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FAQs
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What does heterogeneous mean?
Heterogeneous refers to a structure with dissimilar components or elements, appearing irregular or variegated. For example, a dermoid cyst has heterogeneous attenuation on CT. It is the antonym for homogeneous, meaning a structure with similar components. Heterogenous refers to a structure having a foreign origin. -
What is an example of a heterogeneous mixture?
A salad with lettuce, cheese, seeds, tomatoes, broccoli, and other vegetables is an example of a heterogeneous mixture. Soil is an example of a heterogeneous mixture. It combines many different components which are not uniform, such as stone, clay, decaying plant material and even living things. -
What is a heterogeneous equilibrium?
A heterogeneous equilibrium is a system in which reactants and products are found in two or more phases. The phases may be any combination of solid, liquid, or gas phases, and solutions. -
What is an example of a heterogeneous reaction?
Examples. The reaction between acid and metal is a heterogeneous reaction. A reaction between a gas and a liquid, as between air and seawater, is heterogeneous. A reaction at the surface of a catalyst is heterogeneous. -
What's an example of heterogeneous?
Mixing together two solids, without melting them together, typically results in a heterogeneous mixture. Examples include sand and sugar, salt and gravel, a basket of produce, and a toy box filled with toys. ... The liquid that is immiscible form heterogeneous mixtures. A good example is a mixture of oil and water. -
What are the 5 examples of heterogeneous mixture?
Concrete is a heterogeneous mixture of an aggregate: cement, and water. Sugar and sand form a heterogeneous mixture. ... Ice cubes in cola form a heterogeneous mixture. ... Salt and pepper form a heterogeneous mixture. Chocolate chip cookies are a heterogeneous mixture. -
What is heterogeneous explain?
Heterogeneous most generally means consisting of different, distinguishable parts or elements. The word is used in a more specific way in the context of chemistry to describe a mixture consisting of two or more different substances or the same substance in different phases of matter (such as ice and liquid water). -
What are 10 examples of homogeneous mixtures?
Sea water. Wine. Vinegar. Steel. Brass. Air. Natural gas. Blood. -
What is an example of a heterogeneous equilibrium reaction?
Examples of Heterogeneous Equilibrium As you can see above reaction is in equilibrium and water steam, carbon monoxide, hydrogen is present in gaseous phase while red hot carbon is in solid phase. Therefore, it is an example of heterogeneous equilibrium. -
What are 10 examples of heterogeneous mixtures?
Cereal in milk is a great example of a heterogeneous mixture. ... Oil and water form a heterogeneous mixture. Orange juice with pulp is a heterogeneous mixture. ... Sandy water is a heterogeneous mixture. ... A pepperoni pizza is a heterogeneous mixture. -
What does homogeneous mean in ultrasound?
\u2022 Homogeneous: organ parenchyma is uniform in echogenicity (Figure 1-4). \u2022 Inhomogeneous or heterogeneous: organ parenchyma is not uniform in echogenicity (Figure 1-5). Ultrasound Artifacts. -
What are homogeneous and heterogeneous equilibria?
Homogeneous and heterogeneous equilibrium is a system of chemical equilibrium which depend upon the states of matter of the substances involved. Homogeneous equilibrium involves substances in the same state. Heterogeneous equilibrium involves substances in different states. -
What is heterogeneous solution?
Heterogeneous Mixtures A heterogeneous mixture is a mixture in which the composition is not uniform throughout the mixture. ... A heterogeneous mixture consists of two or more phases. When oil and water are combined, they do not mix evenly, but instead form two separate layers. Each of the layers is called a phase. -
Which of the following represent heterogeneous equilibrium?
We have solids, and we have a gas sharply different phases, so that would represent a heterogeneous equilibrium. -
What is heterogeneous give examples?
Entropy allows for heterogeneous substances to become homogeneous over time. A heterogeneous mixture is a mixture of two or more compounds. Examples are: mixtures of sand and water or sand and iron filings, a conglomerate rock, water and oil, a salad, trail mix, and concrete (not cement). -
What is an example of a heterogeneous solution?
Mixtures in two or more phases are heterogeneous mixtures. Examples include ice cubes in a drink, sand and water, and salt and oil. ... For example, you can make a homogeneous solution of sugar and water, but if there are crystals in the solution, it becomes a heterogeneous mixture. -
What does it mean when a disease is heterogeneous?
