The half life period of a reaction is halved as the initial concentration of the reactants is doubled. The order of reaction is:
A. 0.5
B. 2
C. 1
D. zero
Correct Answer - B
c) `t_(1//2) propto 1/([A_(0)]^(n-1)),(t_(1//2))_(1)/(t_(1//2))_(2) = [A_(0)]_(2)^(n-1)/([A_(0)]_(1)^(n-1))={([A_(0)]_(2))/([A_(0)]_(1))}^(n-1)`
`t/(t_(1//2))=(2a)/(a)^(n-1)` or `2=(2)^(n-1)` or n-1 or n=2
Correct Answer - D
d) `underset("Initial conc")(12M)overset(t_(1//2))to6Moverset(t_(1//2))tounderset("Final conc.")(3M)`
`t_(1//2) = 10`min , k = `(0.693)/(10)=0.0693 min^(-1)`
After 20 minutes, the concentration will be 3M.
rate =k[3M] = `(0.0693 min^(-1) xx 3M)`s
Correct Answer - C
`A + 2B to C`
Since the reaction rate becomes double when the concentration of A is made twice order w.r.t A=1
Since the reaction rate becomes...
Correct Answer - B
`xto` product (zero order)
Till the concentration of X changes from `X_0` to `X_0/2` , it is zero order with rate constant k.
Time taken for concentration...
Correct Answer - D
Consider a hypothetical change.
`A+BhArrC+D`
For the reaction.
`K_(eq)=([C][D])/([A][B])`
For the above reaction if concentration of reactions are doubled then the rate of forward reaction increases for...