The state in which both reactants and products are present at concentrations which have no further tendency to change with time.

learn more… | top users | synonyms

-1
votes
0answers
11 views

identify the choice that best completes the statement [closed]

when a solid barium flouride is in equilibrium with its ions ,the ratio flouride ion to barium is which of the following? a.1:1 b.1:2 c.2:1 d.2:3 e.3:2
-2
votes
2answers
94 views

Predict the standard potential at 310 K for the cell constructed from the hydrogen electrode and metal-insoluble salt electrode

I've run into trouble on this question Predict the standard potential at 310 K for the cell constructed from the hydrogen electrode and metal-insoluble salt electrode $\ce{Ag(s)|AgCl(s)|Cl-}$. ...
0
votes
0answers
48 views

How to determine how much strong acid has been added to phosphate buffer? [closed]

A student dilutes a solution of $0.100~\mathrm{mol}$ of $\ce{H3PO4}$ and $0.150~\mathrm{mol}$ of $\ce{NaOH}$ with water to a volume of $1.00~\mathrm{L}$ but then realizes that the "distilled water" ...
1
vote
1answer
26 views

Stuck with derivation of the integrated rate equation for a pseudo first order equilibrium reaction

I was reading about the integrated rate law. However I have problems to follow the solution. I have an equilibrium reaction: [A]+[B]=[AB] with forward and back reaction. I approximate the ...
2
votes
1answer
51 views

Where does this equation for the activity in the gas phase equilibrium between N2, H2 and NH3 come from?

I have a question with Equilibrium Constant. I understand that for a reaction in equilibrium $aA +bB \rightleftharpoons cC +dD$ $$K_c= \frac{[C]^c[D]^d}{[A]^a[B]^b}$$ and $K_p$ is just using the ...
13
votes
2answers
240 views

What is the difference between “reaction in both directions” and “equilibrium”?

According to the Wikipedia page on Chemical Equations: Symbols are used to differentiate between different types of reactions. To denote the type of reaction: "$=$" symbol is used to denote a ...
2
votes
2answers
37 views

Is this reaction at equilibrium?

The following equilibrium occurs: $$\ce{2 NOCl(g) <=> 2 NO(g) + Cl2(g)}$$ A gaseous mixture of $\ce{NOCl}$, $\ce{NO}$ and $\ce{Cl2}$ is put in a container. After a few minutes it is found that ...
0
votes
1answer
30 views

In the following reaction, will the ratio between substances be 3:1?

In the reaction $$\ce{3 C2H2(g) <=> C6H6(g)}$$ will the ratio of $\ce{[C2H2(g)]}$ to $\ce{[C6H6(g)]}$ at equilibrium be 3:1? How is the mole ratio related to the equilibrium (or lack thereof) ...
3
votes
1answer
47 views

Which has a greater entropy?

Which of the following has greater entropy? a. $\ce{CH3COOH~ (aq)}$ or b. $\ce{CH3COO^{-}~ (aq) + H+~(aq)}$ They are both in the same state, and have the same number of particles.. so how do ...
0
votes
1answer
29 views

Will room-temperature water in a sealed flask evaporate?

Some liquid water is present inside a sealed flask at room temperature. Is water evaporating, and is the system at equilibrium? First of all, can water evaporate in a sealed flask at room temperature? ...
1
vote
1answer
37 views

Can there be more than one combination of reactant/product concentration for a specific equilibrium constant?

For an elementary reaction like $$\ce{A + B -> AB},$$ $$K_{c} = \frac{\ce{[AB]}}{\ce{[A][B]}}$$ and $$\frac{\mathrm{d}\ce{[AB]}}{\mathrm{d}t} = k\ce{[A][B]}.$$ If I let the reaction reach ...
0
votes
1answer
12 views

Exothermic reactions at high temperature and the chemical equilibrium

Why are many exothermic reactions, like Haber process, conducted at high temperature, thus their unfavourable equilibrium position?
0
votes
1answer
15 views

Trouble to predict the effect of pressure and temperature for a reaction in equilibrium

I have trouble to predict the effect of decreasing pressure and increasing temperature on the reaction $N_2 +O_2 = NO_2$. Increasing temperature caused this reaction to shift in the forward direction ...
1
vote
1answer
47 views

Why is CO a major species only in fuel-rich combustion?

In fuel-rich combustion, my understanding is that enough fuel reacts and consumes all of the oxygen present. The combustion products $\ce{CO2}$ and $\ce{H2O}$ undergo dissociation until equilibrium is ...
3
votes
1answer
30 views

Why do strong acids dissociate (almost) fully on a molecular level?

