Search found 29 matches
- Fri Mar 15, 2019 11:30 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Ka Kb = Kw
- Replies: 5
- Views: 903
Re: Ka Kb = Kw
The Ka/Kb can also help you find the concentrations of H+ of OH- ions depending on whether the reaction is acidic or basic, which can then help you find pH.
- Fri Mar 15, 2019 11:21 pm
- Forum: Arrhenius Equation, Activation Energies, Catalysts
- Topic: 15.69 6th Edition
- Replies: 3
- Views: 327
Re: 15.69 6th Edition
Essentially, the question is telling you that there's a k before the catalyst was added, let's call it k1, and a k after, k2. 1000k1=k2. From here, you can plug in the Arrhenius equation and the givens in order to find the original activation energy. There's a confusing part where you have to take e...
- Fri Mar 08, 2019 2:05 pm
- Forum: Method of Initial Rates (To Determine n and k)
- Topic: Units of k
- Replies: 4
- Views: 490
Re: Units of k
K's unit changes depending on the order of the reaction because the reaction rate will always have to be some variation of M/s, and k compensates for the extra M's that gets added to the number when the reaction goes up in order.
- Fri Mar 08, 2019 2:02 pm
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: Water in a cell diagram
- Replies: 5
- Views: 587
Re: Water in a cell diagram
I think you do include water if it's not in liquid phase and if the H or O is one of the things being oxidized/reduced (this is rare but can happen), although I'm not really sure.
- Fri Mar 08, 2019 1:58 pm
- Forum: General Rate Laws
- Topic: 15.1
- Replies: 3
- Views: 360
Re: 15.1
They're basically asking you to give the ratio of N2 to H2, NH3 to H2, and NH3 to N2
- Fri Mar 01, 2019 6:21 pm
- Forum: Balancing Redox Reactions
- Topic: Half Reactions in a Basic Solution
- Replies: 4
- Views: 425
Re: Half Reactions in a Basic Solution
First, balance everything but Hydrogen and electrons. Then write down how many Hydrogens you need to balance the equation on the side that needs the Hydrogens. Then replace the Hydrogens with H2O molecules and add the same number of OH- molecules to the opposite side of the equation. In effect, this...
- Fri Mar 01, 2019 6:17 pm
- Forum: Balancing Redox Reactions
- Topic: Oxidation State
- Replies: 4
- Views: 569
Re: Oxidation State
An fast way to quickly identify what elements in a reaction could be being oxidized is to pinpoint anything that is not oxygen or hydrogen, since it is really rare for these two to have their oxidation numbers change. This usually leaves only two elements you have to calculate the oxidation numbers ...
- Fri Mar 01, 2019 6:07 pm
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: Cell Diagrams (Using Platinum)
- Replies: 10
- Views: 1001
Re: Cell Diagrams (Using Platinum)
We use platinum in a cell diagram when either the cathode or the anode lacks a solid that can be used to conduct electrons from one side of the beaker to the other. This is because platinum is inert and will not react with anything else in the reaction.
- Thu Feb 21, 2019 5:25 pm
- Forum: Balancing Redox Reactions
- Topic: Oxidation States
- Replies: 10
- Views: 1010
Re: Oxidation States
The best way to find the oxidation state of a transition metal is to use the oxidation states of the other molecules in the compound witht he transition metal.
- Thu Feb 21, 2019 5:13 pm
- Forum: Balancing Redox Reactions
- Topic: Oxidation States
- Replies: 2
- Views: 258
Re: Oxidation States
There are a few rules that I memorized when assigning oxidation numbers, but they're fairly complicated 1.) Group 1 elements are always +1, Group 2 elements are always +2 2.) The oxidation numbers have to equal the total charge of the ion or molecule 3.) Hydrogen is +1 unless it is bonded to a metal...
- Thu Feb 21, 2019 5:08 pm
- Forum: Balancing Redox Reactions
- Topic: problem 14.1 6th edition
- Replies: 1
- Views: 193
Re: problem 14.1 6th edition
What I tried doing is to have H+ ions in the oxidation equation too. When I tried this I got C2H5OH ---> 6e- +C2H4O + 2H+
The problem with this is that even though the atoms add up, it doesn't balance the charges out in the equations, and I can't figure that part out.
The problem with this is that even though the atoms add up, it doesn't balance the charges out in the equations, and I can't figure that part out.
- Thu Feb 14, 2019 10:27 pm
- Forum: Calculating Work of Expansion
- Topic: S=0
- Replies: 12
- Views: 1800
Re: S=0
I think it's deltaS that can be zero. Not too sure if S itself can be zero, maybe at the hypothetical subzero?
- Tue Feb 12, 2019 2:15 pm
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: Application of Standard Enthalpy of Formation
- Replies: 1
- Views: 601
Application of Standard Enthalpy of Formation
I'm working through problem 8.99 in the 6th edition and I'm confused about how to apply finding the enthalpy of formation. The problem is long, and parred down to the relevant information it reads: A technician carries out the reaction 2 SO2(g) + O2(g) S 2 SO3(g) at 25 C and 1.00 atm in a constant-p...
- Thu Feb 07, 2019 6:26 pm
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: 4.15 (7th edition)
- Replies: 2
- Views: 361
Re: 4.15 (7th edition)
For reaction enthalpies of combustion, its products-reactants, while it is the other way around for reaction enthalpies of formation. I just kinda memorize this.
- Thu Feb 07, 2019 6:22 pm
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: Units
- Replies: 2
- Views: 281
Re: Units
Some problems will give you the amount of a substance and ask how much heat it gives off, and this is when J/mol comes into play. Other than that I don't think it matters if they're just asking for enthalpy.