A genetic or allelic heterogeneous condition is one where the same disease or condition can be caused, or contributed to, by varying different genes or alleles. In clinical trials and statistics the concepts of homogeneous and heterogeneous populations is important. -
What is the meaning of heterogeneous solution?
A heterogeneous mixture is a mixture with a non-uniform composition. ... Here, a homogeneous mixture is one in which all components are in a single phase, while a heterogeneous mixture contains components in different phases. -
What does homogeneous mean in medical terms?
Medical Definition of homogeneous : of uniform structure or composition throughout. Other Words from homogeneous. -
What does heterogeneous mean in medical terms?
Heterogeneous medical condition or heterogeneous disease in medicine are those medical conditions which have several etiologies, like hepatitis or diabetes. ... The word is used as an opposition to homogeneous, meaning that given a group of patients, the disease is the same for all of them. -
What does it mean if something is heterogeneous?
: consisting of dissimilar or diverse ingredients or constituents : mixed an ethnically heterogeneous population. -
What is homogeneous and heterogeneous equilibrium give examples?
Therefore, the reaction which takes place between the solutes belongs to a single homogeneous equilibrium. ... A heterogeneous equilibrium, on the other hand, can be defined as a reaction system where the products and the reactants are found in two or more phases. -
What is heterogeneous equilibrium with example?
Dissolving of a gas in a liquid involves changes of two phases. These types of changes are examples of heterogeneous equilibrium. For this type of equilibrium, the equilibrium constant is expressed by the partial pressure rather than by the ratio of pressure and concentration. -
What is the example of heterogeneous?
Mixtures in two or more phases are heterogeneous mixtures. Examples include ice cubes in a drink, sand and water, and salt and oil. The liquid that is immiscible form heterogeneous mixtures. A good example is a mixture of oil and water. -
What does it mean if a mixture is heterogeneous?
A heterogeneous mixture is a mixture in which the composition is not uniform throughout the mixture. ... A heterogeneous mixture consists of two or more phases. When oil and water are combined, they do not mix evenly, but instead form two separate layers. Each of the layers is called a phase. -
What is heterogeneous equilibrium give an example?
The usual examples include reactions where everything is a gas, or everything is present in the same solution. A heterogeneous equilibrium has things present in more than one phase. The usual examples include reactions involving solids and gases, or solids and liquids.
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Heterogenous initial
Let's say we wanted to figure out the equilibrium constant for the reaction boron trifluoride in the gaseous plus 3-- so for every mole of this, we're going to have 3 moles of H2O in the liquid state-- and that's in equilibrium. It's going forward and backwards with 3 moles of hydrofluoric acid, so it's in the aqueous state. It's been dissolved in the water. If it wasn't dissolved, if it was in the solid state, you would call this hydrogen fluoride. Once it's in water, you call it hydrofluoric acid, and we'll talk more about naming in the future, hopefully. Plus 1 mole of boric acid, also in the aqueous state. It's dissolved in the water. H3BO3 in the aqueous state. So what would the expression for the equilibrium constant look like in this situation? So you might be tempted say, OK, that's easy enough, Sal. So the equilibrium constant, you just take the right-hand side. That's just the convention. There's symmetry here. I could've rewritten it either way, but let's just say you take the right-hand side and say, OK, this is dependent on the concentration of the hydrofluoric acid, the concentration of the HF, or the molarity of the HF, to the third power, times the concentration of the boric acid, H3BO3. And remember, this intuition of why you're taking this to the third power is what's the probability-- because in order for the reaction to go this way, you need to have 3 molecules of hydrofluoric acid being very close to 1 molecule of the boric acid. So if you watched the last video I just made about the intuition behind the equilibrium constant, this is indicative of the probability of this reaction happening or the probability of finding all of these molecules in the same place. Of course, you can adjust it with a constant and that's essentially what that does. But that's on the product side, or the reactant, depending on what direction you're viewing this equation, divided by the molarity of the boron trifluoride times-- and I'll do this in a different color-- the molarity of the H2O to the third power. And that's, of course, the H2O liquid. So there you go. We'll just figure this out. And my rebuttal to you is I want you to figure out the molarity of the water. What is the concentration of the water? Remember, the concentration is moles per volume, but in this case, what's happening? I'm putting some boron trifluoride gas essentially into some water, and it's creating these aqueous acids. These other molecules