## 15.99 (e)(f)

$aR \to bP, Rate = -\frac{1}{a} \frac{d[R]}{dt} = \frac{1}{b}\frac{d[P]}{dt}$

Hannah Guo 3D
Posts: 56
Joined: Fri Sep 29, 2017 7:06 am

### 15.99 (e)(f)

15.99 Which of the following plots will be linear?
(e) k against temperature;
(f) initial rate against [A] for a reaction that is first order in A;

Can someone explain why e is not linear and f is linear?

Thank you!

Abigail Yap 2K
Posts: 51
Joined: Fri Sep 29, 2017 7:07 am

### Re: 15.99 (e)(f)

I think this is because k and temperature are not directly proportional (they change at different rates), whereas rate and concentration are directly proportional for a reaction that is first order in A (rate = k[A]).

Seth_Evasco1L
Posts: 54
Joined: Thu Jul 27, 2017 3:00 am

### Re: 15.99 (e)(f)

For e) Plotting k against temperature will not produce a linear graph.

If you look at the Arrhenius equation, you'll find that k and T are not directly proportional. If we linearize the equation by taking the natural log of both sides we'll find that ln(k) and 1/T are directly proportional and will produce a linear graph.

Jingyi Li 2C
Posts: 56
Joined: Fri Sep 29, 2017 7:06 am

### Re: 15.99 (e)(f)

(e). The plot of ln(k) against 1/T will be a straight line.
(f). For first order in A, rate=k[A], so initial rate against [A] will be a straight line.