Search found 67 matches
- Sun Mar 17, 2019 10:16 pm
- Forum: Experimental Details
- Topic: Psuedo First Order
- Replies: 7
- Views: 1482
Re: Psuedo First Order
A pseudo first order reaction is like a second order reaction that acts like a first order reaction under certain conditions.
- Sun Mar 17, 2019 1:01 am
- Forum: Concepts & Calculations Using First Law of Thermodynamics
- Topic: adiabatic vs isothermal
- Replies: 2
- Views: 493
Re: adiabatic vs isothermal
In an adiabatic reaction q =0 while in an isothermal reaction, delta T = 0.
- Sat Mar 16, 2019 10:40 pm
- Forum: Phase Changes & Related Calculations
- Topic: Enthalpy
- Replies: 1
- Views: 392
Re: Enthalpy
It depends on whether C is given in per moles or per grams (molar heat capacity or specific heat capacity).
- Sat Mar 16, 2019 10:39 pm
- Forum: Gibbs Free Energy Concepts and Calculations
- Topic: ∆G and work
- Replies: 3
- Views: 898
Re: ∆G and work
I believe that delta G is the measure of the maximum amount of energy available for work.
- Sat Mar 16, 2019 10:37 pm
- Forum: Concepts & Calculations Using First Law of Thermodynamics
- Topic: q and delta H
- Replies: 6
- Views: 965
Re: q and delta H
I think q = delta H under constant pressure. I also think that delta H implies constant pressure already so they can be used interchangeably but I am not sure.
- Sat Mar 16, 2019 9:51 pm
- Forum: Concepts & Calculations Using Second Law of Thermodynamics
- Topic: Free Expansion
- Replies: 3
- Views: 674
Re: Free Expansion
When a system expands, it is doing work on the surroundings which means it would be losing energy. Therefore, work is negative. If the surroundings were to do work on the system, then work would be positive because the system is gaining energy.
- Sat Mar 16, 2019 9:49 pm
- Forum: Arrhenius Equation, Activation Energies, Catalysts
- Topic: Catalysts
- Replies: 2
- Views: 519
Re: Catalysts
To expand on the above, a homogeneous catalyst is a catalyst of the same phase as the reactants while a heterogeneous catalyst is one that is of a different phase than the reactants.
- Sun Mar 10, 2019 9:43 pm
- Forum: Zero Order Reactions
- Topic: Meaning of Zero, First, and Second Order?
- Replies: 4
- Views: 637
Re: Meaning of Zero, First, and Second Order?
Remember you can also relate order numbers to individual reactants themselves or also the overall reaction order.
- Sun Mar 10, 2019 9:41 pm
- Forum: Arrhenius Equation, Activation Energies, Catalysts
- Topic: What does the Arrhenius Equation tell us?
- Replies: 1
- Views: 228
Re: What does the Arrhenius Equation tell us?
If you look at the Arrhenius equation, you will see that increasing temperature increases the number to which e is taken to the power of (T is in the denominator and the number is negative so the number becomes a smaller negative). This increases the value of K. If activation energy decreases, then ...
- Sun Mar 10, 2019 9:28 pm
- Forum: Administrative Questions and Class Announcements
- Topic: Morris Review
- Replies: 4
- Views: 788
Re: Morris Review
He said he would post the slides online but if you still want notes I can send them!
- Sun Mar 03, 2019 11:47 am
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: liquid and gaseous states in a cell diagram
- Replies: 3
- Views: 416
Re: liquid and gaseous states in a cell diagram
To continue the answers above, remember to use a single line when referencing a porous disc versus the double line used for a salt bridge.
- Sun Mar 03, 2019 11:29 am
- Forum: General Rate Laws
- Topic: Kinetics
- Replies: 3
- Views: 373
Re: Kinetics
When you are looking at a chemical reaction, the rate at which each reactant and product is changing might be different from one another. A unique rate would be the rate of change for any species in a chemical reaction divided by its stoichiometric coefficient. Unique rates should be the same for ea...
- Sun Mar 03, 2019 11:22 am
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: H+ and OH
- Replies: 3
- Views: 434
Re: H+ and OH
Sometimes in the homework, the solutions would include KOH instead of OH. Is there a reason for this and should we include salts in our cell diagrams too?