are dissolved completely in the water. So what's the solvent here? The solvent is H2O. This might be how the reaction happens, but pretty much, there's water everywhere. The water is in surplus. So if you were to really figure out the concentration of water, it's everywhere. I mean, you could say everything but the boron trifluoride, but it's a very high number. And if you think about it from the probability point of view, if you say, OK, in order for this reaction to happen forward, I need to figure out the probability of finding a boron trifluoride atom or molecule-- actually, molecule-- in a certain volume, and it also needs 3 moles of water in that certain volume. But you say, hey, there's water everywhere. This is the solvent. There's water everywhere, so I really just need to worry about the concentration of the boron trifluoride. So you could say the forward reaction rate, rate forward, is going to be dependent on some forward constant times just the concentration of the boron trifluoride. The water's everywhere, so you don't have to multiply it times the concentration of water, whatever that means, because the water's everywhere. So the denominator here, you do not put the solvent. So the correct answer for this one is you only put whatever is actually dissolved in the solution. Because frankly, the concentration doesn't actually makes sense for everything else, and if you think about it from the probability point of view, that also makes sense, because there's always water around. If you said, OK, what's the probability of finding water at any small volume of our fluid, it's going to be 1, so you could just multiply it by a 1 there, but that doesn't make a difference. Now, what about the following reaction? Any equilibrium where you have different states of matter is called a heterogeneous equilibrium. And so let me write another heterogeneous equilibrium. So let's say I have H2O in the gaseous state and that's essentially steam-- so it's not going to be the solvent this time-- plus carbon in the solid state. And let's say that that's an equilibrium with hydrogen in the gas state plus carbon dioxide in the gaseous state. This is a heterogeneous equilibrium because you have things in the gaseous and the solid state. And solid state, by definition, it can't be dissolved either into the gas or into the-- when we talk about solutions, we talked about colloids and suspensions and mixtures before, but we're talking about solutions. By definition, if this is in the solid state, it's not dissolved. If this was dissolved, we would write an aq here. It would be the aqueous state. So if you talk about the forward reaction, what's the forward reaction going to be dependent on? So the rate forward, well, the solid, there's a big block of carbon sitting there. There's a big cube of carbon there, and there's steam, there's water gas all around it. So if you pick any volume, especially if you pick some volume near the boundary of the carbon, you're always going to have carbon around. It's just what matters is the concentration of the water gas. That's what's going to drive the forward rate, so the forward rate is going to be dependent on some constant times the concentration of the water gas. And, of course, the backwards rate, so you need to get some H2, some molecules of-- let me draw it like that, because it has 2 hydrogen molecules plus a carbon dioxide, so maybe a carbon dioxide looks like that. So the reverse reaction, so rate, let's call that reverse, is going to be equal to some constant times the probability of finding both of these molecules in the same place. And, of course, the probability is related to or it's on a first-level approximation, depending on the concentration. So it's concentration of H2 times the concentration-- and to find both of them, you multiply the probability, because you need this and that-- times the concentration of CO. So when a reaction is in equilibrium, these two equal each other-- this is an r right here-- so this is going to be equal to the reverse rate of reaction H2 times carbon dioxide. Divide both sides by the K's, both sides by the H2O, and you get the forward coefficient or constant or whatever you want to call that, divided by the reverse constant-- I'm just dividing both sides by that-- is equal to this-- let me just copy and paste that-- is equal to that divided by this. You take that and you divide it by that. And so if we call this the equilibrium constant, because it's just two arbitrary constants, so we can just call this the equilibrium constant, you see that it actually makes a lot of sense to ignore the solid state in your equilibrium reaction. So the two takeaways here is when you're trying to calculate an equilibrium constant, you should ignore-- especially when it's in a heterogeneous equilibrium-- you should ignore the solution-- or not the solution. Ignore the solvent in that first example, where I did it with boron trifluoride with water. Water was the solvent, so I ignored it. Because water is everywhere, and you also ignore the solid state. Ignore the solid. Anyway, we'll probably use these in future things where we actually calculate the equilibrium constant. See you in the next video where we'll learn about Le Chatelier's principle.
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