Q1) The activation energy of the reaction: 2HI (g) --------> H₂ + I₂ is 209.5 KJ/mol. Calculate the fraction of molecules of reactants having energy equal to or greater than activation energy.

Q2) The half life for radioactive decay of ¹⁴C    C is 5730 years. A sample had 80%  ¹⁴C . Estimate the age of the sample.

Q3)The rate constant for the decomposition of hydrocarbons is 2.418 * 10^-5  at 546 K. If the energy of activation is 179.9 kJ/mol, what is the value of pre-exponential factor.

Q4)The decomposition of A into product has value of k as 4.5 * 10³ /s at 10 degrees celsius and energy of activation 60 kJ/mol. At what temperature would k be 1.5 8 10⁴ /s.

pls explain

thnx

fpr d last one

log (k2/k1)=Ea/(2.303R)*(T2 - T1/t2*t1)

here substitue k1 as d given value

and k2 we wanna find hope it helps

4 pretty same asw the third one

use the equation k=Ae^-E/RT

so for the process occurin at different temperature energy of activation will remain the same

k1=Ae^-E/RT1

k2=Ae^-E/RT2

so k1/k2=e^(E/R)(1/T2-1/T1)

so let k1=4.5*10^3

T1=283K

k2=1.5*10^4

T2=?

E=60kJ/mol=60000J/mol

solve and calculate the ans

it is a little lengthy calculation but if you have any doubts then please feel free to ask