## size

$\frac{d[R]}{dt}=-k[R]; \ln [R]=-kt + \ln [R]_{0}; t_{\frac{1}{2}}=\frac{0.693}{k}$

kevinolvera1j
Posts: 103
Joined: Fri Aug 02, 2019 12:15 am

### size

Does the size of the reactant influence the rate? I.E. is a bigger molecule consumed at a faster rate than say a hydrogen atom?

Dina Marchenko 2J
Posts: 54
Joined: Thu Jul 25, 2019 12:16 am

### Re: size

I believe only the stoichiometric coefficient of the reaction would impact the rate (ie- if 2 or 1 or 3 molecules are colliding, etc.)

Abby Soriano 1J
Posts: 103
Joined: Sat Aug 24, 2019 12:16 am

### Re: size

I would assume that it would make it easier for the molecules to collide if they were bigger in size, so it is possible that the rate would increase, but I'm not too sure.

Anthony Hatashita 4H
Posts: 103
Joined: Wed Sep 18, 2019 12:21 am

### Re: size

It's possible given that it would be able to come into contact with more at one time, but for this class I'm pretty sure just the stoichiometric coefficients matter.

KnarGeghamyan1B
Posts: 102
Joined: Fri Aug 09, 2019 12:15 am

### Re: size

Smaller particles have more surface area, which allow for the possibility of more collisions and increase the rate.

Philomena 4F
Posts: 27
Joined: Wed Feb 27, 2019 12:16 am

### Re: size

I read that if a particle (ie. solid reactant) is broken down into small bits, it leads to greater surface area and a faster reaction rate. But it doesn't affect the formed products in any way.

Ayushi2011
Posts: 101
Joined: Wed Feb 27, 2019 12:17 am

### Re: size

No, only stoichiometric coeffecients affect the rate of a reaction, not the size of the reactant molecules.