## Search found 66 matches

Wed Mar 13, 2019 8:25 pm
Forum: Reaction Mechanisms, Reaction Profiles
Topic: Pre-equilibrium approach
Replies: 4
Views: 116

### Re: Pre-equilibrium approach

shouse1f wrote:I know Lavelle mentioned the steady state approach but only went over the pre-equilibrium, so is the pre-equilibrium approach the only one we are expected to know?

Yep, he said that we are only required to know the pre-equilibrium one.
Wed Mar 13, 2019 8:18 pm
Forum: Kinetics vs. Thermodynamics Controlling a Reaction
Topic: rate constants at equilibrium
Replies: 2
Views: 249

### Re: rate constants at equilibrium

The rate constants of the forward and reverse are not always necessarily equal. Go off of the formula K=k/k'. Since K, in that case, is equal to one, we can say 1=k/k', which is the same as k=k'. However, the equilibrium constant K is not always 1.
Wed Mar 13, 2019 8:12 pm
Forum: Phase Changes & Related Calculations
Topic: Isothermic vs. Adiabatic
Replies: 3
Views: 262

### Re: Isothermic vs. Adiabatic

I think adiabatic means something has no heat transfer while isothermic means that there is no change in temperature, but in the overall scheme of things they both refer to q=0.
Sun Mar 10, 2019 1:03 am
Forum: Equilibrium Constants & Calculating Concentrations
Topic: Initial Concentration and Equilibrium Concentration
Replies: 3
Views: 167

### Re: Initial Concentration and Equilibrium Concentration

I'm guessing that the question is kind of talking about how relative to the equilibrium concentration, when there is more initial concentration, then the reaction tends to favor the products in order to reach the equilibrium concentrations. So there probably is a case where the product is smaller th...
Sun Mar 10, 2019 12:50 am
Forum: Equilibrium Constants & Calculating Concentrations
Topic: Kp
Replies: 7
Views: 206

### Re: Kp

As long as the units are consistent within the problem, any units of atm or bars is alright.
Sun Mar 10, 2019 12:47 am
Forum: General Science Questions
Topic: Discussion Section Test
Replies: 3
Views: 301

### Re: Discussion Section Test

Actually, I am not too sure because I put deltaG>0 for photosynthesis also, but it seems like they originally marked me off, but then crossed it out and gave me the points. I would talk with the TA for clarification.
Tue Feb 26, 2019 5:53 pm
Forum: Balancing Redox Reactions
Topic: Balancing Redox Reactions
Replies: 3
Views: 115

### Re: Balancing Redox Reactions

Cu was probably the reducing agent, meaning that the reaction occurred in the anode (since the other reaction must've had a larger Ecell value). This would mean that oxidation occurs in the anode, making the reaction the reverse reaction.
Tue Feb 26, 2019 5:40 pm
Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
Topic: Moles of electrons?
Replies: 6
Views: 146

### Re: Moles of electrons?

I usually did balance out the half reactions in order to determine the n. If there are any other ways, I would be glad to know too!
Tue Feb 26, 2019 5:39 pm
Forum: Appications of the Nernst Equation (e.g., Concentration Cells, Non-Standard Cell Potentials, Calculating Equilibrium Constants and pH)
Topic: Contradictory Ecell equations
Replies: 2
Views: 83

### Re: Contradictory Ecell equations

The equations should be the same because cathodes are actually always on the right, and the anodes are always on the left.
Fri Feb 22, 2019 12:36 pm
Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
Topic: Galvanic Cells
Replies: 2
Views: 59

### Re: Galvanic Cells

The electrons from the anode are negatively charged, meaning that they want to flow towards the positive charge, which is at the cathode
Fri Feb 22, 2019 12:31 pm
Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
Topic: Proportionality and current?
Replies: 2
Views: 80

### Re: Proportionality and current?

Yes, I do believe so based on Faraday's Laws
Fri Feb 22, 2019 12:21 pm
Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
Topic: Cell potential and Gibbs free energy
Replies: 2
Views: 70

### Re: Cell potential and Gibbs free energy

That is because in the equation ΔG = - nFE, a positive cell potential is associated with a negative Gibbs free energy, which means a reaction is spontaneous. A negative cell potential would make the Gibbs free energy positive, meaning that the reaction is no longer spontaneous.
Fri Feb 22, 2019 12:16 pm
Forum: Balancing Redox Reactions
Topic: OH-, Adams, Disc 1A
Replies: 3
Views: 84

