For the following reaction,
$$2X + Y\buildrel k \over
\longrightarrow P$$ the rate of reaction is $${{d[P]} \over {dt}} = k[X]$$. 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
Which of the following plots is(are) correct for the given reaction?
([P]0 is the initial concentration of P)
A
B
C
D
3
JEE Advanced 2019 Paper 1 Offline
MCQ (More than One Correct Answer)
+4
-1
In the decay sequence.
x1, x2, x3 and x4 are particles/radiation emitted by the respective isotopes. The correct option(s) is(are)
A
Z is an isotope of uranium
B
x2 is $$\beta $$-
C
x1 will deflect towards negatively charged plate
D
x3 is $$\gamma $$-ray
4
JEE Advanced 2018 Paper 2 Offline
MCQ (More than One Correct Answer)
+4
-1
For a first order reaction $$A\left( g \right) \to 2B\left( g \right) + C\left( g \right)$$ at constant volume and $$300K,$$ the total pressure at the beginning $$(t=0)$$ and at time $$t$$ are $${P_0}$$ and $${P_1},$$ respectively. Initially, only $$A$$ is present with concentration $${\left[ A \right]_0},$$ and $${t_{1/3}}$$ is the time required for the partial pressure of $$A$$ to reach $$1/{3^{rd}}$$ of its initial value. The correct option(s) is (are) (Assume that all these gases behave as ideal gases)