In the Brønsted-Lowry theory, strong acids $\ce{HA}$ dissociate using water and react into hydronium ions and the conjugate bases $\ce{A-}$. However I never understood in the strong acids case what ...
0
votes
2answers
29 views

Balancing Ionic and Net Ionic equations

I am currently taking a chemistry course about acids and bases. One of the things I am a bit confused about, is the acid and base neutralization reaction, and how to balance it. For Example: ...
3
votes
2answers
68 views

If the equilibrium constant in a reaction is greater than 1 is it possible that there are more moles of reactants than products?

I'm wondering if this is possible because could there not be a situation in which the reactants were pure solids/liquids and would therefore not contribute to the value of k but still contain more ...
2
votes
2answers
87 views

Can Ketones next to a Nitrogen hetero atom tautomerise?

I worry that the electronegative N will stabilise keto form so much that equilibrium will be so far towards keto it would be unreasonable to call the enolisiation process a factor
1
vote
1answer
69 views

Redox Question: Concentration of Pb2+ is unknown

What is the concentration of $\ce{Pb^{2+}}$ in a lake that has a pH of 6.0 and is in equilibrium with $\ce{PbO2(s)}$ and atmospheric oxygen? $\ce{PbO2(s) +4H+ +2e- -> Pb2+ +2H2O}$ log K = 49.2 ...
1
vote
3answers
74 views

Filling a buret tip before an experiment

I have a question that asks if the buret tip is not filled before the experiment what would happen (effect on molarity for acid/base titration). The way I'm thinking about it, it's not like you're ...
1
vote
1answer
31 views

can i calculate equilibrium constant of this reaction?

Good day, i had organic chemistry labs. And we had this reaction: $$\ce{(CH3)3COH + HCl -> (CH3)3CCl + H2O}$$ My question is: how do i explain my yield of reaction is only 40%? My theory is: ...
0
votes
1answer
30 views

How do I calculate equilibrium partial pressures of $\ce{H2}$, $\ce{N2}$, and $\ce{H2O}$ and $K_{eq}$ for this problem?

This is the complete problem: A mixture of $0.10$ mol of $\ce{NO}$, $0.050$ mol of $\ce{H2}$, and $0.10$ mol of $\ce{H2O}$ is placed in a $1.0$ L vessel at $300$ K. The following equilibrium is ...
1
vote
1answer
24 views

Is it possible to normalize the concentration equilibrium constant between different reactions for comparison?

A follow up question from this answer: Compare: $\ce{A(aq) +B(aq)->AB(aq)}$ $\ce{2A(aq) +B(aq)->A2B(aq)}$ We have two similar reactions but the equilibrium constants can vary by a ...
1
vote
1answer
43 views

Does Combining Solid/Liquid Concentration with $K_c$ Matter when Comparing $K_c$ of Different Reactions?

I know it is convention to take liquid/solid concentrations as constants and lump it with the equilibrium constant. However, if we were trying to compare the equilibrium constants of two different ...
-1
votes
1answer
47 views

In a reaction if the equilibrium constant K was infinity, could you produce an infinite number of products at equilibrium?

It's impossible to produce an infinite amount products if the k constant was infinity? no right?
2
votes
2answers
51 views

Finding initial pressure in a chemical equilibrium

Consider the equilibrium below. If $K = 4$ and initial pressures of $\ce{CO}$ and $\ce{H2O}$ are equal, giving a total pressure of $1.5~\mathrm{bar}$ at equilibrium. What was the initial pressure of ...
1
vote
2answers
91 views

Effect of addition of inert gas in reaction at equilibrium

Can anyone please explain dissociation reaction increases with the addition of an inert gas? I am still new to the topic equilibrium so please explain in simple words.
0
votes
2answers
29 views

Effect of temperature on equilibrium

Why is exothermic reactions are favoured by low temperature while endothermic reactions are favoured by high temperature?
1
vote
0answers
42 views

Equilibrium constant and reaction Quotient

does reaction quotient After equilibrium has been achieved make any sense? At equilibrium point rates of forward and backward reaction are same and the system is in dynamic equilibrium.The graph of ...
1
vote
0answers
53 views

Are there actually any reactions during which STATIC equilibrium is reached, as opposed to dynamic?

Static would be where a set amount of both products and reactants is formed. Dynamic would be where both the forward and backward reactions occur at equal rates, meaning no change in the overall ...
2
votes
2answers
57 views

Why is equilibrium achieved at different stages of a reaction?

In other words, I want to know why some reactions attain equilibrium early in the reaction while some reactions obtain equilibrium at the end of the reaction. Why is this the case?
0
votes
2answers
25 views

Actual meaning of equilibrium

What is actually meant by that concentration of reactants and products remain constant in equilibrium?
0
votes
1answer
80 views

Buffer action of borax

How does a mixture of borax and boric acid act as an acidic buffer? Please also describe the mechanism of its buffer action.
8
votes
2answers
131 views

How can a protein folding transition state have zero lifetime?