- Sun Feb 24, 2019 9:24 pm
- Forum: Balancing Redox Reactions
- Topic: Salt bridge
- Replies: 1
- Views: 216
Re: Salt bridge
In the cell, electrons move from the anode to the cathode which would make the cathode extremely negatively charged. If left like this, electrons would not travel toward the cathode any longer due to the buildup of a negative charge there. The salt bridge helps maintain a neutral state for both solu...
- Sun Feb 24, 2019 9:18 pm
- Forum: Work, Gibbs Free Energy, Cell (Redox) Potentials
- Topic: Spontaneous?
- Replies: 13
- Views: 1588
Re: Spontaneous?
I think the only way to be sure of spontaneity is when ΔG is negative (when ΔH −TΔS is negative) though I could be wrong.
- Sun Feb 24, 2019 9:15 pm
- Forum: Work, Gibbs Free Energy, Cell (Redox) Potentials
- Topic: Spontaneous Process
- Replies: 2
- Views: 274
Re: Spontaneous Process
A process is spontaneous when ΔG is negative (when ΔH < TΔS).
- Sun Feb 17, 2019 7:44 pm
- Forum: Entropy Changes Due to Changes in Volume and Temperature
- Topic: Calculating entropy
- Replies: 5
- Views: 438
Re: Calculating entropy
When we calculate the two independently, we are essentially splitting it up into steps which is allowed since entropy is a state function. First we change the volume and then we change the temperature to reach the final form.
- Sun Feb 17, 2019 7:42 pm
- Forum: Gibbs Free Energy Concepts and Calculations
- Topic: Intensive vs extensive
- Replies: 4
- Views: 491
Re: Intensive vs extensive
I would assume that Gibbs free energy is an extensive property since the feasibility of a reaction depends on factors such as the amount of matter/availability of reactants, etc. Please correct me if I'm wrong!
- Fri Feb 15, 2019 8:19 pm
- Forum: Calculating Work of Expansion
- Topic: Work without change in volume
- Replies: 8
- Views: 1131
Re: Work without change in volume
If there is no change in volume, no work will be done. If you are referring to an isothermal process with constant pressure, then I'm pretty sure work = -(external P)(Delta V).
- Sun Feb 10, 2019 7:57 pm
- Forum: Heat Capacities, Calorimeters & Calorimetry Calculations
- Topic: Using R
- Replies: 10
- Views: 1027
Using R
How do I know which R to use and when? Thanks.
- Sun Feb 10, 2019 7:51 pm
- Forum: Concepts & Calculations Using First Law of Thermodynamics
- Topic: Effects of Constant Volume or Temp
- Replies: 1
- Views: 195
Re: Effects of Constant Volume or Temp
Constant volume means that no work is done and so delta U is equal to q. When temperature is constant, delta U is equal to 0.
- Sun Feb 10, 2019 7:49 pm
- Forum: Concepts & Calculations Using First Law of Thermodynamics
- Topic: U = (3/2)nRT
- Replies: 2
- Views: 727
U = (3/2)nRT
When do we use the equation U = 3/2 nRT? I saw this on the constants and equations sheet but I have no idea when to use it.
- Sun Feb 03, 2019 11:25 am
- Forum: Concepts & Calculations Using First Law of Thermodynamics
- Topic: kJ vs J
- Replies: 9
- Views: 832
Re: kJ vs J
Either should be fine as long as you are consistent in your calculations and make sure that everything matches up properly.
- Thu Jan 31, 2019 5:18 pm
- Forum: Heat Capacities, Calorimeters & Calorimetry Calculations
- Topic: Extensive vs. Intensive
- Replies: 5
- Views: 796
Re: Extensive vs. Intensive
I am not entirely sure about extrinsic versus intrinsic though I think they are similar. Intrinsic properties are ones that do not depend on outside factors / amount of substance such as boiling point/density whereas extrinsic properties depend on outside factors / amount of substance such as weight...
