Ethyl chloride vapor decomposes by the first-order reaction c2h5cl → c2h4 hcl the activation energy is 249 kj/mol and the frequency factor is 1.6 × 1014 s−1. find the temperature at which the rate of the reaction would be twice as fast as when the reaction runs at 730.6 k. enter your answer numerically and in terms of kelvin.

The temperature at which the rate of the reaction would be twice as fast as when the reaction runs at 730.6 K is 743.12 K.

Explanation:

According to the Arrhenius equation,

= rate of reaction at

= rate of reaction at

= activation energy

R = gas constant  

We have:

The temperature at which the rate of the reaction would be twice as fast as when the reaction runs at 730.6 K is 743.12 K.

"you start with 15.67 g mgco3-xh2o, when heated and all the water is removed, you are left with 7.58 g mgco3 only.

therefore, you had 15.67 - 7.58 = 8.09g h2o  

moles of each :

7.58g mgco3 = ? moles = 7.58g / 83.4g/mole = 0.09moles  

8 09g h2o = ? moles = 8.09g / 18g/mole = 0.44moles  

molar ratio between the two by dividing both numbers by the smallest number :

0.09 / 0.09 = 1  

0.44 / 0.09 = 4.8  

mgco3-5h2o"