### Re: OH-, Adams, Disc 1A

You would use OH- when balancing a basic solution. I would refer to toolbox 6K.1 and example 6K.2 in the 7th edition for a better guideline on the use of OH-.
Wed Feb 13, 2019 4:35 am
Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
Topic: HOTDOG #12 part B
Replies: 6
Views: 218

### Re: HOTDOG #12 part B

(1)(219.2)(163)+(6)(29.4)(163) only gives you part of the answer as you need to heat it up from 37 to 200, then use the DeltaHrxn then cool it down from 200 to 37. DeltaH1=(1)(219.2)(163)+(6)(29.4)(163) DeltaH2=-2756kJ DeltaH3=(6)(37.1)(-163)+(6)(75.3)(-163) DeltaH1+DeltaH2+DeltaH3 Should give you ...
Wed Feb 13, 2019 4:02 am
Forum: Calculating Work of Expansion
Topic: Expansion Against a Vacuum
Replies: 4
Views: 150

### Re: Expansion Against a Vacuum

When the gas is expanding in a vacuum, there is nothing to oppose the gas (free expansion), making the work = 0. In a vacuum, there is also no change in temperature or heat change, making delta U = 0, thus q= 0. delta S in free expansion would still be equal to nRln(V2/V1).
Wed Feb 13, 2019 2:44 am
Forum: Entropy Changes Due to Changes in Volume and Temperature
Topic: Hotdog #5
Replies: 6
Views: 650

### Re: Hotdog #5

I'm guessing that because the problem doesn't say that the pressure is independent of the temperature, the change in temperature affects a change in the pressure of the system.
Thu Feb 07, 2019 6:47 pm
Forum: Calculating Standard Reaction Entropies (e.g. , Using Standard Molar Entropies)
Topic: Statistical vs Residual Entropy
Replies: 4
Views: 125

### Re: Statistical vs Residual Entropy

I think statistical and residual are the same except that for residual entropy, the system does not account for thermal entropy, meaning T=0. I think the large error in W means that there is a large error in determining the number of states possible? This part I am not too sure.
Thu Feb 07, 2019 6:34 pm
Forum: Entropy Changes Due to Changes in Volume and Temperature
Topic: Difference between 2 delta S equations?
Replies: 1
Views: 73

### Re: Difference between 2 delta S equations?

The book is a little inconsistent with their variables, but if you look at the example following the formula, they do use ΔS = nCln(T2/T1). So I'm just guessing they combine the n with C in the book, but both ultimately do use ΔS = nCln(T2/T1).
Thu Feb 07, 2019 6:23 pm
Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
Topic: 4D7
Replies: 2
Views: 96

### Re: 4D7

The change in internal energy is ΔU = q + w. The problem gives you q as q = -318 kJ, so we have to find w, or the work done in by the system due to the reaction. w could be found by -PΔV, which means ΔU = q + -PΔV. Because they did not give the volume or pressure, we could convert -PΔV to -ΔnRT beca...
Wed Jan 30, 2019 12:11 pm
Forum: Calculating Work of Expansion
Topic: Work
Replies: 2
Views: 83

### Re: Work

Adding on, a reversible and isothermal path should be at equilibrium.
Wed Jan 30, 2019 12:07 pm
Forum: Heat Capacities, Calorimeters & Calorimetry Calculations
Topic: Regular heat capacity: why?
Replies: 4
Views: 136

### Re: Regular heat capacity: why?

I guess that heat capacity will just give you quick information about the energy needed to raise a specific amount of substance, but I do agree that specific heat capacity is more useful in that it could just calculate the heat capacity of that amount of a substance anyway.
Wed Jan 30, 2019 12:03 pm
Forum: Heat Capacities, Calorimeters & Calorimetry Calculations
Topic: Extensive vs. Intensive
Replies: 5
Views: 162

### Re: Extensive vs. Intensive

Extensive means that the properties can change based on the amount of substance (so conditions such as mass and volume), while intensive means that the properties are independent of the amount of substance (so mass and volume would not change an intensive value).
Tue Jan 22, 2019 10:30 pm
Forum: Applying Le Chatelier's Principle to Changes in Chemical & Physical Conditions
Topic: Increasing the pressure (decreasing volume)
Replies: 2
Views: 65

