Search found 64 matches
- Sat Mar 17, 2018 8:57 pm
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: Water and Cell Diagrams
- Replies: 3
- Views: 721
Water and Cell Diagrams
Would you ever include H2O in a cell diagram if it were part of a half reaction? For example, how would you write this reduction half reaction in a cell diagram: NO3- + 2H + e - ==> NO2 + H2O?
- Sat Mar 17, 2018 8:37 pm
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: Inert Electrodes
- Replies: 1
- Views: 355
Inert Electrodes
When do you need an inert electrode? If you have an inert electrode, do you put it on both sides of a cell diagram or just one?
- Fri Mar 16, 2018 11:35 am
- Forum: Third Law of Thermodynamics (For a Unique Ground State (W=1): S -> 0 as T -> 0) and Calculations Using Boltzmann Equation for Entropy
- Topic: Homework Problem 9.25
- Replies: 1
- Views: 486
Homework Problem 9.25
"If SO2F2 adopts a positionally disordered arrangement in its crystal form, what might its residual molar entropy be?" I understand how to do the math for this, but whenever I input the numbers in my calculator: 1.38 x 10^-23 ln(6^6.02 x 10^23), I get an "overflow error". Is this...
- Mon Mar 12, 2018 12:21 am
- Forum: Reaction Mechanisms, Reaction Profiles
- Topic: Collision Theory
- Replies: 3
- Views: 496
Re: Collision Theory
The higher the speed, the more likely particles are to collide and break/form bonds. Activation energy is the energy required to break/form bonds, so the higher the activation energy, the more difficult it will be to break/form bonds because the reaction requires a large input of energy before the p...
- Mon Mar 12, 2018 12:20 am
- Forum: Zero Order Reactions
- Topic: Half life
- Replies: 7
- Views: 1201
Re: Half life
Yes, just plug your given values into the equations and solve!
- Mon Mar 12, 2018 12:19 am
- Forum: Kinetics vs. Thermodynamics Controlling a Reaction
- Topic: Equilibrium constant
- Replies: 3
- Views: 671
Re: Equilibrium constant
K = k/k' where k' is the rate constant for a reaction's reverse form.
- Wed Mar 07, 2018 2:48 am
- Forum: First Order Reactions
- Topic: Pseudo First Order Reactions
- Replies: 2
- Views: 418
Pseudo First Order Reactions
How do we know if something is a pseudo-first-order reaction? Or would that be specified?
- Wed Feb 28, 2018 12:57 am
- Forum: Method of Initial Rates (To Determine n and k)
- Topic: Homework Problem 15.99
- Replies: 1
- Views: 316
Homework Problem 15.99
"15.99 Which of the following plots will be linear? (a) [A] against time for a reaction that is first order in A; (b) [A] against time for a reaction that is zero order in A; (c) ln[A] against time for a reaction that is first order in A; (d) 1/[A] against time for a reaction that is second ord...
- Tue Feb 27, 2018 10:49 pm
- Forum: Kinetics vs. Thermodynamics Controlling a Reaction
- Topic: Homework for Test 3
- Replies: 2
- Views: 450
Homework for Test 3
What homework problems cover 15.1-15.6 for Test 3?
- Tue Feb 27, 2018 9:03 pm
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: Cell diagram order
- Replies: 4
- Views: 452
Re: Cell diagram order
I think that usually cell diagrams are written in the order of oxidation | reduction, although the solutions manual sometimes does have it in a different order. I would stick with oxidation | reduction because that's what we've mostly seen in lecture.
- Mon Feb 26, 2018 5:25 pm
- Forum: First Order Reactions
- Topic: Equation in the Book vs. in Lecture
- Replies: 2
- Views: 427
Equation in the Book vs. in Lecture
The equation that the book gives for the integrated rate law of first-order reactions is [A] t = [A] 0 e -kt , but the equation for the integrated rate law of first-order reactions given in lecture is ln[A] = -kt + ln[A] 0 . Does it matter which equation we use since both are essentially the same? I...
