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