- Thu Feb 07, 2019 6:20 pm
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: 4D7
- Replies: 2
- Views: 402
Re: 4D7
-PΔV = -ΔnRT is used to calculate w, which can be calculated using the equation w=-P*ΔV. You need to calculate w in order to calculate ΔU. I don't have the seventh edition, so is there anymore information that the book gives you? Like whether the reaction is reversible or irreversible, or whether T/...
- Thu Jan 31, 2019 9:10 pm
- Forum: Thermodynamic Systems (Open, Closed, Isolated)
- Topic: Studying gases
- Replies: 2
- Views: 371
Re: Studying gases
If it's a work problem, we're probably going to be dealing with gases. Heat problems, however, can have things in basically any state. There's a ton of homework problems, for example, that involve heating a piece of solid metal.
- Thu Jan 31, 2019 9:08 pm
- Forum: Thermodynamic Systems (Open, Closed, Isolated)
- Topic: Extensive
- Replies: 4
- Views: 468
Re: Extensive
A good way to remember the difference between extensive and state property is that the distance between your house and the supermarket is a state property; no matter how you get to the supermarket, that distance will always be the same, it's the state the distance will always be in. The path you tak...
- Thu Jan 31, 2019 9:08 pm
- Forum: Thermodynamic Systems (Open, Closed, Isolated)
- Topic: Extensive
- Replies: 4
- Views: 468
Re: Extensive
A good way to remember the difference between extensive and state property is that the distance between your house and the supermarket is a state property; no matter how you get to the supermarket, that distance will always be the same, it's the state the distance will always be in. The path you tak...
- Thu Jan 31, 2019 9:02 pm
- Forum: Thermodynamic Systems (Open, Closed, Isolated)
- Topic: Piston Problem in class
- Replies: 2
- Views: 415
Re: Piston Problem in class
The external pressure in the equation is really just the normal pressure outside of the system. When work is done by the system and pushes the piston up, this displaces the particles on the other side of the piston and thus results in the energy change. The external pressure changes so little when t...
- Fri Jan 25, 2019 1:44 pm
- Forum: Non-Equilibrium Conditions & The Reaction Quotient
- Topic: ignoring x
- Replies: 10
- Views: 912
Re: ignoring x
You can also check for this by finding the percent protonization by taking the concentration you get and dividing it bby the original concentration of your acid/base. If it's less than 5% then treating x as being so small that it is insignificant is valid.
- Fri Jan 25, 2019 1:41 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: autoprotolysis on Test 1?
- Replies: 2
- Views: 277
Re: autoprotolysis on Test 1?
Solving autoprotolysis should be the same as other weak acids/bases questions, using an ICE table and a pKa/pKb of 10^-7.
- Fri Jan 25, 2019 1:38 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Equilibrium Favoring
- Replies: 4
- Views: 801
Re: Equilibrium Favoring
A reaction favoring either side of an equation is really just saying will the reaction proceed in the forwards or the backwards direction. You know this by calculating Q and then comparing it to K. Since in these quotients are a fraction with products on the top and reactants on the bottom, Q being ...
- Thu Jan 17, 2019 7:33 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Conjugate base
- Replies: 7
- Views: 736
Re: Conjugate base
If the reaction is in water, then whatever molecule that isn't the hydronium or hydroxide ion is the conjugate acid/base, depending on whether the molecule before the reaction is an acid or a base. Acids have conjugate bases and bases have conjugate acids.
- Thu Jan 17, 2019 7:30 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: How temperature affects K
- Replies: 4
- Views: 456
Re: How temperature affects K
Don't quote me on this, but I vaguely recall from high school chemistry that temperature measures the activity level of the particles in a substance while heat measures the energy they give off. I'm probably wrong since my memory is shoddy, and I'm sure we'll learn about this more in detail later on...
- Thu Jan 17, 2019 7:26 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: ICE Tables [ENDORSED]
- Replies: 11
- Views: 2453
Re: ICE Tables [ENDORSED]
If you really want to be sure you can always just check the percent ionization after you solve the problem. If the concentration of the conjugate base/acid divided by the initial concentration of the acid/base is less than 5%, then you're good.
- Thu Jan 10, 2019 5:40 pm
- Forum: Applying Le Chatelier's Principle to Changes in Chemical & Physical Conditions
- Topic: Inert gases
- Replies: 4
- Views: 622
Re: Inert gases
Adding inert gases will only affect the equilibrium if the reaction is in a closed system. They add more particles, which increases the overall pressure and affects the other gases's partial pressure.
- Thu Jan 10, 2019 5:36 pm
- Forum: Applying Le Chatelier's Principle to Changes in Chemical & Physical Conditions
- Topic: compression vs pressure
- Replies: 6
- Views: 692
Re: compression vs pressure
Wait, if compression changes which side of the equation is favored, would that eventually change the Kc too, since Kc tells you which side of the reaction is favored? I'm not really sure, can someone clarify?
- Thu Jan 10, 2019 5:32 pm
- Forum: Applying Le Chatelier's Principle to Changes in Chemical & Physical Conditions
- Topic: Effect of water
- Replies: 2
- Views: 348
Re: Effect of water
Keep in mind that aqueous substances are used in the equilibrium constant, but not liquid substances.
To add on, think of adding more liquid to a system with an aqueous substance like increasing the volume of a gaseous substance. It decreases the concentration of aqueous substances and affects Kc
To add on, think of adding more liquid to a system with an aqueous substance like increasing the volume of a gaseous substance. It decreases the concentration of aqueous substances and affects Kc