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### Units of k

Posted: Wed Feb 28, 2018 9:15 pm
Can someone go over how we determine the units of k for different orders of reactions? What impacts do the units make on our calculations?

### Re: Units of k

Posted: Wed Feb 28, 2018 9:18 pm
Basically you take the rate law (rate=k[a] for first order) and the units of rate are always mol.L-1.s-1 and then the units of concentration are always mol.L-1 and then you plug those in to find units of k, which would be s-1.

### Re: Units of k

Posted: Wed Feb 28, 2018 9:19 pm
The units of k can change the units for rate when you are using it in a calculation

### Re: Units of k

Posted: Thu Mar 01, 2018 8:41 am
Rate = k[A]^n, where n is the exponent that represents order of the reaction. Concentration is always going to have units of M/L, which is the equivalent to mol.L-1.s-1. Be sure to apply the exponent to the units of the concentration as appropriate. You want to isolate k to be alone on one side of the equal sign to find its units. Since the units of rate are always mol.L-1.s-1, you can divide the units of the rate by the units of [A]^n.

### Re: Units of k

Posted: Thu Mar 01, 2018 10:04 am
Also the time units do not always have to be in seconds. Any time unit works, just make sure that you units are consistent throughout the calculation.

### Re: Units of k

Posted: Thu Mar 01, 2018 3:41 pm
the units themselves have no impact on the numerical answer, unless they involve a conversion factor (for example mmol to mol)

### Re: Units of k

Posted: Fri Mar 02, 2018 9:20 am
Since Rate= mol•L^-1•S^-1
AND [A]= mol•L-1

First order rate = K1*[A]

And calculate the unit of K1

### Re: Units of k

Posted: Fri Mar 02, 2018 11:07 am
Unit of K is in a format so that the rate becomes mol/L S

### Re: Units of k

Posted: Fri Mar 02, 2018 11:11 am
Units of k start out at mol/(L*s) at the zero order and every time you go up one order you can multiply by L/mol to get the new units of k.

### Re: Units of k

Posted: Fri Mar 02, 2018 1:04 pm
I think the units of k is the same units as concentration.

### Re: Units of k

Posted: Fri Mar 02, 2018 1:14 pm
For a 1st order reaction, k units = s^-1
2nd order reaction, k units = L/(mol*s)
and increasing the powers of L and mol as you go up in reaction order so that rate will be in unit of mol/(L*s)

### Re: Units of k

Posted: Fri Mar 02, 2018 2:15 pm
I know this question has been answered many times, but the simplest response is just to do dimensional analysis and multiply everything out. The units of k will be whatever makes the equation work out, so they differ according to the order of the reaction.

### Re: Units of k

Posted: Fri Mar 02, 2018 2:45 pm
The unit of the rate of reaction is mol•L^-1•S^-1, so you just have to manipulate the unit of K so that when put into the equation will give you mol•L^-1•S^-1.

### Re: Units of k  [ENDORSED]

Posted: Fri Mar 02, 2018 2:56 pm
An easy way of rememberin gthis is to to take (M^1-x)/s where s is the order of the reaction.
For example, for a 1st order reaction 1-1=0 and M^0=1 so the unit for k will be 1/s for 1st order rxn.