Question
A chemical reaction was carried out at $$300\,K$$ and $$280\,K.$$ The rate constants were found to be $${k_1}$$ and $${k_2}$$ respectively. then
A.
$${k_2} = 4{k_1}$$
B.
$${k_2} = 2{k_1}$$
C.
$${k_2} = 0.25\,{k_1}$$
D.
$${k_2} = 0.5\,{k_1}$$
Answer :
$${k_2} = 0.25\,{k_1}$$
Solution :
The rate constant doubles for $${10^ \circ }C$$ rise in temperature.
For $${20^ \circ }C$$ rise, the rate constant will be 4 times
$$\therefore \,\,{k_1} = 4{k_2}\,\,{\text{or}}\,\,{k_2} = 0.25\,{k_1}$$