- Thu Jan 31, 2019 11:25 am
- Forum: Heat Capacities, Calorimeters & Calorimetry Calculations
- Topic: Heat Capacity
- Replies: 5
- Views: 540
Re: Heat Capacity
To build on, heat capacity is therefore an extensive property because heat capacity is the heat required to raise the temperature of an object by 1 degree celsius. The heat required to raise the temperature of an object depends on how much of the object there is or the amount of substance.
- Thu Jan 24, 2019 11:44 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Equilibrium Favoring
- Replies: 4
- Views: 790
Re: Equilibrium Favoring
I think that the question is asking what the reaction favors when it is at equilibrium (as opposed to when we use Q to see which direction the reaction will go when it is not at equilibrium). I do not remember the exact numbers but I believe in the first few lectures Dr. Lavelle talked about the rea...
- Thu Jan 24, 2019 11:37 pm
- Forum: Calculating pH or pOH for Strong & Weak Acids & Bases
- Topic: determining x for weak acids and bases
- Replies: 6
- Views: 787
Re: determining x for weak acids and bases
I think that you can ignore the x when you are adding it or subtracting it to some constant (e.g. 1.0-x) because the difference that x will make on the number is insignificant when x is that small. It is important to note that x does not equal zero though.
- Thu Jan 24, 2019 7:34 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: HW 6A.21
- Replies: 1
- Views: 223
Re: HW 6A.21
Because you know that the solution is neutral water (pH ~7), the hydronium and hydroxide concentrations must equal each other and balance each other out.
- Fri Jan 18, 2019 4:27 pm
- Forum: Applying Le Chatelier's Principle to Changes in Chemical & Physical Conditions
- Topic: Inert Gases
- Replies: 5
- Views: 627
Re: Inert Gases
Concentration is dependent on the number of moles and volume (n/v). Though adding inert gas does change the pressure, it changes neither of the number of moles nor the volume which means concentration stays the same! If you changed pressure by changing the volume, then concentration would change and...
- Fri Jan 18, 2019 4:10 pm
- Forum: Ideal Gases
- Topic: The Difference between Q and Kc [ENDORSED]
- Replies: 18
- Views: 8793
Re: The Difference between Q and Kc [ENDORSED]
As said above, Q has the same formula as Kc but can be calculated at anytime, not just when a reaction is at equilibrium. To explain the comparison a little more, when Q < Kc, a forward reaction will be favored. This is because Q is calculated as [products] / [reactants]. If Q is smaller than Kc, we...
- Fri Jan 18, 2019 3:59 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: When is X negligible.
- Replies: 6
- Views: 559
Re: When is X negligible.
As the others mentioned before, the general rule is that you can disregard the X when the K value is smaller than 10^-3. Afterward, you can also confirm that the X you get is less than 5% of the initial concentration in order to double check that your approximation is valid.
- Sat Jan 12, 2019 6:23 pm
- Forum: Ideal Gases
- Topic: K and Q
- Replies: 7
- Views: 513
Re: K and Q
They have the same formula but don't equal each other because K is calculated using molarities at equilibrium but Q is calculated using molarities at any point in time during the reaction. We can then use Q and compare it to K to see at where the reaction is at. If Q<K, then a forward reaction is fa...
- Sat Jan 12, 2019 6:19 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Kp and Kc
- Replies: 1
- Views: 142
Re: Kp and Kc
Kp is the equilibrium constant calculated using partial pressure (of gases). Kc is the equilibrium constant calculated using concentration of products and reactions at equilibrium. You can convert between partial pressure and concentration through PV = nRT. where P = (n/v)RT and n/v is concentration.
- Sat Jan 12, 2019 6:12 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Solving for K
- Replies: 7
- Views: 474
Re: Solving for K
We use brackets in our calculation for Kc because we are using the molarity/concentration which is denoted with brackets. I don't think its necessary to use brackets when solving for Kp because we are using partial pressure though I'm not sure.
- Sat Dec 08, 2018 8:57 pm
- Forum: Shape, Structure, Coordination Number, Ligands
- Topic: A X5 E
- Replies: 6
- Views: 689
Re: A X5 E
AX5E is square pyramidal!
