Luke Monroe

Towson University
Teaching Assistant

Biography

I graduated from in 2018 with B.S. in Chemistry. I am currently pursuing a PhD in chemistry with a focus on atmospheric particles and their impacts on the environment.

Education

BA Chemistry
Towson University

Educator Statistics

Numerade tutor for 4 years
644 Students Helped

Topics Covered

Unlocking the Power of Thermodynamics: A Comprehensive Guide
Discover the Wonders of Chemistry: Your Introductory Guide
Discover the Power of Liquids: Boost Your Health and Wellness Today!
Acid-Base Equilibria: Understanding the Balance
Understanding Chemical Equilibrium: A Comprehensive Guide
Aqueous Equilibria: Understanding the Balance of Solutions
Exploring the Fascinating World of Thermochemistry | Learn More Today

Luke's Textbook Answer Videos

06:17
Chemistry

The following diagrams represent solutions containing a weak acid $\mathrm{HA}\left(\mathrm{p} K_{\mathrm{a}}=5.0\right)$ and its sodium salt $\mathrm{NaA}$. (1) Which solution has the lowest pH? Which has the highest pH? (2) How many different species are present after the addition of two $\mathrm{H}^{+}$ ions to solution (a)? (3) How many different species are present after the addition of two OH - ions to solution (b)?

Chapter 17: Acid-Base Equilibria and Solubility Equilibria
Luke Monroe
09:55
Chemistry

A solution is made by mixing exactly 500 mL of $0.167 M \mathrm{NaOH}$ with exactly $500 \mathrm{mL}$ of $0.100 \mathrm{M} \mathrm{CH}_{3} \mathrm{COOH}$. Calculate the equilibrium concentrations of $\mathrm{H}^{+}, \mathrm{CH}_{3} \mathrm{COOH}, \mathrm{CH}_{3} \mathrm{COO}^{-}, \mathrm{OH}^{-}$
and $\mathrm{Na}^{+}$

Chapter 17: Acid-Base Equilibria and Solubility Equilibria
Luke Monroe
08:38
Chemistry

Calculate whether or not a precipitate will form if $2.00 \mathrm{mL}$ of $0.60 M \mathrm{NH}_{3}$ is added to $1.0 \mathrm{L}$ of $1.0 \times 10^{-3} \mathrm{M} \mathrm{FeSO}_{4}$

Chapter 17: Acid-Base Equilibria and Solubility Equilibria
Luke Monroe
03:29
Chemistry

Referring to Figure $18.1,$ we see that the probability of finding all 100 molecules in the same flask is $8 \times 10^{-31}$. Assuming that the age of the universe is 13 billion years, calculate the time in seconds during which this event can be observed.

Chapter 18: Entropy, Free Energy, and Equilibrium
Luke Monroe
05:48
Chemistry

The following diagram represents a gas-phase equilibrium mixture for the reaction $\mathrm{AB} \rightleftharpoons \mathrm{A}+\mathrm{B}$ at a certain temperature. Describe what would happen to the system after each of the following changes: (a) the temperature is decreased,
(b) the volume is increased, (c) He atoms are added to the mixture at constant volume, (d) a catalyst is added to the mixture.

Chapter 15: Chemical Equilibrium
Luke Monroe
1 2

Luke's Quick Ask Videos

02:42
Chemistry 101

A 32.80 g sample of a solid is placed in a flask. Toluene, in which the solid is insoluble, is added to the flask so that the total volume of solid and liquid together is 46.00 mL. The solid and toluene together weigh 58.36 g. The density of toluene at the temperature of the experiment is 0.864 g/mL.
What is the density of the solid?
Express your answer in grams per milliliter to three significant figures.

Luke Monroe
29:26
Chemistry 101

Phosphorous acid, H3PO3(aq), is a diprotic oxyacid that is an important compound in industry and agriculture.

pKa1 = 1.30
pKa2 = 6.70

Calculate the pH for each of the points in the titration of 50.0 mL of 1.5 M H3PO3(aq) with 1.5 M KOH(aq).

Before the addition of any KOH:
After addition of 25.0 mL KOH:
After addition of 50.0 mL KOH:
After addition of 75.0 mL KOH:
After addition of 100.0 mL KOH:

Luke Monroe
06:02
Chemistry 101

Using these molar enthalpy values:
(1) MgO(s) + 2 HCl(aq) → MgCl2(aq) + H2O(aq) ΔH1 = -134 kJ/mol
(2) Mg(s) + 2 HCl(aq) → MgCl2(aq) + H2(g) ΔH2 = -587 kJ/mol
(3) H2(g) + 1/2 O2(g) → H2O(l) ΔH3 = -285.84 kJ/mol
Calculate the enthalpy of reaction 4 using Hess's Law.
(4) Mg(s) + 1/2 O2(g) → MgO(s) ΔH4 = ??? kJ/mol

Luke Monroe
06:50
Chemistry 101

A buffer is created by combining 3.65 g of NH3 with 4.86 g of
HCl and diluting to a total volume of 800.0 mL .
Determine the pHpH of the buffer.
Express your answer using two decimal places.

Luke Monroe
04:21
Chemistry 101

Buffer capacity is a measure of a buffer solution's resistance
to changes in pH as strong acid or base is added. Suppose that you
have 115 mL of a buffer that is 0.220 M in both propanoic acid
(C2H5COOH) and its conjugate base (C2H5COO−). Calculate the
maximum volume of 0.460 M HCl that can be added to the buffer
before its buffering capacity is lost.

Luke Monroe
03:42
Chemistry 101

Calculate the solubility of CuCl in 0.10M CaCl2. Ksp of CuCl =
1.9 x 10^-7.

Luke Monroe
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