units

[Rhea Shah 2F]

How do I determine the units of k for a reaction?

[SnehinRajkumar1L]

In your rate law equation, you'd multiply out the units of the reactants to find the units.

[JonathanS 1H]

The equilibrium constant, K has no units. If you mean rate constant, k, then the units are mol.L^-1.s^-1 for a zero order reaction, s^-1 for a first order reaction, and L.mol^-1.s^-1 for a second order reaction.

[Cavalli_1H]

K is a relative ratio so from my understanding it has no specific units

[KHowe_1D]

K (the equilibrium constant) has no units.

[VLi_2B]

K = equilibrium constant has no units
k = rate constant units fluctuate between orders

0 order units: M/s, M/min, M/hr, etc.
1st order units: s-1, min-1, hr-1, etc.
2nd order units: M-1s-1, M-1min-1, M-1hr-1, etc.

[Chris Charton 1B]

The equilibrium constant does not have units

[chari_maya 3B]

There is a chart explaining this on page 595 of the textbook

[Areli C 1L]

I don't think K has units? thought it was unitless since its an EQ constant.

[Niharika 1H]

the rate constant k has units s-1 for a first order reaction, and (L*mol-1*s-1) for a second order reaction.

[Nathan Rothschild_2D]

for 0 order reactions the units are M/s (or any unit for time)

[Zoya Mulji 1K]

the units will depend on the rate law and the order of the reaction because that will influence the power to which the units are multiplied. I would find the answer and then write out the formula with just the units to calculate/find what those would be.

[Orrin Zhong 4G]

k has different units depending on what order the reaction is. Since rate has units (mol x L)/s, you just set up a unit equation: mol x L/s = k x (mol x L)^(order of rxn) and solve for the units of k.