- Sat Dec 08, 2018 8:54 pm
- Forum: Electron Configurations for Multi-Electron Atoms
- Topic: Diamagnetic vs. Paramagnetic
- Replies: 1
- Views: 462
Re: Diamagnetic vs. Paramagnetic
I find that drawing out the orbitals and filling in the electrons help. That way you can easily visualize whether there are unpaired electrons (paramagnetic) or no unpaired electrons (diamagnetic).
- Sat Dec 08, 2018 8:47 pm
- Forum: Naming
- Topic: bis-, tris-, etc.
- Replies: 4
- Views: 572
Re: bis-, tris-, etc.
You use bis-, tris-, and tetrakis- when the ligand name already has di-, tri-, tetra-, etc or if they are polydentate. For oxalate, you would use bis-, tris-, etc as it is bidentate.
- Sat Dec 08, 2018 8:38 pm
- Forum: *Molecular Orbital Theory (Bond Order, Diamagnetism, Paramagnetism)
- Topic: inter- and intra-
- Replies: 5
- Views: 1573
Re: inter- and intra-
The greater the difference in electronegativity between two atoms, the greater the ionic character of their bond. I think the number mentioned in class was that if the value of electronegativity is greater than 2, than the bond is considered generally ionic.
- Sat Dec 08, 2018 8:35 pm
- Forum: Shape, Structure, Coordination Number, Ligands
- Topic: determining the coordination compound
- Replies: 1
- Views: 240
Re: determining the coordination compound
If you are talking about the coordination number, the coordination number is the number of ligands bound to the central atom!
- Sat Dec 08, 2018 8:34 pm
- Forum: Shape, Structure, Coordination Number, Ligands
- Topic: Ligands
- Replies: 1
- Views: 239
Re: Ligands
Do you mean what it means for it to be cis? Cisplatin is a chemotherapy drug that forms a coordination compound with DNA, particularly guanine, to stop cell division.
- Sat Dec 01, 2018 3:01 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Polar Molecules
- Replies: 12
- Views: 937
Re: Polar Molecules
It would be best to, from the Lewis structure, figure out the shape of the molecule through VSEPR and use the electronegativity of each atom to determine the total dipole movement.
- Sat Dec 01, 2018 2:54 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Dissociation energy
- Replies: 7
- Views: 656
Re: Dissociation energy
When bonds are formed, energy is released (negative) as atoms move toward a more stable state. The opposite, the breaking of bonds, would therefore require an input of energy (positive) in order to pull atoms away from that stable state.
- Sat Dec 01, 2018 2:40 pm
- Forum: Lewis Acids & Bases
- Topic: Lewis and Bronsted
- Replies: 8
- Views: 834
Re: Lewis and Bronsted
The two are essentially the same but they relate the ions through different means. The Lewis definition relates two ions using the transfer of electrons. A Lewis acid is an electron acceptor while a Lewis base is the electron donor. The Bronsted definition relates the two through protons in which a ...
- Sat Nov 24, 2018 10:35 pm
- Forum: Sigma & Pi Bonds
- Topic: Sigma Bonds
- Replies: 2
- Views: 281
Re: Sigma Bonds
In a double bond, one will always be a sigma bond and one will always be a pi bond. In a triple bond, one will always be a sigma bond and two will be pi bonds. This is because, in order to form sigma bonds, the orbitals need to align end to end. Afterward, the lobes can only align in a parallel form...
- Sat Nov 24, 2018 9:05 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: Polarity and Boiling Point
- Replies: 3
- Views: 5258
Re: Polarity and Boiling Point
Molecules with higher polarity have greater dispersion forces and therefore stronger dipole-dipole interactions. This greater intermolecular attraction force leads to a higher boiling point. This explains why water (with all its hydrogen bonds) has a high boiling point.
- Sat Nov 24, 2018 8:35 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: molecular shape vs molecular geometry
- Replies: 3
- Views: 308
Re: molecular shape vs molecular geometry
Looking at VSEPR notations might help. For AX4, a molecule without lone pairs, both its molecular and electron geometry are tetrahedral. For AX3E, its molecular geometry would be trigonal pyramidal but its electron geometry is tetrahedral.
