q vs k
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Re: q vs k
Q is the reaction quotient and expresses the relative ratio of products to reactants at a given instant. On the other hand, K is the equilibrium constant and is used to calculate the final concentrations at equilibrium for a reaction using an ICE table. If Q and K equal each other, the reaction is at equilibrium.
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Re: q vs k
Yes, when Q=K the solution has reached its equilibrium composition and doesn't change in either direction.
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Re: q vs k
Yes Q is just the value of equilibrium at any given point and K is the equilibrium constant. When Q and K are equal, that would show you that the reaction is at equilibrium.
Re: q vs k
Q value is calculated when you don't know whether the reaction is at equilibrium or not. If Q equals K, then the reaction is at equilibrium.
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Re: q vs k
The q value will eventually reach k given a long period of time, because that's where the reaction occurs at equilibrium.
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Re: q vs k
Q represents the current state of the system but K is the equilibrium state. Eventually, Q will go towards K.
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Re: q vs k
Yes, Q is the reaction quotient that is calculated at any point in time during the reaction. You can compare Q to K to determine which way the reaction will proceed to eventually establish equilibrium where Q=K.
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Re: q vs k
Q is the reaction quotient for any specific moment during a reaction, technically Q does not approach K but the concentrations of the reactant and products will change so that the ratio will be equal to K.
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Re: q vs k
Q should reach K if the reaction is left alone. Once Q equals K the reaction is at equilibrium and the forward and reverse rates of the reaction are the same. If Q > K more reactants will be formed and if Q<K more products will be formed until these values are the same.
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Re: q vs k
Q is the reaction quotient (taken at any time during the reaction). If you let the reaction go until it reaches equilibrium, Q should equal K (since K is the equilibrium constant).
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Re: q vs k
Q is the reaction quotient which is the concentration of products to the concentration of reactants raised to their coefficients. Q can be less than K, greater than K, and equal to K. When Q is less than K, that means there are more reactants than products and the forward reaction needs to occur at a greater rate to reach equilibrium. When Q is greater than K, that means there are more products than reactants and the reverse reaction needs to occur at a greater rate to reach equilibrium. When Q equals K, the reaction is at equilibrium.
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Re: q vs k
yes k and q are the same but k represents the ratio at equilibrium and and q represents other points in the reaction
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Re: q vs k
Yes, q will eventually reach k after letting the reaction take place over time. Q is finding the ratio at a certain time during the reaction, which could be greater than, less than, or equal to k. If the q is equal to k, then the reaction is at equilibrium. However, if q<k, that means there are more reactants in the ratio compared to the equilibrium constant ratio, so the reaction will form more products so that the equilibrium constant is reached. Same applies when q>k, which means there are more products in the ratio, so the reaction will form more reactants so that the equilibrium constant is attained.
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Re: q vs k
Hi! The reaction quotient basically represents the concentration of production to reactant at any given time in the reaction. However, K specifically implies the ratio at equilibrium.
Hope it helps!
Hope it helps!
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Re: q vs k
Yes, Q=K once the reaction is at equilibrium. We use Q for calculations when we're unsure if the reaction has reached equilibrium.
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Re: q vs k
Q, the reaction quotient, tells us the [p]/[r] ratio at any point in the reaction. The value of Q then tells us if our reaction is at equilibrium if (Q=K). If K>Q, then the forward reaction is favored, and if K<Q, then the reverse reaction is favored. We use Q when we are not sure if the reaction is at equilibrium or not.
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Re: q vs k
Hi!
Q is the reaction quotient, or the ratio of products to reactants at any given point in the reaction. Q may equal K (when the reaction is at equilibrium) or it may higher or lower than K (when the reaction is not at equilibrium). If Q is higher than K, the reaction favors the reactants. If Q is lower than K, the reaction favors the products. Hope this helps!!
Q is the reaction quotient, or the ratio of products to reactants at any given point in the reaction. Q may equal K (when the reaction is at equilibrium) or it may higher or lower than K (when the reaction is not at equilibrium). If Q is higher than K, the reaction favors the reactants. If Q is lower than K, the reaction favors the products. Hope this helps!!
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Re: q vs k
Q is the reaction quotient and can be used to figure out which direction the reaction will shift in order to reach equilibrium.
K > Q: reaction proceeds forward, R --> P.
K < Q: reaction proceeds in reverse direction, P --> R.
Q = K: system is at equilibrium, no shift to either left or right
K > Q: reaction proceeds forward, R --> P.
K < Q: reaction proceeds in reverse direction, P --> R.
Q = K: system is at equilibrium, no shift to either left or right
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Re: q vs k
I don't know if this right, but I like to think of Q as any random moment in time during my life, and K as my home. I could be out and about at school, hitting the town on a Saturday night, or watching TV on my couch (pre/post quarantine of course). Q can either be greater than, less than, or equal to K. It all depends on what "moment" you choose (what concentrations/partial pressures) you are given. Sorry if that didn't make sense, I'm feeling kind of poetic today.
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Re: q vs k
they're both the same calculation method but the letter q usually means the solution isn't at equilibrium. but eventually q should reach k after a certain period of time
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Re: q vs k
Q and K are calculated in the same way but Q is the calculation that is not done at equilibrium.
