Search found 49 matches
- Sat Mar 06, 2021 4:23 pm
- Forum: Second Order Reactions
- Topic: Zero-Order Catalysts
- Replies: 9
- Views: 714
Re: Zero-Order Catalysts
He means that when you have a reaction with catalysts the rate of reaction depends on the catalyst and not the reactant concentration as you have more reactants than catalysts, so the catalyst is always busy, and no matter how much you increase the reactant concentration by the rate of the reaction ...
- Sat Mar 06, 2021 4:19 pm
- Forum: Second Order Reactions
- Topic: half life for second-order reactions
- Replies: 9
- Views: 576
Re: half life for second-order reactions
That's because the plots of concentration vs. time, for first and second orders are different. So when you simplify the equations you get different definitions for t1/2, so t1/2 = 0.693/k for first order and t1/2 = 1/k[A]0 for second order.
- Sat Mar 06, 2021 4:04 pm
- Forum: First Order Reactions
- Topic: Stoichiometric Coefficients and Integrated Rate Laws
- Replies: 5
- Views: 378
Re: Stoichiometric Coefficients and Integrated Rate Laws
And adding on, since that is a constant, in the integration, you can take it out of the internal and just multiply the constant in the final answer.
- Sat Mar 06, 2021 4:01 pm
- Forum: First Order Reactions
- Topic: 1st Order Reactions
- Replies: 29
- Views: 1980
Re: 1st Order Reactions
So you are simply graphing different equations. So ln[A]= -kt+[A]0 (ln[A] gives a straight line), you can modify that to get [A]=[A]0e^-kt and if you plot that you get a decreasing exponential.
- Sat Mar 06, 2021 3:56 pm
- Forum: First Order Reactions
- Topic: Finding order through graphs
- Replies: 17
- Views: 1136
Re: Finding order through graphs
So to find out order from graphs you must compare three graphs, [A] v time, ln[A] v time, and 1/[A] for a certain reactant. Whichever one, is the closest to a linear graph it is the order for that reactant.
- Sat Mar 06, 2021 3:17 pm
- Forum: First Order Reactions
- Topic: Graphing
- Replies: 20
- Views: 1008
Re: Graphing
So it is unlikely that we will have to plot the graphs (although we do it in 14BL). But one way this can be applied is that the question gives us three graphs. One that is [A] v time, other 1/[A] v time and another ln[A] v time. So the one that is the closest to a straight line will be the order of ...
- Sat Mar 06, 2021 3:06 pm
- Forum: Zero Order Reactions
- Topic: Zero order
- Replies: 8
- Views: 689
Re: Zero order
Another example is an enzyme catalyst in a biological reaction. So basically if you need the enzyme to make the reaction happen, the rate of the reaction will only depend on how long the enzyme takes to make the reaction happen if you have fewer enzymes compared to reactants (so the enzyme is never ...
- Sat Mar 06, 2021 3:00 pm
- Forum: Zero Order Reactions
- Topic: Catalyst/Enzymes and Zero Order
- Replies: 4
- Views: 338
Re: Catalyst/Enzymes and Zero Order
So if you think about enzymes as what you need to make the reaction happen. So like an oven when you are trying to make a cake. In this example cake batter is the reactant, but the energy required to make the batter become cake is very high, so you can't just leave the batter out and wait for it to ...
- Sat Mar 06, 2021 2:51 pm
- Forum: Zero Order Reactions
- Topic: Occurrence of Zero Order Reactions
- Replies: 13
- Views: 794
Re: Occurrence of Zero Order Reactions
Zero-order reactions happen normally when you have a catalyst (e.g enzymes) that can facilitate the reaction, which means that once your catalyst is saturated no matter how much you increase your reactant concentration the rate will be the same. So yes, mathematically, the reactant concentration doe...
- Sat Mar 06, 2021 2:44 pm
- Forum: Kinetics vs. Thermodynamics Controlling a Reaction
- Topic: Reaction/Average Rate
- Replies: 13
- Views: 771
Re: Reaction/Average Rate
The average rate of the reaction represents the rate over a certain time interval while the instantaneous rate of the reaction represents the rate of the reaction at a specific point. It is also important to notice that the instantaneous rate of the reaction will normally decrease over time until th...