I'm doing a module on my Biochemistry course looking at protein folding, and in a discussion of [folding] transition states I was a little confused at the thought of a zero-lifetime transition state - ...
2
votes
2answers
73 views

Can assumptions made during calculation of ka of buffer solutions be justified?

We make many assumptions in sciences which are not always true but as they make little difference we ignore them for simplicity. But today I have decided that I can no longer be lured into using ...
0
votes
0answers
14 views

How do you calculate the proportion of ammonia produced from different pressures in the Haber process using the equilibrium equation?

I tried to write a increase in pressure to twice as much like this: $$\frac{2(x+1)^2}{(0.5-0.5x)2(1.5-1.5x)^3}=K$$
3
votes
1answer
40 views

Finding the equilibrium constant Kₚ, when temperature is given

At $1000~\mathrm{K}$, $K_p = 1.85$ for the reaction. $$\ce{SO_2 + \frac{1}{2}O_2 <=> SO_3}$$ What is the value of $K_p$ for the reaction $$\ce{SO_3 <=> SO_2 + ...
0
votes
1answer
46 views

Why is the water column empty in ICE table

In the ICE table pure solids and liquids have a value of one in the equilibrium expression but when we create an ICE table, why is the $\ce{H_{2}O}$ column empty? Should it not have a value of one?
2
votes
2answers
810 views

Determining if reaction is endothermic or exothermic using equilbrium constant

For the following reaction: $$W_{(s)}+4\,Br_{(g)}\rightleftharpoons WBr_{4(g)}$$ At 900 K, $K_{p}=100$ and at 2800 K, $K_{p}=5$. At higher temperatures, the equilibrium has shifted towards the ...
1
vote
1answer
78 views

Applying the Le chateliers principle

I am an issue understanding the changes that take place when we decrease the pressure of a reaction. I have understood that when we increase the pressure the side having more number of moles wants ...
2
votes
1answer
35 views

Where can I find Equilibrium Constants?

When trying to develop mathematical models to show the concentration in a reaction, where can one find a database or good source of known equilibrium constants if it is not necessarily very convenient ...
2
votes
1answer
69 views

Why is the equilibrium constant given in litre per mole?

At $800\:\mathrm{K}$ a reaction mixture contained $0.5\:\mathrm{mol}$ of $\ce{SO2}$, $0.12\:\mathrm{mol}$ of $\ce{O2}$ and $5\:\mathrm{mol}$ of $\ce{SO3}$ at equilibrium. $K_c$ for the equilibrium ...
0
votes
0answers
54 views

Name the equation $\Delta G=\Delta G^{\circ}+RT \ln Q$

As the title states, what is the name of the equation $$\Delta G=\Delta G^{\circ}+RT \ln Q$$ My textbook does not explicitly state the name and I could not find anything on google.
1
vote
1answer
56 views

Determining vapor pressure from equilibrium constant

The reaction is $$CoCl_{2(s)}+6\,H_{2}O_{(g)}\rightleftarrows [Co(H_{2}O)_{6}]Cl_{2(s)}$$ Note that the reaction is at equilibrium. I have determined the value of $K_{p}=5.5\times10^{12}$. The next ...
1
vote
1answer
45 views

What does (heated) mean in a chemical equation?

I'm supposed to balance the following equation: $\text{Potassium chlorate (heated) --> Potassium chloride + Oxygen}$ But I don't understand what the (heated) means in front of the first element. ...
2
votes
0answers
26 views

Analytically combining Dynamic Equilibria that have a two way affect?

Lets say I want to model a water system as the following set of equilibria: $\ce{H2O <=> OH- + H3O+}$ | $\ce{A=[OH^{-}][H3O+]}$ $\ce{CO2 + H2O <=> H2CO3}$ | ...
6
votes
1answer
320 views

Acid-base equilibrium of NH4CN

I'm having difficulties understanding this problem. We have in the problem that $K_a$ for $\ce{HCN} = 6.2\cdot10^{-10}$ and $K_b$ for $\ce{NH3} = 1.8\cdot10^{-5}$. Write chemical equations to ...
3
votes
3answers
111 views

Why is the equilbrium constant expressed the way it is?

Why are the two molarity's multiplied and not added and why is each raised to the power of the coefficient rather than multiplied by it? What is the reasoning behind this form? Was it simply ...
0
votes
2answers
27 views

Finding the value of stoichiometric coefficient x

$\ce{2A_{(s)} + xB_{(g)} <=> 3C_{(g)}}$ $K_p=19.3, K_c=0.45, T=523K$ I work $\Delta n$ to be 1, So would $x$ be 1 or 2? I'm not sure if the coefficient is part of $\Delta n$.
2
votes
1answer
98 views

Relationship between rate equation and equilibrium constant

I have read mannaia's answer on the question of 'rate order and confusion', as well as Nicolau Saker Neto's answer to a related question. They have both been very helpful. As I understand, the ...