- Tue Feb 20, 2018 11:30 pm
- Forum: Work, Gibbs Free Energy, Cell (Redox) Potentials
- Topic: Homework Problem 14.55b [ENDORSED]
- Replies: 2
- Views: 1883
Homework Problem 14.55b [ENDORSED]
"A 1.0 m NiSO4(aq) solution was electrolyzed by using inert electrodes. Write (a) the cathode reaction; (b) the anode reaction. (c) With no overpotential or passivity at the electrodes, what is the minimum potential that must be supplied to the cell for the onset of electrolysis?" The solu...
- Tue Feb 20, 2018 9:47 pm
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: Cell Diagrams [ENDORSED]
- Replies: 2
- Views: 396
Cell Diagrams [ENDORSED]
Does it matter what order the items in the anode side and cathode side of a cell diagram are written? For example, if you have Cl2 (g) and HCl (aq) on the anode side, would it make a difference if you wrote Cl2 (g) | HCl (aq) or if you wrote HCl (aq) | Cl2 (g) for the anode?
- Tue Feb 20, 2018 9:09 pm
- Forum: Appications of the Nernst Equation (e.g., Concentration Cells, Non-Standard Cell Potentials, Calculating Equilibrium Constants and pH)
- Topic: Expression for Q (Homework 14.37)
- Replies: 1
- Views: 348
Expression for Q (Homework 14.37)
I'm a little confused about how to calculate Q. I thought that the expression for Q was [product A]^a/[reactant B]^b using either the concentrations of the reactant and product or the partial pressures of the reactant and product. However, when doing 14.37a and c, the solutions manual combines the c...
- Wed Feb 14, 2018 12:15 am
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: delta H for Isothermal Reversible Expansion [ENDORSED]
- Replies: 1
- Views: 341
delta H for Isothermal Reversible Expansion [ENDORSED]
Is it possible to find delta H for an isothermal reversible expansion?
- Tue Feb 13, 2018 8:33 pm
- Forum: Concepts & Calculations Using First Law of Thermodynamics
- Topic: delta U for Isothermal Expansion of Ideal Gas
- Replies: 2
- Views: 677
Re: delta U for Isothermal Expansion of Ideal Gas
The equation for an ideal gas is U=3/2*nRT. When you're calculating the change in internal energy, the number of moles and the gas constant are constant values and that means the change in internal energy is dependent upon temperature change. But in an isothermal expansion temperature doesn't chang...
- Tue Feb 13, 2018 8:29 pm
- Forum: Gibbs Free Energy Concepts and Calculations
- Topic: delta G for Phase Changes
- Replies: 1
- Views: 437
delta G for Phase Changes
Does delta G = 0 for phase changes at the proper melting/boiling points? For example, homework problem 9.91b says that the standard Gibbs free energy for the vaporization of water at 100°C is 0. Why is this? Does this apply for the fusion/vaporization of other substances at their melting/boiling poi...
- Tue Feb 13, 2018 7:43 pm
- Forum: Gibbs Free Energy Concepts and Calculations
- Topic: Homework Problem 9.81
- Replies: 1
- Views: 380
Homework Problem 9.81
"Which is the thermodynamically more stable iron oxide in air, Fe3O4(s) or Fe2O3(s)? Justify your selection." The solutions manual says to look at the reaction converting Fe3O4 to Fe2O3, calculate the delta G for that, and then based on the delta G/spontaneity of the reaction, you'll know ...
- Tue Feb 13, 2018 6:43 pm
- Forum: Concepts & Calculations Using First Law of Thermodynamics
- Topic: delta U for Isothermal Expansion of Ideal Gas
- Replies: 2
- Views: 677
delta U for Isothermal Expansion of Ideal Gas
Why does delta U = 0 for the isothermal expansion of an ideal gas?
- Tue Feb 13, 2018 2:31 pm
- Forum: Thermodynamic Definitions (isochoric/isometric, isothermal, isobaric)
- Topic: isothermal system [ENDORSED]
- Replies: 3
- Views: 562
Re: isothermal system [ENDORSED]
There is no temperature change because energy from heat transfer is equal to energy from work. If they weren't equal, then the energy change from the heat transfer would result in a temperature change. However, because they are equal, the energy supplied by work makes up for that would-be temperatur...
