The rate constant of a certain reaction is known to obey the Arrhenius equation, and to have an activation energy Ea= 50.0 KJ/mol. If the rate constant of this reaction is 0.14M^-1 s^-1 at -8.0°C. What will the rate constant be at 56.0°C?

The rate constant at 56.0°C is

Explanation:

To calculate rate constant at two different temperatures of the reaction, we use Arrhenius equation, which is:

where,

= equilibrium constant at -8.0°C =

= equilibrium constant at 56°C = ?

= Activation energy = 50.0 kJ/mol = 50000 J/mol   (Conversion factor:  1 kJ = 1000 J)

R = Gas constant = 8.314 J/mol K

= initial temperature =

= final temperature =

Putting values in above equation, we get:

Hence, the rate constant at 56.0°C is

explanation:

metals have excess of electrons whereas non-metals have deficiency of electrons. thus, in order to gain stability metals easily donate their electrons to the non-metals.

for example, electronic configuration of sodium is and electronic configuration of phosphorous is .

when a phosphorous atom and sodium atom combine together then sodium will donate is extra one electron to the phosphorous atom. as a result there will be formation of ionic bond between sodium and phosphorous.

the reaction will be as follows.

there, are three sodium sodium atoms and each of them will donate its one extra electron to phosphorous atom. thus, the sub-shell of phosphorous gets completely filled.  

thus, we can conclude that electrons are transferred from atoms of sodium to atoms of phosphorous. this transfer makes the sodium atoms donate one electron and the phosphorous atoms to gain one electron. as a result, the sodium and phosphorus atoms strongly attract each other.

atomic number of carbon is 6

electronic configuration of carbon is 1s²2s²2p²

orbital diagram of c is as shown here in the image.