For the following reaction

the rate of reaction is $$\frac{d[P]}{dt} = k[X]$$. Two moles of X are mixed with one mole of Y to make 1.0 L of solution. At 50 s, 0.5 mole of Y is left in the reaction mixture. The correct statement(s) about the reaction is(are)
(Use: ln 2 = 0.693)

A

The rate constant, k, of the reaction is $$13.86 \times 10^{−4} s^{-1}$$.

B

Half-life of X is 50 s.

C

At 50 s, $$-\frac{d[X]}{dt} = 13.86 \times 10^{-3} mol L^{-1} s^{-1}$$

D

At 100 s, $$-\frac{d[Y]}{dt} = 3.46 \times 10^{-3} mol L^{-1} s^{-1}$$