- Tue Feb 13, 2018 2:29 pm
- Forum: Gibbs Free Energy Concepts and Calculations
- Topic: Delta G Units
- Replies: 1
- Views: 361
Re: Delta G Units
The rule that I usually follow is to use kJ for standard delta G of a whole reaction because the products aren't necessarily only present in 1 mole. Therefore, you can't say that standard delta G of a reaction is necessarily going to be kJ/mole; all that "standard delta G" implies is that ...
- Thu Feb 08, 2018 2:42 pm
- Forum: Concepts & Calculations Using Second Law of Thermodynamics
- Topic: Self-Test 9.7A
- Replies: 2
- Views: 600
Re: Self-Test 9.7A
Trouton's law says that the standard entropy of vaporization are commonly 85 J/(K*mol). It talks about entropy, not enthalpy. The question, on the other hand, asks you to solve for the enthalpy of vaporization of bromine liquid. The question asks you to apply the assumption that the entropy of vapo...
- Tue Feb 06, 2018 2:52 pm
- Forum: Calculating Standard Reaction Entropies (e.g. , Using Standard Molar Entropies)
- Topic: Example 9.10
- Replies: 1
- Views: 293
Example 9.10
Example 9.10 says, "Calculate the change in entropy of the surroundings when mercury freezes at 49 C; use Hfus(Hg) 2.292 kJ mol 1 at 49 C." It then goes on to solve the problem and sets T as (-49 + 273) K = 224 K. Are you just supposed to assume that the initial temperature is 0 C aka 273 ...
- Tue Feb 06, 2018 1:39 pm
- Forum: Concepts & Calculations Using Second Law of Thermodynamics
- Topic: Self-Test 9.7A
- Replies: 2
- Views: 600
Self-Test 9.7A
I'm a little confused about how to apply Trouton's Law. For example, self-test 9.7A says "Use Trouton’s rule to estimate the standard enthalpy of vaporization of liquid bromine, which boils at 59 C." I thought that Trouton's Law said that most liquids have a standard enthalpy of vaporizati...
- Mon Feb 05, 2018 9:58 am
- Forum: Calculating Work of Expansion
- Topic: Solving Reversible vs irreversible [ENDORSED]
- Replies: 2
- Views: 362
Re: Solving Reversible vs irreversible [ENDORSED]
I think the problems would say if they involve reversible or irreversible expansions.
- Mon Feb 05, 2018 9:57 am
- Forum: Calculating Work of Expansion
- Topic: Naming Question [ENDORSED]
- Replies: 5
- Views: 745
Re: Naming Question [ENDORSED]
Reversible expansion is expansion that occurs as a result of infinitesimally small steps that can push the expansion either forward or backwards with the smallest of changes. This results in a maximum of work being done. In contrast, irreversible expansion is expansion that occurs as result of finit...
- Mon Feb 05, 2018 9:53 am
- Forum: Entropy Changes Due to Changes in Volume and Temperature
- Topic: Entropy question [ENDORSED]
- Replies: 2
- Views: 381
Re: Entropy question [ENDORSED]
If the universe is constantly expanding, then entropy is also increasing with it.
- Mon Feb 05, 2018 9:51 am
- Forum: Gibbs Free Energy Concepts and Calculations
- Topic: Delta G equal Zero [ENDORSED]
- Replies: 4
- Views: 662
Re: Delta G equal Zero [ENDORSED]
Not necessarily, but delta G = 0 does mean that the reaction is at equilibrium.
- Mon Feb 05, 2018 9:50 am
- Forum: Concepts & Calculations Using First Law of Thermodynamics
- Topic: test question 7 [ENDORSED]
- Replies: 6
- Views: 756
Re: test question 7 [ENDORSED]
delta H (fusion) of ice would have been given
- Mon Feb 05, 2018 9:49 am
- Forum: Concepts & Calculations Using Second Law of Thermodynamics
- Topic: Types of Disorders [ENDORSED]
- Replies: 5
- Views: 692
Re: Types of Disorders [ENDORSED]
I think that positional disorder has to do with how much space particles have to move around in. The greater the space, the greater the positional entropy because the more particles can move around. Thermal disorder has to do with temperature, so the higher the temperature, the greater the particle ...