- Sat Mar 06, 2021 2:39 pm
- Forum: Kinetics vs. Thermodynamics Controlling a Reaction
- Topic: average rate
- Replies: 11
- Views: 644
Re: average rate
so for the average rate of the reactants, (-1/a)dA/dt, the dA/dt will always be negative since the reactant is decreasing as the reaction progresses, but since we are multiplying it by -1/a the overall rate will always be positive.
- Sat Mar 06, 2021 2:35 pm
- Forum: Kinetics vs. Thermodynamics Controlling a Reaction
- Topic: Kinetic stability
- Replies: 14
- Views: 735
Re: Kinetic stability
Ximeng Guo 2K wrote:Is energy barrier equivalent to activation energy?
Yes, the energy barrier is equivalent to the activation energy. In other words, they both exemplify the energy input required to break certain bonds in the reaction.
- Sat Mar 06, 2021 2:26 pm
- Forum: Kinetics vs. Thermodynamics Controlling a Reaction
- Topic: Diamond vs. Graphite
- Replies: 23
- Views: 1127
Re: Diamond vs. Graphite
Yes, it could happen, but it is extremely kinetically unfavorable, therefore it would take a lot of time.
- Sun Feb 21, 2021 10:54 pm
- Forum: Concepts & Calculations Using First Law of Thermodynamics
- Topic: delta U=nCvdeltaT
- Replies: 4
- Views: 2109
Re: delta U=nCvdeltaT
When volume is constant no expansion/compression work is done, remember w= -PdeltaV or w=- deltanRT or for reversible pathways w=-nRTln(v2/V1). So when deltaV=0, w=0 and deltaU= q because deltaU = q+w. And we calculate using q=nCvdeltaT and so delta=nCvdeltaT
- Sun Feb 21, 2021 10:47 pm
- Forum: Calculating Standard Reaction Entropies (e.g. , Using Standard Molar Entropies)
- Topic: 4H.9 textbook
- Replies: 4
- Views: 351
Re: 4H.9 textbook
You need to distinguish between moles and particles. They all have the same number of atoms, but diatomic molecules will have half the number of particles because the atoms are bound together.
- Sun Feb 21, 2021 10:42 pm
- Forum: Calculating Standard Reaction Entropies (e.g. , Using Standard Molar Entropies)
- Topic: Determining most to least ordered (Sapling #7)
- Replies: 5
- Views: 465
Re: Determining most to least ordered (Sapling #7)
In the problem that you are referring to, they discuss the change in molar entropy due to phase change from liquid to gas. This means that all liquids will have a relatively large change in entropy since they are entering a significantly more disordered phase and we are considering that the gases yo...
- Sun Feb 21, 2021 10:37 pm
- Forum: Van't Hoff Equation
- Topic: Van't Hoff [ENDORSED]
- Replies: 6
- Views: 604
Re: Van't Hoff [ENDORSED]
It depends on the information that you are given and what you are trying to solve. So if they give you two K values for two different temperatures, that is a clue that the van't Hoff equation can be used. If you are ever unsure on what equation to use write down everything you know and what do you n...
- Sun Feb 21, 2021 10:34 pm
- Forum: Van't Hoff Equation
- Topic: Celcius vs Kelvin for T1 and T2
- Replies: 84
- Views: 7118
Re: Celcius vs Kelvin for T1 and T2
You should use Kelvin in the van't Hoff equation. If you forget just look at the units in the gas constant which are given in kelvin.
- Sun Feb 21, 2021 10:31 pm
- Forum: Gibbs Free Energy Concepts and Calculations
- Topic: Spontaneity of a System
- Replies: 38
- Views: 2922
Re: Spontaneity of a System
The one thing that will give you "true" spontaneity is the Gibbs Free energy of the reaction because it considers both enthalpy and entropy and which temperature that it is occurring in. Remember that elements want to inhabit the lowest energy state possible but want to inhabit more disord...
