Answer:
The value is 
Explanation:
From the question we are told that
The area is 
The root mean square value is 
The time taken is 
Generally the energy is mathematically represented as

=> 
=> 
Missing details. Complete text is:"The following reaction has an activation energy of 262 kJ/mol:
C4H8(g) --> 2C2h4(g)
At 600.0 K the rate constant is 6.1× 10–8 s–1. What is the value of the rate constant at 785.0 K?"
To solve the exercise, we can use Arrhenius equation:

where K are the reaction rates, Ea is the activation energy, R=8.314 J/mol*K and T are the temperatures. Using T1=600 K and T2=785 K, and Ea=262 kJ/mol = 262000 J/mol, on the right side of the equation we have

And so

And using

, we find K2:
Answer:
T=5797.8 K
Explanation:
Given that
Power P = 3.9 x 10²⁶ W
Radius ,r= 6.96 x 10⁸ m
We know that ,From Plank's law
P = σ A T⁴
σ = 5.67 x 10 ⁻⁸
A= Area ,T= Temperature ( in Kelvin)

Now by putting the values


T=5797.8 K
The temperature of surface will be 5797.8 K
Lucas works in the biopharming field. (Hope it’s right!)