- Sun Nov 18, 2018 10:09 am
- Forum: Interionic and Intermolecular Forces (Ion-Ion, Ion-Dipole, Dipole-Dipole, Dipole-Induced Dipole, Dispersion/Induced Dipole-Induced Dipole/London Forces, Hydrogen Bonding)
- Topic: Energy of Intermolecular Forces
- Replies: 6
- Views: 939
Re: Energy of Intermolecular Forces
Breaking bonds generally requires an addition of energy. The opposite, forming bonds, is a release of energy which explains the negative number.
- Sun Nov 18, 2018 10:03 am
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Molecular shape vs electron geometry
- Replies: 4
- Views: 389
Re: Molecular shape vs electron geometry
An example would be AX3E. Its molecular geometry would be trigonal pyramidal but its electron geometry is tetrahedral. For those without lone pairs on the central atom such as AX4, both its molecular and electron geometry is tetrahedral.
- Sun Nov 18, 2018 9:50 am
- Forum: *Molecular Orbital Theory (Bond Order, Diamagnetism, Paramagnetism)
- Topic: Sigma and Pi Bonds
- Replies: 5
- Views: 706
Re: Sigma and Pi Bonds
A single bond will always be a sigma bond, a double bond will be a sigma bond and a pi bond, and a triple bond will be a sigma bond and two pi bonds. The first bond is able to overlap head-on which allows the bound atoms to rotate. However, the second and third bonds are forced to bond side by side ...
- Fri Nov 09, 2018 7:16 pm
- Forum: Electron Configurations for Multi-Electron Atoms
- Topic: Placement of the 3d orbital
- Replies: 1
- Views: 322
Re: Placement of the 3d orbital
The 4s orbital comes before the 3d orbital because the 4s shell actually has a lower energy level than the 3d orbital. However, if the 4s orbital is filled (2 electrons), then its energy level rises to higher than the 3d orbital which is why we write it after the 3d (exceptions: Chromium and Copper).
- Thu Nov 08, 2018 2:22 pm
- Forum: Polarisability of Anions, The Polarizing Power of Cations
- Topic: Electronegativity
- Replies: 6
- Views: 680
Re: Electronegativity
I think that oxygen is more electronegative. Oxygen is smaller than chlorine, with chlorine having a whole other shell of electrons which means that valence electrons in oxygen feel a stronger force.
- Thu Nov 08, 2018 1:01 pm
- Forum: Formal Charge and Oxidation Numbers
- Topic: Formal Charge & Stable lewis structures
- Replies: 6
- Views: 823
Re: Formal Charge & Stable lewis structures
To add on to the previous posts, it is also most desirable to have the lowest possible charge on the central atom for stability though this is not always possible.
- Sun Nov 04, 2018 12:48 am
- Forum: Octet Exceptions
- Topic: Lewis acids and bases
- Replies: 4
- Views: 329
Re: Lewis acids and bases
A lewis base simply donates an electron within a coordinate covalent bond and a lewis acid accepts an electron in a coordinate covalent bond!
- Sun Nov 04, 2018 12:43 am
- Forum: Trends in The Periodic Table
- Topic: Ionization Energy: Oxygen
- Replies: 1
- Views: 99
Re: Ionization Energy: Oxygen
This is because oxygen's 2p orbitals has 4 electrons (1 paired, 2 unpaired). Losing one electron from the pair would create a half filled stable orbital which is desired, hence the low ionization energy!
- Sun Nov 04, 2018 12:36 am
- Forum: Lewis Structures
- Topic: Drawing Lewis Structures
- Replies: 4
- Views: 375
Re: Drawing Lewis Structures
Unless the question asks you specifically to draw all the resonance structures, I think that one is okay.
- Sun Oct 28, 2018 11:10 am
- Forum: Ionic & Covalent Bonds
- Topic: Replacement for Modules
- Replies: 7
- Views: 672
Re: Replacement for Modules
In addition to the resources stated above, I also really enjoy going through worksheets from workshops, step-up sessions, etc. You can just look them up on chem community!
- Sun Oct 28, 2018 11:06 am
- Forum: Ionic & Covalent Bonds
- Topic: ionization energy [ENDORSED]
- Replies: 4
- Views: 237
Re: ionization energy [ENDORSED]
After the first electron is removed, the ratio of protons to electrons increases and therefore the pull on the remaining electrons increases. This raises the ionization energy.