- Sun Feb 21, 2021 10:22 pm
- Forum: Gibbs Free Energy Concepts and Calculations
- Topic: When to use delta H of formation and when to use delta H
- Replies: 4
- Views: 275
Re: When to use delta H of formation and when to use delta H
The delta H of formation will be equal to the delta H of the reaction only when the reaction you are observing is the formation of a compound from elements in their standard states (think O2 and C forming CO2). For when to multiply the moles, just keep a lookout for the units of the delta H (kJ/mol ...
- Sun Feb 14, 2021 11:05 pm
- Forum: Gibbs Free Energy Concepts and Calculations
- Topic: Sapling #20
- Replies: 9
- Views: 495
Re: Sapling #20
In #20 when Q=K you are at equilibrium, it is where reactions 'want' to be since it is the lowest energy state and there is no net change in the concentration of products or reactants. Therefore, when Q is not equal to K the reaction will go toward K. If Q<K we know that there is an excess of reacta...
- Sun Feb 14, 2021 10:57 pm
- Forum: Gibbs Free Energy Concepts and Calculations
- Topic: Sapling W5-6 Q15
- Replies: 6
- Views: 336
Re: Sapling W5-6 Q15
For this question you need to pay attention to the manipulations and the units. A + B --> 2D C --> D so you know you want the Ds to cancel and only have A,B,C in your equation so your first step should be to get the Ds at opposite sides. So you reverse the second reaction and multiply dH and dS by -...
- Sun Feb 14, 2021 10:41 pm
- Forum: Thermodynamic Definitions (isochoric/isometric, isothermal, isobaric)
- Topic: Which R to use
- Replies: 42
- Views: 3092
Re: Which R to use
One easy way to know which R to use is by looking at the units, so R=0.08205 L atm mol^-1 K^-1 has both a pressure unit and a volume unit, therefore you need an equation that either requires some value(s) with volume and pressure or you want an answer with volume/pressure. R=8.314 J K^-1 mol^-1 has ...
- Sun Feb 14, 2021 10:32 pm
- Forum: Thermodynamic Definitions (isochoric/isometric, isothermal, isobaric)
- Topic: Sapling Number 5
- Replies: 8
- Views: 483
Re: Sapling Number 5
So in this question, we want to find deltaS and we were given a heat capacity and a temperature change therefore we can use: deltaS= nCvln(t2/t1) all you need to do is plug-in the numbers that you were given and find n using PV=nRT. Remember that your temperatures both should be in Kelvin and that R...
- Sun Feb 07, 2021 8:33 pm
- Forum: Concepts & Calculations Using First Law of Thermodynamics
- Topic: Sapling week 3 and 4 #18
- Replies: 5
- Views: 263
Re: Sapling week 3 and 4 #18
Hi, so you can calculate internal energy change in two ways in this problem. One you can find work by finding the volume change by using Ideal Gas law (PV=nRT), find the volume with the initial temp, and then find the volume with the final temp. (work= - change in volume * pressure, but you have to ...
- Sat Feb 06, 2021 12:32 pm
- Forum: Phase Changes & Related Calculations
- Topic: Why does steam cause severe burns?
- Replies: 22
- Views: 1796
Re: Why does steam cause severe burns?
Steam is in a different phase than boiling water, therefore when water enters in contact with cold skin the heat released is the heat that takes to cool water from boiling temp (100 celsius) to skin temperature. However, when steam enters in contact with the cold skin the difference in temperature m...
- Tue Feb 02, 2021 10:00 pm
- Forum: Applying Le Chatelier's Principle to Changes in Chemical & Physical Conditions
- Topic: How Does Temperature Affect the Equilibrium Constant?
- Replies: 25
- Views: 22713
Re: How Does Temperature Affect the Equilibrium Constant?
Think about this as adding heat or taking away heat from the system. So if the reaction is endothermic, it requires heat, so adding more heat to the system means that the system will want to counter it by using up that heat, so the reaction will favor the product (increase K). If the reaction is exo...
- Tue Feb 02, 2021 9:55 pm
- Forum: Applying Le Chatelier's Principle to Changes in Chemical & Physical Conditions
- Topic: Explaining Le Chatelier's Principle
- Replies: 14
- Views: 1142
Re: Explaining Le Chatelier's Principle
Le Chatelier's principle states that the reaction will try to minimize the effects of changes made upon it. So try to think of this in terms of correcting a change. So if you add reactants to a system, you will make more products to counter the addition of reactants. The same thing happens with pres...