- Tue Jan 30, 2018 8:35 pm
- Forum: Concepts & Calculations Using First Law of Thermodynamics
- Topic: isothermal
- Replies: 5
- Views: 576
Re: isothermal
If an equation is isothermal, that means there is no heat transfer and therefore no change in temperature.
- Tue Jan 30, 2018 8:34 pm
- Forum: Concepts & Calculations Using Second Law of Thermodynamics
- Topic: unit of entropy
- Replies: 11
- Views: 1152
Re: unit of entropy
The units are J/K (Joules per Kelvin)!
- Tue Jan 30, 2018 8:34 pm
- Forum: Concepts & Calculations Using Second Law of Thermodynamics
- Topic: 9.27 D
- Replies: 3
- Views: 423
Re: 9.27 D
It might also be easier to think about this in terms of PV = PV. Pressure and volume are inversely related. Therefore, the bigger the pressure (in this case, 2 atm instead of 1 atm), the smaller the volume (the volume for 2 atm would be half that at 1 atm).
- Tue Jan 30, 2018 8:32 pm
- Forum: Phase Changes & Related Calculations
- Topic: Hw #8.49 standard state
- Replies: 4
- Views: 581
Re: Hw #8.49 standard state
My TA once said to assume that you're under standard conditions (298K and 1 atm) if the textbook doesn't say what temperature/pressure you're at, so I think you'd just assume that you're at standard state.
- Tue Jan 30, 2018 8:31 pm
- Forum: Heat Capacities, Calorimeters & Calorimetry Calculations
- Topic: heat capacities
- Replies: 5
- Views: 710
Re: heat capacities
The heat capacities for ice and water are different. Therefore, you would use the heat capacity of ice for ice and the heat capacity of water for water.
- Sun Jan 21, 2018 4:13 pm
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: ∆nRT in Reactions with no ∆n
- Replies: 2
- Views: 503
Re: ∆nRT in Reactions with no ∆n
If there is no change in the number of moles (no delta n), then that means that there is no change in volume (no delta V). Because w = -P(delta)V, if there is no delta V then there is no work done!
- Sun Jan 21, 2018 4:04 pm
- Forum: Concepts & Calculations Using First Law of Thermodynamics
- Topic: Homework Question 8.47
- Replies: 4
- Views: 334
Re: Homework Question 8.47
But that ultimately give you a negative work, whereas work done ON a system should be positive??? I just realized my mistake. Work done ON a system is positive, but EXPANSION work means that work is done on the surroundings/BY the system because the system is expanding. Therefore, work would be neg...
- Thu Jan 18, 2018 4:42 pm
- Forum: Concepts & Calculations Using First Law of Thermodynamics
- Topic: Homework Question 8.47
- Replies: 4
- Views: 334
Homework Question 8.47
For 8.47, why does the solutions manual use the equation (delta)H = U + P(delta)V instead of just U = q+ w? I'm also confused as to why work would be positive instead of negative because I thought that expansion work done ON a system is negative.
- Mon Jan 15, 2018 5:01 pm
- Forum: Concepts & Calculations Using First Law of Thermodynamics
- Topic: U = q + w assumptions
- Replies: 5
- Views: 703
U = q + w assumptions
Does the equation (change in)U = q + w assume that there is constant pressure? Or does the pressure not have to be constant?
- Sat Jan 13, 2018 4:22 pm
- Forum: Thermodynamic Definitions (isochoric/isometric, isothermal, isobaric)
- Topic: Irreversible vs. Reversible Processes
- Replies: 3
- Views: 382
Irreversible vs. Reversible Processes
Is the only difference between reversible and irreversible processes the fact that reversible processes are isothermal?
- Sat Jan 13, 2018 4:17 pm
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: Enthalpy of physical change?
- Replies: 3
- Views: 1068
Re: Enthalpy of physical change?
I'm not entirely sure, but I think that the 44.0 kJ/mol is just a value that was experimentally determined. I think that we would be given that in a table of H values or something if we needed it on a test (don't quote me on this though). The values given -- Hvap 40.7 kJ/mol at 100 degrees Celsius a...