- Sun Oct 28, 2018 11:04 am
- Forum: DeBroglie Equation
- Topic: Kg vs Grams
- Replies: 6
- Views: 687
Re: Kg vs Grams
I think something that would help would be to write out the units for all parts of the equation. In h/mv, h is given in kg.m^2.s^-1. In order to cancel out the kg, the mass "m" needs to be in kilograms as well. The velocity should cancel out m.s^-1 and leave meters for λ.
- Sun Oct 21, 2018 9:07 am
- Forum: DeBroglie Equation
- Topic: de broglie post module q 35 [ENDORSED]
- Replies: 2
- Views: 236
Re: de broglie post module q 35 [ENDORSED]
You would just solve this as you normally do. λ = h/p = h/mv h = 6.626 x 10^-34 m = 275 kg v = 34.72 m/s λ = (6.626 x 10^-34)/(275*34.72) = 6.94 x 10^-38 m A car does not have wavelike properties as only very small objects have measurable wavelike properties. As objects become larger, wavelike prope...
- Sun Oct 21, 2018 8:37 am
- Forum: Properties of Light
- Topic: Test 2
- Replies: 7
- Views: 623
Re: Test 2
I would focus on the topics explored in the last four video modules and all the information given up until Friday's lecture.
- Sun Oct 21, 2018 8:35 am
- Forum: Photoelectric Effect
- Topic: spectral lines
- Replies: 6
- Views: 635
Re: spectral lines
Both work since wavelength is the inverse of frequency. It just depends on what you are trying to solve for in the problem! I think that something of this topic will most likely appear on the exam.
- Sat Oct 13, 2018 11:02 pm
- Forum: Balancing Chemical Reactions
- Topic: Test 1 and Future Tests
- Replies: 5
- Views: 787
Re: Test 1 and Future Tests
Maybe you could try balancing in steps one element at a time just in case a mistake is made so you can receive partial credit.
- Sat Oct 13, 2018 10:02 pm
- Forum: Significant Figures
- Topic: sig fig calculations
- Replies: 3
- Views: 659
Re: sig fig calculations
For addition and subtraction, you use the least number of decimal points from the given values and for multiplication, you use the least number of sig figs from the given values.
- Sat Oct 13, 2018 9:56 pm
- Forum: Administrative Questions and Class Announcements
- Topic: Writing in Pen
- Replies: 13
- Views: 1037
Re: Writing in Pen
If you really dislike writing in pen, I would just ask your TA whether he/she cares! My TA said she did not mind whether we use pen or not.
- Fri Oct 05, 2018 11:46 am
- Forum: Molarity, Solutions, Dilutions
- Topic: Water Added to Solution Placed in a New Flask
- Replies: 3
- Views: 615
Re: Water Added to Solution Placed in a New Flask
I think here we need to use the M1V1 = M2V2 formula. I would first find the molarity of the original solution by converting 5.00 grams of KMnO4 into moles for the moles of solute and then divide it by the volume of the solution. (0.0316 mol/0.1500 L = 0.211 mol/L) Now you have the initial molarity (...
- Fri Oct 05, 2018 8:56 am
- Forum: Limiting Reactant Calculations
- Topic: Excess Reactant Calculation
- Replies: 2
- Views: 303
Re: Excess Reactant Calculation
After identifying the limiting reactant, determine how much of the other reactant is used up by converting the grams of the limiting reactant to moles and, using the stoichiometric coefficients for the ratio, determining how many moles of the other reactant is used up. Convert that number to grams a...
- Fri Oct 05, 2018 8:16 am
- Forum: Empirical & Molecular Formulas
- Topic: Post-Module Assessment Q22
- Replies: 3
- Views: 336
Re: Post-Module Assessment Q22
After finding the empirical formula (C5H12O5), calculate its molar mass which should be about 152.15 g/mol. The question should give the molar mass of the compound. Divide that number by the 152.15 g/mol you just calculated to find the ratio between the molecular and empirical formula. Use that rati...