### Re: Increasing the pressure (decreasing volume)

The new concentrations can be determined by using PV = nRT. If V is halved, so P(V/2) = nRT, making P = (2n/V)RT, the concentrations are doubled, making the new concentrations to be 3.7 M H2, 2.72 M N2, and 5.82 x10^-3 M NH3.
Tue Jan 22, 2019 10:25 pm
Forum: Equilibrium Constants & Calculating Concentrations
Topic: Kp
Replies: 3
Views: 97

### Re: Kp

It does not really matter since the units will cancel out anyways, and using both bar or atm will get the same Kp value.
Tue Jan 22, 2019 10:24 pm
Forum: Equilibrium Constants & Calculating Concentrations
Topic: Protonation
Replies: 2
Views: 44

### Re: Protonation

Protonation is the adding of a proton to an atom. Percent protonated is the percent of the atoms that added a proton to an atom in a reaction since for weaker acids and bases, not all atoms protonate.
Tue Jan 15, 2019 10:06 pm
Forum: Equilibrium Constants & Calculating Concentrations
Topic: 11.59
Replies: 3
Views: 97

### Re: 11.59

If you plug in the larger positive x value, you will find that the equilibrium concentrations of the reactants are negative, and that is not possible, meaning that value can be disregarded. Therefore, there would be only one valid x value.
Tue Jan 15, 2019 10:01 pm
Forum: Equilibrium Constants & Calculating Concentrations
Topic: Question Focus 5I.17 7th edition
Replies: 1
Views: 39

### Re: Question Focus 5I.17 7th edition

if you do not look at the conclusion the solution manual gives, calculating the equilibrium concentration for N2 and O2 would be .114-X, X being equal to 1.8x10^-4. .114-1.8x^10-4 = .1138, which is essentially .114 mol/L.
Tue Jan 15, 2019 9:57 pm
Forum: Equilibrium Constants & Calculating Concentrations
Topic: Relationship between pKa, pKb, and pH
Replies: 1
Views: 34

### Re: Relationship between pKa, pKb, and pH

Given a pKa value, you can convert the pKa to Ka using pKa = -logKa. Because Ka = [H+][A-]/[HA], you could find [H+] .
-log[H+] would give the pH.
Wed Jan 09, 2019 12:31 pm
Forum: Equilibrium Constants & Calculating Concentrations
Topic: "lie to the right" vs "shifted to the right"
Replies: 6
Views: 77

### Re: "lie to the right" vs "shifted to the right"

Both essentially mean there are more products than reactants, but I'm assuming "lie to the right" refers to when the reaction has not yet reached equilibrium yet, while "equilibrium shifted to the right" has the equation already at equilibrium. that makes sense! But what does it...
Wed Jan 09, 2019 12:29 pm
Forum: Equilibrium Constants & Calculating Concentrations
Topic: 7th Edition 5G.3
Replies: 1
Views: 16

### Re: 7th Edition 5G.3

Yes, generally when the equilibrium constant deals with an equation with only gases in the formula K= [Producrs]/[Reactants], we use partial pressure as the concentration, labeled as "P". There really isn't a difference in the calculations when writing "P" and without it, but if ...
Wed Jan 09, 2019 12:22 pm
Forum: Equilibrium Constants & Calculating Concentrations
Topic: "lie to the right" vs "shifted to the right"
Replies: 6
Views: 77

### Re: "lie to the right" vs "shifted to the right"

Both essentially mean there are more products than reactants, but I'm assuming "lie to the right" refers to when the reaction has not yet reached equilibrium yet, while "equilibrium shifted to the right" has the equation already at equilibrium.
Wed Jan 09, 2019 12:16 pm
Forum: Equilibrium Constants & Calculating Concentrations
Topic: Ratios of Concentration
Replies: 1
Views: 29

### Re: Ratios of Concentration

If I interpreted the question correctly, the stoichiometric coefficients don't change in an equation unless if the equation was not balanced in the first place. If "coefficients" refers to the differing concentrations, then yes the ratio of concentrations between products and reactants wou...
Sat Dec 08, 2018 1:56 am
Forum: Polyprotic Acids & Bases
Topic: Strong Acids - HClO4 and HClO3
Replies: 1
Views: 1373

