A first order reaction has rate constants of 4.6 x 10-2 s-1 and 8.1 x 10-2 s-1 at 0ºC and 20ºC, respectively. What is the value for the activation energy?
A.
0.566 J/mol
B.
2.5 x 10-4 J/mol
C.
2260 J/mol
D.
18,800 J/mol
E.
1.76 J/mol

D.  18,800 J/mol

Explanation:

We need to use the Arrhenius equation to solve for this problem:

, where k is the rate constant, A is the frequency factor, is the activation energy, R is the gas constant, and T is the temperature in Kelvins.

We want to find the value of , so let's plug some of the information we have into the equation. The gas constant we can use here is 8.31 J/mol-K.

At 0°C, which is 0 + 273 = 273 Kelvins, the rate constant k is . So:

At 20°C, which is 20 + 273 = 293 Kelvins, the rate constant k is . So:

We now have two equations and two variables to solve for. We just want to find Ea, so let's write the first equation for A in terms of Ea:

Plug this in for A in the second equation:

After some troublesome manipulation, the answer should come down to be approximately:

Ea = 18,800 J/mol

The answer is thus D.

the answer is definitely c.

answer: e.   sour taste

explanation: acids are those substances which dissociates in water to give ions. as they dissociate to give ions, they act as electrolytes and thus are electrically conductive. acids are sour in taste. example: hcl

bases are those substances which dissociates in water to give ions or accepts ions. as they dissociate to give ions, they act as electrolytes and thus are electrically conductive. bases are bitter in taste. bases are slippery in nature.