- Sat Jan 13, 2018 4:13 pm
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: Standard Enthalpy of Formation from Most Stable Form
- Replies: 3
- Views: 1304
Standard Enthalpy of Formation from Most Stable Form
I know that the standard enthalpy of formation of an element in its most stable form is zero, but does that mean that the element begins in an unstable form and goes to its stable form, ex: N2 (l) ==> N2 (g)? Or would the element begin in its most stable form and then stay in its most stable form, e...
- Wed Dec 06, 2017 3:00 am
- Forum: Acidity & Basicity Constants and The Conjugate Seesaw
- Topic: Ka and Concentration
- Replies: 3
- Views: 1613
Ka and Concentration
Is Ka the same thing as [H3O+]?
- Mon Dec 04, 2017 11:10 am
- Forum: Properties & Structures of Inorganic & Organic Acids
- Topic: Using The Equilibrium Arrow
- Replies: 5
- Views: 3231
Re: Using The Equilibrium Arrow
You use the equilibrium arrow for weak acids and bases because they don't fully dissociate. Strong acids and bases completely dissociate, so you would use a regular arrow for equations with strong acids/bases.
- Mon Dec 04, 2017 11:08 am
- Forum: Significant Figures
- Topic: Significant Figures [ENDORSED]
- Replies: 3
- Views: 592
Re: Significant Figures [ENDORSED]
I'm not sure if you would get full credit, but try to round as little as possible in the course of solving the problem until you get to the very end so that your answer is as correct as possible.
- Thu Nov 30, 2017 12:22 am
- Forum: Naming
- Topic: aqua = (OH2) or (H20)
- Replies: 2
- Views: 598
Re: aqua = (OH2) or (H20)
OH2 is written with the O first because the O is the atom with which bonds are formed.
- Thu Nov 30, 2017 12:22 am
- Forum: Non-Equilibrium Conditions & The Reaction Quotient
- Topic: Quotient
- Replies: 12
- Views: 860
Re: Quotient
Q is the reaction quotient, while K is the equilibrium quotient. They both follow the same expression -- the product of the concentrations or partial pressures of each product raised to the power of its stoichiometric coefficient over the product of the concentrations or partial pressures of each re...
- Sat Nov 25, 2017 8:22 pm
- Forum: Ideal Gases
- Topic: Units of Partial Pressure
- Replies: 7
- Views: 952
Re: Units of Partial Pressure
Partial pressure units should usually be atm. However, sometimes other units may be used, so be careful to convert then!
- Sat Nov 25, 2017 8:21 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Polarity of NH3?
- Replies: 4
- Views: 25259
Re: Polarity of NH3?
NH3 is polar because it has 3 dipoles that do not cancel out. Each N-H bond is polar because N is more electronegative than H. NH3 is overall asymmetrical in its VSEPR shape, so the dipoles don't cancel out and it is therefore polar.
- Wed Nov 15, 2017 12:46 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Regions of electron density
- Replies: 4
- Views: 492
Re: Regions of electron density
Yes, it does!
- Wed Nov 15, 2017 12:45 pm
- Forum: Hybridization
- Topic: Notation
- Replies: 6
- Views: 749
Re: Notation
Px, Py, and Pz are simply the three orbitals in the P subshell (the three horizontal lines we draw). You don't necessarily need to write them out; usually we would just write P2, P3, etc. P(however many electrons are in the P subshell).
- Wed Nov 08, 2017 3:35 pm
- Forum: Bohr Frequency Condition, H-Atom , Atomic Spectroscopy
- Topic: Principal Energy Level Change Sig Figs
- Replies: 2
- Views: 476
Principal Energy Level Change Sig Figs
When you're calculating the frequency emitted from a jump in principal energy levels (i.e. n=1 to n=3), how would you determine the significant figures needed for the answer?
- Wed Nov 08, 2017 8:51 am
- Forum: Lewis Structures
- Topic: Organic Molecules [ENDORSED]
- Replies: 1
- Views: 338
Organic Molecules [ENDORSED]
Would we be expected to know how to draw the Lewis structure for a lot of organic molecules on the midterm? Or would we mainly be drawing Lewis structures for inorganic compounds?