### Re: Strong Acids - HClO4 and HClO3

HClO4 is still neutral because we can look at the formal charges in the Lewis structure to determine the charge of HClO4. The Cl atom would have three double bonds with three oxygen atoms and one single bond with OH, causing the formal charge of Cl to be 0 (7-(0+14/2)). All the oxygens will also hav...
Thu Dec 06, 2018 7:19 pm
Forum: Properties & Structures of Inorganic & Organic Acids
Topic: Strongs Acids
Replies: 4
Views: 351

### Re: Strongs Acids

I think some strong acids to know are in group 17 ( HCl, HBr, HI) and nitric acid, (HNO3), sulfuric acid (H2SO4), perchloric acid (HCLO4), and chloric acid (HClO3).
Thu Dec 06, 2018 6:16 pm
Forum: Shape, Structure, Coordination Number, Ligands
Topic: Neutral Ligand
Replies: 2
Views: 83

### Re: Neutral Ligand

A neutral ligand would be a molecule that attaches to a central metallic atom, examples being H2O, CO, NH3, etc.
Thu Dec 06, 2018 6:11 pm
Forum: Properties & Structures of Inorganic & Organic Acids
Topic: Determining Lewis Acids and Bases
Replies: 1
Views: 55

### Re: Determining Lewis Acids and Bases

The Lewis acid will be the compound that is the electron acceptor while the Lewis base would be the compound that is the electron donor. So in something Like Na+ + Cl- -> NaCl, Na+ will be the Lewis acid and Cl- would be the Lewis base.
Tue Nov 27, 2018 6:35 pm
Forum: Determining Molecular Shape (VSEPR)
Topic: Seesaw Shape Bond Angles
Replies: 8
Views: 240

### Re: Seesaw Shape Bond Angles

The bond angles are less than 90 and 120 degrees.
Tue Nov 27, 2018 6:35 pm
Forum: Dipole Moments
Topic: LDF
Replies: 5
Views: 212

### Re: LDF

Yep, all molecules should have LDF!
Tue Nov 27, 2018 6:33 pm
Forum: Determining Molecular Shape (VSEPR)
Topic: Bond Angles
Replies: 3
Views: 79

### Re: Bond Angles

The bond angles are the following:
See-saw: less than 90 and 120 degrees
T-Shape: less than 90 degrees
Square Pyramidal: less than 90 degrees
Square Planar: 90 degrees
Tue Nov 27, 2018 6:17 pm
Forum: Hybridization
Topic: Hybridization of Central Atom
Replies: 3
Views: 128

### Re: Hybridization of Central Atom

I think it is because carbon is on the second row of the periodic table, making it 2.
Sat Nov 24, 2018 1:46 am
Forum: Sigma & Pi Bonds
Topic: Delta Bonds
Replies: 4
Views: 141

### Delta Bonds

How are delta bonds formed?
Sat Nov 24, 2018 1:30 am
Forum: Hybridization
Topic: 2.45 (7th ed)
Replies: 1
Views: 88

### Re: 2.45 (7th ed)

I am guessing since the lone pairs are not part of a sigma or a pi bond, the 2 is not included in the notation. There might not be a need for the distinguishment for the second row when there are no bonds with lone pairs.
Wed Nov 21, 2018 3:02 am
Forum: Sigma & Pi Bonds
Topic: formation of pi bond
Replies: 6
Views: 209

### Re: formation of pi bond

I do not think so, pi bonds are formed only after a sigma bond has formed.
Tue Nov 13, 2018 8:54 pm
Forum: Lewis Structures
Topic: Lewis Structure
Replies: 3
Views: 184

### Re: Lewis Structure

Hey Nicolette,
I think there actually are 3 lone pairs on the Cl instead of 2, or else the total valence electrons would not match up
Tue Nov 13, 2018 8:49 pm
Forum: Interionic and Intermolecular Forces (Ion-Ion, Ion-Dipole, Dipole-Dipole, Dipole-Induced Dipole, Dispersion/Induced Dipole-Induced Dipole/London Forces, Hydrogen Bonding)
Topic: dipole dipole and london forces
Replies: 2
Views: 67

