored, the forward reaction or the reverse reaction? (d) If the reaction were written to produce $\mathrm{H}_{2} \mathrm{O}(g)$ instead of $\mathrm{H}_{2} \mathrm{O}(l),$ would you expect the magnitude of $\Delta H$ to increase, decrease, or stay the same? Explain.

Chapter 5: Thermochemistry
Daniel Gosser
04:01
Chemistry The Central Science

Methyl isocyanate, $\mathrm{CH}_{3} \mathrm{NCO},$ was made infamous in 1984 when an accidental leakage of this compound from a storage tank in Bhopal, India, resulted in the deaths of about 3800 people and severe and lasting injury to many thousands more. (a) Draw a Lewis structure for methyl isocyanate. (b) Draw a ball-and-stick model of the structure, including estimates of all the bond angles in the compound. (c) Predict all the bond distances in the molecule. (d) Do you predict that the molecule will have a dipole moment? Explain.

Chapter 9: Molecular Geometry and Bonding Theories
Daniel Gosser
01:48
Chemistry

At 500 $\mathrm{K}$ in the presence of a copper surface, ethanol decomposes according to the equation
$$
\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}(g) \longrightarrow \mathrm{CH}_{3} \mathrm{CHO}(g)+\mathrm{H}_{2}(g)
$$
The pressure of $\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}$ was measured as a function of time
and the following data were obtained:
since the pressure of a gas is directly proportional to the con- centration of gas, we can express the rate law for a gaseous reaction in terms of partial pressures. Using the above data, deduce the rate law, the integrated rate law, and the value of the rate constant, all in terms of pressure units in atm and time in seconds. Predict the pressure of $\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}$ after $900 .$ s from the start of the reaction. (Hint: To determine the order of the reaction with respect to $\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH},$ compare how the pressure of $\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}$ decreases with each time listing.)

Chapter 12: Chemical Kinetics
Daniel Gosser
03:13
Chemistry

The Ostwald process for the commercial production of nitric acid involves the following three steps:
$$4 \mathrm{NH}_{3}(g)+5 \mathrm{O}_{2}(g) \longrightarrow 4 \mathrm{NO}(g)+6 \mathrm{H}_{2} \mathrm{O}(g)$$
$$2 \mathrm{NO}(g)+\mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{NO}_{2}(g)$$
$$3 \mathrm{NO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow 2 \mathrm{HNO}_{3}(a q)+\mathrm{NO}(g)$$
a. Which reactions in the Ostwald process are oxidation–reduction reactions?
b. Identify each oxidizing agent and reducing agent.

Chapter 18: Electrochemistry
Daniel Gosser
1 2 3 4 5 ... 6

Daniel's Quick Ask Videos

01:57
Chemistry 101

Synthesis of p-nitroacetanilide experiment:
- Grams of limiting reagent used (acetanilide): 3.3 g
- Moles of limiting reagent used: 0.024 mol
- Theoretical yield: 0.024 mol (4.32 g)
- Actual yield: 0.00247 mol (0.445 g)
- Percent yield: 10%
- Typical percent yield: 40%
- Melting point range: 213-215

Questions:
1) Was the compound you synthesized pure? Explain.
2) Compare your yield with typical yield. If it is lower, give possible reasons.

Daniel Gosser
01:54
Chemistry 101

1) A voltaic cell is constructed from a standard Fe2+|Fe half-cell (E°red = -0.440V) and a standard Cu2+|Cu+ half-cell (E°red = 0.153V). (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank.)
The anode reaction is:
Fe(s) → Fe2+(aq) + 2e-

The cathode reaction is:
Cu2+(aq) + 2e- → Cu(s)

The spontaneous cell reaction is:
Fe(s) + Cu2+(aq) → Fe2+(aq) + Cu(s)

The cell voltage is V.

2) A voltaic cell is constructed from a standard Cr3+|Cr half-cell (E°red = -0.740V) and a standard Hg2+|Hg half-cell (E°red = 0.855V).
The anode reaction is:
Cr(s) → Cr3+(aq) + 3e-

The cathode reaction is:
Hg2+(aq) + 2e- → Hg(l)

The spontaneous cell reaction is:
Cr(s) + 2Hg2+(aq) → Cr3+(aq) + 2Hg(l)

The cell voltage is V.

Daniel Gosser
01:51
Chemistry 101

15. Which of the following statements regarding acid-base reactions is/are correct?
(i) 2HCl(aq) + Mg(OH)2(aq) → MgCl2(aq) + 2H2O(l) is an Arrhenius, Bronsted-Lowry, and a Lewis acid-base reaction.
(ii) H2SO4(d) + H3PO4(d) → H4PO4+(d) + HSO4–(d) is a Bronsted-Lowry and a Lewis acid-base reaction, but not an Arrhenius acid-base reaction.
(iii) SO2(d) + PCl3(d) → Cl3P–SO2(d) is a Lewis acid-base reaction, but not an Arrhenius or a Bronsted-Lowry acid-base reaction.

Multiple Choice:
a) only i and ii are true
b) only i and iii are true
c) only i is true
d) only ii and iii are true
e) i, ii, and iii are all true

Daniel Gosser
03:14
Chemistry 101

Create a species diagram (a plot of α vs pH) using excel for
carbonic acid dissociations that
are part of the CO2 equilibria system (for the species CO2(aq),
HCO3-, CO32-).

Daniel Gosser
04:08
Chemistry 101

CO32-

Electron Geometry ______________

Molecular Shape _______________

polar, non-polar, an ion __________

H2O

Electron Geometry ______________

Molecular Shape _______________

polar, non-polar, an ion __________

HCO2-

Electron Geometry ______________

Molecular Shape _______________

polar, non-polar, an ion __________

H2CCHF

Electron Geometry ______________

Molecular Shape _______________

polar, an ion __________

Daniel Gosser
02:33
Chemistry 101

Determining the Composition of a Star

Scientists cannot directly investigate the composition of stars, due to their extreme distances from Earth and their extreme temperatures. Fortunately, scientists have developed a method for investigating the composition of stars indirectly.

Stars are large balls of hot gases held together by their own gravity. The starlight that you see comes from gases on a star's outer surface. When exothermic nuclear reactions occur within a star, electrons that are found within the gaseous atoms of a star are promoted to higher energy levels. When these electrons return to their ground state, they emit the absorbed energy in the form of light radiation.

Astronomers use telescopes with diffraction gratings to separate starlight into its component wavelengths. They can identify gases within a star by comparing the star's spectrum to the spectra of various gases. Using this method, astronomers have discovered that most stars are mainly composed of hydrogen and helium. In fact, approximately 90% of the atoms in a star are hydrogen, making hydrogen the most abundant element in the universe!

The sun is our closest star. From its spectrum, scientists know that over 99.9% of atoms in the Sun are either hydrogen or helium. The remaining 0.1% include 67 other elements, such as oxygen, carbon, and nitrogen.

Scientists may not have discovered all the elements in the Sun. Since a star consists of many layers, light that is released from the inner layers is not necessarily detected because it cannot escape from the star. The challenge of the designers of modern astronomical instruments is to design instruments that can precisely measure the spectra of extremely faint stars.

Questions

1. Describe the method that astronomers use to determine the composition of a star (2 marks)
2. When observing a star's spectrum, you notice that the lines of certain elements are not present. Can you conclude that this element is not present in the star? Why or why not? (2 marks)
3. How do stars emit light? (2 marks)
4. In what ways can determining the composition of a star be considered qualitative analysis? (1 mark)

Daniel Gosser
1 2 3 4 5 ... 113