## Zero Order Meaning

$\frac{d[R]}{dt}=-k; [R]=-kt + [R]_{0}; t_{\frac{1}{2}}=\frac{[R]_{0}}{2k}$

AngelaLin_1D
Posts: 5
Joined: Fri Sep 25, 2015 3:00 am

### Zero Order Meaning

If the reaction is a zero order, and the rate of reaction is independent, how come a slope still exists for the straight line?

Chem_Mod
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### Re: Zero Order Meaning

for zero order, Rate=k so plotting the concentration vs time gives a constant slope, ie. straight line

Millie Unti 4H
Posts: 13
Joined: Fri Sep 25, 2015 3:00 am

### Re: Zero Order Meaning

Basically, what its saying, is the CHANGE of the concentration of the reactant/reactants doesn't have an affect on the line.

Hue_Vo_1D
Posts: 19
Joined: Wed Sep 21, 2016 2:56 pm

### Re: Zero Order Meaning

Rate of zero-order rxn = k

Note that what we're plotting in zero-order reaction is Concentration of R vs Time, which yields a straight line with slope of m, represented by k. The reaction is independent of initial condition, so [R]-reactant concentration of that specific rxn will decrease at a constant rate of k despite initial [R] given.

mayasinha1B
Posts: 70
Joined: Fri Sep 29, 2017 7:04 am

### Re: Zero Order Meaning

Will a zero order reaction mean that changing the concentrations will result in no change?

Jennie Fox 1D
Posts: 66
Joined: Sat Jul 22, 2017 3:01 am

### Re: Zero Order Meaning

Rate is equal to k in a zero order reaction, and therefore plotting the points creates a straight line