### Re: dipole dipole and london forces

London forces occur in all molecules (non-polar and polar), while dipole-dipole forces occur only in polar molecules. Dipole-dipole is the result of an attraction of a positive charge on one side of a molecule to the negative charge on another molecule. London forces occur in all molecules because e...
Tue Nov 13, 2018 8:30 pm
Forum: Determining Molecular Shape (VSEPR)
Topic: Difference between molecular shape & shape
Replies: 2
Views: 91

### Re: Difference between molecular shape & shape

Yeah, I think the terms are interchangeable as both point to the shape of the molecule, so both molecular shape and shape do not exclude lone pairs
Tue Nov 13, 2018 7:54 pm
Forum: Determining Molecular Shape (VSEPR)
Topic: VSEPR Formula
Replies: 3
Views: 100

### Re: VSEPR Formula

We have kind of gone over the general VSEPR concept, but I do not think we have looked over all the shapes and their bond angles in class yet. For 2E.13, I would just find the number of bonds and lone pairs and then determine the shape and bond angle with that information through figure 2E.1 or any ...
Mon Nov 05, 2018 2:42 pm
Forum: Administrative Questions and Class Announcements
Topic: Wavelengths
Replies: 3
Views: 120

### Re: Wavelengths

Generally, anything below 10^-18 m in wavelength is undetectable making that the shortest.
Sat Nov 03, 2018 9:17 pm
Forum: Lewis Structures
Topic: 2C.5 part c (7th edition)
Replies: 2
Views: 69

### Re: 2C.5 part c (7th edition)

The nitrogen cannot have an expanded octet, thus it cannot form five bonds. There are no available d-orbitals for nitrogen to have that expanded octet for two double bonds with the oxygen and one single bond.
Mon Oct 29, 2018 11:06 pm
Forum: Formal Charge and Oxidation Numbers
Topic: Formal Charge of Ions
Replies: 9
Views: 318

### Re: Formal Charge of Ions

I think Dr. Lavelle meant for the central atom of sulfur to have a formal charge of 0, but the overall formal charge to stay at 2-. For sulfur here, with 6 valence electrons, in the formula FC = V - (l + s/2), FC = 6-(0 +12/2), FC=0.
Mon Oct 29, 2018 10:51 pm
Forum: Lewis Structures
Topic: D block valence electrons
Replies: 2
Views: 53

### Re: D block valence electrons

You only count the s and p block electrons. You do not count the d block electrons because the d block would not be part of the outermost shell. For instance, with gallium, [3d104s24p1], the s and p are in the same larger shell than d (4 compared to 3). For transition metals, groups 3-11, they are a...
Mon Oct 29, 2018 10:32 pm
Forum: Lewis Structures
Topic: Valence Electrons in d orbital
Replies: 2
Views: 85

### Re: Valence Electrons in d orbital

Valence electrons refer to the outermost electrons in the outermost shells, so usually when an atom has a d orbital, you would just count the electrons in the s and p shells. If you are referring to how many electrons can be in each orbital of the d shell, then yes there can be one or two electrons ...
Mon Oct 22, 2018 10:57 pm
Forum: Heisenberg Indeterminacy (Uncertainty) Equation
Topic: Formula confusion
Replies: 5
Views: 86

### Re: Formula confusion

The h constant would be given on the test
Mon Oct 22, 2018 10:56 pm
Forum: Heisenberg Indeterminacy (Uncertainty) Equation
Topic: Formula confusion
Replies: 5
Views: 86

### Re: Formula confusion

The h in the heisenberg equation actually has a slash through the h, which symbolizes h/2π. This means that the "h" variable, the planck constant, 6.63 x 10^-34 Js is the same in both the wavelength = hp and heisenberg equation.
Mon Oct 22, 2018 10:26 pm
Forum: Bohr Frequency Condition, H-Atom , Atomic Spectroscopy
Topic: post assessment
Replies: 1
Views: 60

### Re: post assessment

I'm sure that the value 1.22 x10^-7 is correct, but you have to also be aware that the negative that you got from the calculations earlier comes from the hydrogen atom emitting energy. This means that when the problem asks for the wavelength, the wavelength must have a positive value because a negat...
Mon Oct 22, 2018 10:10 pm
Forum: Einstein Equation
Topic: De Broglie's
Replies: 4
Views: 403