- Tue Feb 02, 2021 9:46 pm
- Forum: Applying Le Chatelier's Principle to Changes in Chemical & Physical Conditions
- Topic: Endothermic and Exothermic Concepts
- Replies: 12
- Views: 664
Re: Endothermic and Exothermic Concepts
Think of this as changes to the system. So if additional heat is added to an exothermic reaction (that releases heat) the reaction will favor the reactants because the reverse reaction of an exothermic reaction is an endothermic reaction, so by favoring the reactants the system will "use up&quo...
- Tue Feb 02, 2021 9:35 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: K vs. Kc
- Replies: 36
- Views: 1431
Re: K vs. Kc
They represent the same concept, the equilibrium constant. Kc is just K using concentrations, while Kp is K using partial pressures. I believe the textbook does not differentiate between K and Kp, and just uses K and Kc, so keep that in mind when doing problems.
- Tue Feb 02, 2021 9:30 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Factors that affect the equilibrium constant
- Replies: 31
- Views: 4197
Re: Factors that affect the equilibrium constant
The only factor that affects K is temperature. So if you change the temperature of a system the reaction you are observing will have another equilibrium constant entirely. Other factors such as pressure and concentration will affect Q, so that the reaction will probably not be at K anymore and will ...
- Tue Feb 02, 2021 9:25 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Making X negligible
- Replies: 34
- Views: 1495
Re: Making X negligible
At first, you should use the Ka/Kb value to see if you can approximate if the equilibrium constant is below 10^-4 then we say that x is so small that the impact it will have on the concentration of the reactant is almost zero, so we don't consider it. However, after you finish your calculation you s...
- Tue Feb 02, 2021 9:20 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Taking the Anti-Log
- Replies: 37
- Views: 2685
Re: Taking the Anti-Log
Here is a quick way to sum it up:
-log(x)=y
x=10^(-y)
-log(x)=y
x=10^(-y)
- Tue Feb 02, 2021 9:16 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: pka vs ka
- Replies: 28
- Views: 1429
Re: pka vs ka
This is because of log laws. If we assume that Ka x Kb = Kw is true we take the -log of both sides: -log(Ka x Kb) = -log (Kw) log law: log(ab)=log(a) + log(b): -log(Ka)+ (-log(Kb))= -log(Kw) So since pKa=-logKa, pKb=-logKb, pKw=-logKw you can write: pKa+pKb=pKw I believe Dr.Lavelle has some math rev...
- Tue Feb 02, 2021 9:07 pm
- Forum: Ideal Gases
- Topic: Reversing Reactions
- Replies: 68
- Views: 2548
Re: Reversing Reactions
When you reverse a reaction that you know K, you can assume that the equilibrium constant for that reaction will be 1/K if the temperature remains the same.
- Tue Feb 02, 2021 9:05 pm
- Forum: Ideal Gases
- Topic: Inverse Kc [ENDORSED]
- Replies: 41
- Views: 2283
Re: Inverse Kc [ENDORSED]
You use 1/Kc when you are looking at the Kc of a reverse reaction. So for example, if they give you Kc=3 for 2C+O2--->2CO @ a given temperature, then 2CO---> 2C+O2 will have a Kc=1/3 at that same temperature.
- Tue Feb 02, 2021 9:01 pm
- Forum: Ideal Gases
- Topic: Chem BL
- Replies: 107
- Views: 8901
Re: Chem BL
Hi, I am taking chem 14BL right now and it mostly overlaps with 14A content, so you might need to freshen up on that, but it shouldn't be a problem for you to take it with 14C.
- Tue Feb 02, 2021 8:59 pm
- Forum: Ideal Gases
- Topic: Exo vs Endothermic
- Replies: 40
- Views: 2566
Re: Exo vs Endothermic
If a reaction is exothermic it releases heat, while if it is endothermic it absorbs/requires heat. When you are forming bonds the reaction is always exothermic because bonds form because they are in a lower energy form than the single atoms, so the element "want" to form bonds. Breaking bo...
