The equation below shows a reaction that is second order in A and first order in B.

2A(g) +B(g) -- C(g)

What is the rate law for the reaction?

A. R=k[A][B]^2
B. R=k[A]^2[B]
C. R=k[AB]^2
D. R=k[2AB]
@aaronq

Question

The equation below shows a reaction that is second order in A and first order in B.

2A(g) +B(g) --> C(g)

What is the rate law for the reaction? 

A. R=k[A][B]^2
B. R=k[A]^2[B]
C. R=k[AB]^2
D. R=k[2AB]
@aaronq

aaronq · Answer

the "order" just refers to the exponent in the rate law.

$\sf rate=k[A]^y[B]^x$

here A is to the 'yth' order and B is to the 'xth' order

anonymous · Answer

I don't understand.
Would i plug stuff in?
Im lost.

anonymous · Answer

OH!

anonymous · Answer

It would be B wouldn't it.

aaronq · Answer

you dont have to plug anything in. Just look at the options.

The equation below shows a reaction that is $\sf second ~order ~in ~A$ and $\sf first ~order ~in ~B$.

aaronq · Answer

yes

anonymous · Answer

Oh! I get it. Thanks, i'll post another.

aaronq · Answer

no problem!