### Re: De Broglie's

I think it depends on the problem at hand, most likely the problem would state if you need to use the weight of a neutron or proton or a car. However, the weight of a neutron and proton are very similar and almost essentially the same at 1.67 x 10^-27 kg.
Fri Oct 19, 2018 12:17 pm
Forum: *Black Body Radiation
Topic: Test
Replies: 9
Views: 610

### Re: Test

HI, I don't think so, the professor said that we do not have to go over it.
Mon Oct 15, 2018 10:17 pm
Forum: Properties of Electrons
Topic: Detectable Electron Wavelength
Replies: 2
Views: 84

### Re: Detectable Electron Wavelength

I think anything generally shorter than 10^-18 m for wavelength
Mon Oct 15, 2018 10:10 pm
Forum: Bohr Frequency Condition, H-Atom , Atomic Spectroscopy
Topic: Rydberg Equation
Replies: 4
Views: 124

### Re: Rydberg Equation

Hi, the Rydberg Equation is just a derivation of ΔEn = Efinal - Einitial, with En = -hR/n^2. In other words, it is just the simplified form to find the change in energy from one energy level to another for the frequency or 1/λ. The professor wanted to show how this formula was derived, but I think i...
Tue Oct 09, 2018 2:53 am
Forum: Empirical & Molecular Formulas
Topic: Polyatomic Ions and Naming
Replies: 3
Views: 310

### Re: Polyatomic Ions and Naming

I'm not a hundred percent sure, but I think it would be best to look over the names of the polyatomic ions again and refresh your memory since on the tests there might be word problems where only the chemical name is given and you would have to derive the chemical formula yourself. It doesn't hurt t...
Tue Oct 09, 2018 2:43 am
Forum: Limiting Reactant Calculations
Topic: Help with M9?
Replies: 2
Views: 733

### Re: Help with M9?

So first, you have the balanced equation: Cu(NO3)2 + 2NaOH --> Cu(OH)2 + 2NaNO3 The next step after this is to find the moles of the reactants in order to find the limiting reactant. So for Cu(NO3)2: n/L =M n/.08L = .500M n = .04 moles Cu(NO3)2 And for NaOH: molar mass: 22.99g/mol Na + 16 g/mol O + ...
Tue Oct 09, 2018 2:24 am
Forum: Limiting Reactant Calculations
Topic: How to find the limiting reactant easily and quickly
Replies: 5
Views: 745

### Re: How to find the limiting reactant easily and quickly

What I usually do is first make sure that the chemical equation is balanced, and then I try to convert the grams of the reactants to moles (unless the problem already gives the number of moles of each reactant). Then, I would take these mole values and divide them by the stoichiometric coefficients ...
Tue Oct 02, 2018 4:46 pm
Forum: Limiting Reactant Calculations
Topic: HW Question M.5
Replies: 2
Views: 101

### Re: HW Question M.5

BrF_3 is the excess because although there are 12 moles of ClO_2 present to react with only 5 moles of BrF_3, the chemical equation (6 ClO_2(g) + 2 BrF_3(l) --> 6 ClO_2F(s) + Br_2(l)) shows that 6 moles of ClO_2 would react with 2 of the moles of BrF_3 for one reaction. After two reactions, 12 moles...
Tue Oct 02, 2018 4:33 pm
Forum: Empirical & Molecular Formulas
Topic: problem F13
Replies: 3
Views: 142

### Re: problem F13

I think the solutions manual skips finding the mass percentage of each element in this problem because the mass percentage, in this case, would only be needed to find the mass of each element and the problem already gives the mass of phosphorus (4.14g) and chlorine (27.8-4.14g). With this, you can l...
Mon Oct 01, 2018 6:46 pm
Forum: Balancing Chemical Reactions
Topic: States of Atoms
Replies: 7
Views: 139

### Re: States of Atoms

Yea usually I would just look it up since we have not really gone over determining the states of the atom in class. The states of molecules will generally be gas (g), liquid (l), solid (s), or aqueous (aq) (when the molecule is dissolved in water). Often times the word problem may give hints to what...
Mon Oct 01, 2018 6:37 pm
Forum: Empirical & Molecular Formulas
Topic: Chemical Equations?
Replies: 4
Views: 243

### Re: Chemical Equations?

The coefficients in a chemical equation are pretty much the stoichiometric coefficients, which means that the coefficients really represent the ratio between the substances in a reaction, so it is not necessarily always the exact molar amount. Expanding to your hydrogen gas example, for the equation...

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