- Tue Feb 02, 2021 8:53 pm
- Forum: Ideal Gases
- Topic: Temperature
- Replies: 99
- Views: 7031
Re: Temperature
Yes, when the temperature is not given we assume it is at 25 celsius. Just keep in mind that the problem you are solving might require temperature in Kelvin so you might need to convert it.
- Tue Feb 02, 2021 8:50 pm
- Forum: Ideal Gases
- Topic: response to change in equilibria
- Replies: 6
- Views: 397
Re: response to change in equilibria
When pressure is decreased the reaction will favor the side with the least moles of gas as it will want to restore equilibrium by increasing the quantity of that molecule(s).
- Tue Feb 02, 2021 8:46 pm
- Forum: Ideal Gases
- Topic: Bars to atm [ENDORSED]
- Replies: 41
- Views: 1987
Re: Bars to atm [ENDORSED]
We established that in this course we are using 1bar=1atm
- Thu Jan 28, 2021 6:19 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Would an aq agent be included in K?
- Replies: 27
- Views: 1076
Re: Would an aq agent be included in K?
So, would H20 (g) be included?
- Sat Jan 23, 2021 5:31 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: pKa and Ka
- Replies: 27
- Views: 1017
Re: pKa and Ka
pKa is the negative log of Ka. Keep in mind that this notation is universal(in chemistry), so when you have p of something that means you are taking the -log of that thing.
So:
pH= -log[H3O+], pOH= -log[OH-], pKb= -logKb etc...
So:
pH= -log[H3O+], pOH= -log[OH-], pKb= -logKb etc...
- Sat Jan 23, 2021 5:26 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: ICE Tables
- Replies: 36
- Views: 1946
Re: ICE Tables
When setting up ICE tables the changes in concentration will be dependent on the stoichiometric coefficient. This is because we want to keep the values balanced. Using an example: N2 + 3H2 ----> 2NH3 You need 1mol of N2 to interact with 3mol of H2 and that forms 2 mol of NH3 and say you start with 4...
- Sat Jan 23, 2021 5:04 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: H3O+ and OH- concentration
- Replies: 3
- Views: 159
Re: H3O+ and OH- concentration
Yes, it is safe to assume that [H3O+] and [OH-] are equal as long as the solution is neutral (pH=7), no matter the temperature (just remember that the Kw will have a different value as 10^-14 applies only to 25C). In the case that you are solving for the pH or pOH and are not sure of those values th...
- Fri Jan 15, 2021 6:01 pm
- Forum: Ideal Gases
- Topic: Q and K relationship
- Replies: 22
- Views: 866
Re: Q and K relationship
Rather than trying to memorize it, you should just remember that K is a constant and so Q represents the state of the reaction in relation to that constant. The reaction will always "want" to be in equilibrium and so it will favor either products or reactants in order to achieve the K rati...
- Fri Jan 15, 2021 5:49 pm
- Forum: Ideal Gases
- Topic: T variable in pv=nrt [ENDORSED]
- Replies: 38
- Views: 1750
Re: T variable in pv=nrt [ENDORSED]
It should always be in Kelvin if the problem gives you temperature units in Celsius you should convert it before plugging it in.
- Fri Jan 15, 2021 5:24 pm
- Forum: Ideal Gases
- Topic: PV=nRT
- Replies: 74
- Views: 4841
Re: PV=nRT
P= pressure in atm
V= volume in liters
n= number of moles
R= gas constant (8.31446261815324 J⋅K−1⋅mol−1)
T= temperature in Kelvin
V= volume in liters
n= number of moles
R= gas constant (8.31446261815324 J⋅K−1⋅mol−1)
T= temperature in Kelvin
- Mon Jan 11, 2021 12:24 pm
- Forum: Ideal Gases
- Topic: Does temperature matter?
- Replies: 19
- Views: 606
Re: Does temperature matter?
Yes, temperature does matter when we are talking about K. Altough you do not directly include temperature when calculating K, if there is a change in temperature the value of K will change for the given reaction (even if you start with the same concentration of reactants and products as you did befo...