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Re: q vs k
If Q equals K, the reaction is at equilibrium. Q is calculated the same way as K when the reaction is not at equilibrium.
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Re: q vs k
Q calculates the same way as K, but Q calculates at concentrations that aren't equilibrium.
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Re: q vs k
Melis Kasaba 2B wrote:Q is the reaction quotient and can be used to figure out which direction the reaction will shift in order to reach equilibrium.
K > Q: reaction proceeds forward, R --> P.
K < Q: reaction proceeds in reverse direction, P --> R.
Q = K: system is at equilibrium, no shift to either left or right
Thank you for making it easy to understand :)
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Re: q vs k
Yes q will eventually reach k if the temperature remains the same. Also I think of q as a ratio that changes as the reaction continues and becomes equal to k when the reaction “finishes”.
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Re: q vs k
At equilibrium, Q=K. When the value of Q is not the same as the value of Kc, the reaction is not at equilibrium.
Additionally, when Q is less than Kc, the reaction will shift to form more products to reach equilibrium. Vice versa, when Q is more than Kc, the reaction will shift to form more reactants to reach equilibrium.
So eventually if you wait long enough Q=K.
Additionally, when Q is less than Kc, the reaction will shift to form more products to reach equilibrium. Vice versa, when Q is more than Kc, the reaction will shift to form more reactants to reach equilibrium.
So eventually if you wait long enough Q=K.
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Re: q vs k
Yes, it will eventually. Q is the current state reaction quotient and K is the equilibrium constant. Q will eventually reach equilibirum.
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Re: q vs k
When Q = K, the reaction is at equilibrium. K will only change with a temperature change, but Q will change depending on factors such as changes in concentration and pressure.
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Re: q vs k
Yes Q will eventually reach K. And Q is expressed when equilibrium has not yet been reached.
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Re: q vs k
Yes, Q will equal K at equilibrium, while K will not change values (unless the temp is changed) Q will.
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Re: q vs k
Yeah Q will become K, Q is indeed the value when not at equilibrium. Q wants to become closer and closer to K in order to reach equilibrium.
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Re: q vs k
Q is the quotient and will reach K at equilibrium. In the sapling problems there are a few examples of the relationship between q and k, and how knowing both those numbers will tell you which way the reaction is heading.
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Re: q vs k
Hi! Yes you're right, the q value will eventually equal k, when it does this signifies that the reaction is at equilibrium. Yes Q can be calculated at any time, K is only when the reaction is at equilibrium.
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Re: q vs k
Yes, Q can reach K, and when that occurs (Q=K) then the reaction is at equilibrium. Also, yes Q is the value that is calculated when the reaction isn't at equilibrium. On the other hand, K is only calculated when the reaction is at equilibrium.
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Re: q vs k
Yes, Q can reach K, and when that occurs (Q=K) then the reaction is at equilibrium. Also, yes Q is the value that is calculated when the reaction isn't at equilibrium. On the other hand, K is only calculated when the reaction is at equilibrium.
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Re: q vs k
You actually can use q to figure what side the reaction will go to. If q is greater than k the system will shift to the left and if q is less than k the system will shift right.
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Re: q vs k
Yes, the Q value will eventually reach K if the reaction is currently not at equilibrium. If it is at equilibrium then Q = K.
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Re: q vs k
Q is the concentrations at some point before equilibrium is reached and K is at equilibrium.
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Re: q vs k
yep, Q is just a point taken at a certain temperature. When Q=K then it is at equilibrium!
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Re: q vs k
The Q value is the concentrations of the products over the concentration of the reactants at any point in time of the system. This means that Q could be equal to K if the concentrations are equal or proportional to the concentrations at K. Otherwise, Q being greater than or less than K can determine the direction of the system over time. This is all true at any one certain temperature and changes if the temperature is changed.
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Re: q vs k
If Q does not equal K then the reaction is not at equilibrium. If it is less than K then the reaction will shift to the right towards the products to reach equilibrium. If it is greater than K, then it will shift to the left towards the reactants. This makes Q helpful in determining whether a reaction is at equilibrium or not.
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Re: q vs k
Yes, the Q value is the ratio of product/reactant concentrations not at equilibrium, and yes, it should eventually reach equilibrium!
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Re: q vs k
It will eventually reach K yes and q is the initial value measured before k is established
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Re: q vs k
Is there a less obvious explanation for how Q>K because K decreased and K increased because Q< K? The relationship between Q and K is kind of confusing when getting into why Q is < K when the Reactants transfer to the Products side.
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Re: q vs k
When q=k, the reaction is at equilibrium.
If q is greater that k, it means that the reaction will produce more reactants.
If q is less than k, it means that the reaction will produce more products.
If q is greater that k, it means that the reaction will produce more reactants.
If q is less than k, it means that the reaction will produce more products.
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Re: q vs k
Q is the products over reactants at any time of the reaction. If Q=K, then the reaction is at equilibrium. If not, you can determine where the reaction will go to (the products side or the reactants side).
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Re: q vs k
Yeah, q will eventually become K. Q is the product and reaction ratio at a certain time of the reaction. However, as we can infer that it takes a while to get to K. so q is the intermediate until we reach it. Therefore, Q is just a notion of a certain time before it hits K.
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Re: q vs k
The Q value will always come back to equal K. Once the two values are equivalent, it means that the reaction is at equilibrium.
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