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ohms law
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If someone could check my work on this, I'd appreciate it:
Thanks!
Thanks!
ohms law said:@epenguin, it's an equilibrium constant (K), not a rate constant (k).
:)
ohms law said:Gen chem, so all equilibrium constants are dimensionless. Period.
You're talking about stuff in physical chem. I have enough on my plate without adding unnecessary complexity, thanks.
:)
Here's a more complete explanation, though:
View attachment 52439
Besides, this problem was about finding the concentration of one of the reactants. The units work out to Molarity^1, which makes perfect sense, so... what's the problem?
To calculate the reactant concentration from chemical equilibrium moles, you will need to know the equilibrium constant (K) for the reaction and the initial concentrations of the reactants. Then, you can use the formula [Reactant] = [Initial Reactant] - (x * [Stoichiometric Coefficient]), where x is the number of moles consumed or produced in the reaction. This will give you the equilibrium concentration of the reactant.
The equilibrium constant (K) is a value that represents the ratio of the concentrations of products to reactants at equilibrium for a given reaction. It is calculated using the formula K = [Product]n / [Reactant]m, where n and m are the coefficients in the balanced chemical equation. The value of K is dependent on temperature and is a measure of the extent of the reaction at equilibrium.
The initial concentrations of the reactants can be determined by using the known amounts of each reactant and the volume of the solution. If the reaction takes place in a closed system, the initial concentration can be calculated using the ideal gas law, PV = nRT, where P is pressure, V is volume, n is the number of moles, R is the ideal gas constant, and T is temperature.
Yes, you can calculate the reactant concentration at any point during the reaction as long as you know the initial concentrations, the equilibrium constant, and the number of moles consumed or produced at that point. Keep in mind that the equilibrium concentration may change as the reaction progresses, so the calculation will only be accurate for that specific point in time.
The concentration of the reactant does not directly affect the equilibrium constant. The value of K is determined by the temperature and the nature of the reaction, not the initial concentrations of the reactants. However, the concentration of the reactant can indirectly affect the value of K if it impacts the rate of the reaction and the time it takes to reach equilibrium.