- Fri Nov 03, 2017 11:16 am
- Forum: Ionic & Covalent Bonds
- Topic: Covalent/ Ionic Bond
- Replies: 5
- Views: 827
Re: Covalent/ Ionic Bond
A metal and a non-metal will typically form an ionic bond, whereas non-metals bonding together will typically form a covalent bond!
- Tue Oct 31, 2017 2:04 pm
- Forum: Wave Functions and s-, p-, d-, f- Orbitals
- Topic: Homework Problem 2.55
- Replies: 5
- Views: 717
Homework Problem 2.55
When the textbook refers to "Group 5 Transition Metals", does that mean Group 5 where Group 1 is the alkali metals? Or does it mean Group 5 where Group 1 is the first column of transition metals (Sc, Y, etc.)?
- Mon Oct 23, 2017 5:47 pm
- Forum: Student Social/Study Group
- Topic: Post All Chemistry Jokes Here
- Replies: 9651
- Views: 2763451
Re: Post All Chemistry Jokes Here
Did you know that you can cool yourself to -273.15˚C and still be 0k?
- Mon Oct 23, 2017 5:41 pm
- Forum: Properties of Electrons
- Topic: Rydberg Equation [ENDORSED]
- Replies: 6
- Views: 1022
Re: Rydberg Equation [ENDORSED]
If the electron is going from n=4 to n=2, then n=2 would be the final energy state and n=4 would be the initial energy state.
- Tue Oct 17, 2017 9:33 pm
- Forum: DeBroglie Equation
- Topic: Particle-Specific/Light-Specific Equations
- Replies: 1
- Views: 380
Particle-Specific/Light-Specific Equations
In class, Professor Lavelle mentioned that the De Broglie equation can only be used for particles with rest mass, like electrons, and therefore can't be used for light. Are there any other equations that can only be used for particles with rest mass or that can only be used for light?
- Mon Oct 16, 2017 9:32 pm
- Forum: Properties of Light
- Topic: Problem 1.23
- Replies: 3
- Views: 498
Re: Problem 1.23
Thompson W 3B wrote:I believe the conversion is given on a sheet of constants and equations, which is attached to the tests. Here is the sheet: https://lavelle.chem.ucla.edu/wp-conten ... ations.pdf
Thank you so much! I didn't see that earlier.
- Mon Oct 16, 2017 8:09 pm
- Forum: Properties of Light
- Topic: Problem 1.23
- Replies: 3
- Views: 498
Problem 1.23
Problem 1.23 gives the energy of gamma ray photons in kiloelectronvolts. Do we have to know the conversion between KeV and joules or do you guys think that energy will be given to us in J?
- Sun Oct 15, 2017 9:58 pm
- Forum: Properties of Light
- Topic: Speed of Light Constant
- Replies: 18
- Views: 1675
Re: Speed of Light Constant
2.998 x 10^8 m/s is more accurate, but Professor Lavelle uses 3.00 x 10^8 in his lecture slides and example problems, so I don't think using 3.00 x 10^8 would be an issue.
- Tue Oct 10, 2017 11:53 pm
- Forum: DeBroglie Equation
- Topic: Post-Module Assessment Q. 34
- Replies: 4
- Views: 449
Re: Post-Module Assessment Q. 34
I think your answer is like correct, meaning approx. close to the answers given b/c when you round the answer you got and change it to scientific notation, you should get 1.00 * 10^5 m/s and since it's way less than speed of light, which if the fastest speed known so far, answer should be reasonabl...
- Sat Oct 07, 2017 10:01 pm
- Forum: Balancing Chemical Reactions
- Topic: Determining order of elements to work with when balancing equations [ENDORSED]
- Replies: 2
- Views: 499
Re: Determining order of elements to work with when balancing equations [ENDORSED]
No, but sometimes starting with the least-occurring element when balancing a chemical reaction gives you an easier starting place for balancing a reaction.
- Sat Oct 07, 2017 9:51 pm
- Forum: SI Units, Unit Conversions
- Topic: Significant Figures in relation to molar mass [ENDORSED]
- Replies: 4
- Views: 11454
Re: Significant Figures in relation to molar mass [ENDORSED]
Keep the molar mass as precise as possible while calculating. You should try to round as little as possible until you reach your final answer! Then you should be fine.