You visited us 1 times! Enjoying our articles? Unlock Full Access!

First Order Reaction

The reaction ...

Question

The reaction $A (g) ⟶ B (g) + 2 C (g)$ is a first order reaction with rate constant $2.772 \times 10^{- 3} s^{- 1}$ . Starting with $0.1$ mole of $A$ in $2$ litre vessel, find the concentration of $A$ after $250 s e c$ when the reaction is allowed to take place at constant pressure at $300 K$ ?

0.0125 M

No worries! We‘ve got your back. Try BYJU‘S free classes today!

0.025 M

Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses

0.05 M

No worries! We‘ve got your back. Try BYJU‘S free classes today!

none of these

No worries! We‘ve got your back. Try BYJU‘S free classes today!

Open in App

Solution

The correct option is D $0.025 M$
Half life of reaction is $t_{1 / 2} = 0.693 / k = 250$ sec.
So after 250 sec concentration become half and remaing concentration is $0.05 / 2 = 0.025 M$ .

Suggest Corrections

Similar questions

A (g) \to 3 B (g) + 2 C (g)

1.386 \times 10^{- 2} m i n^{- 1}

A (g) \to 3 B (g) + 2 C (g)

1.386 \times 10^{- 2} m i n^{- 1}

2 m o l e s

A

12.5 l i t r e

298 K

B

100 m i n

1^{s t}

A (g) \to B (g) + 2 C (g)

K = 10^{- 2} t i m e^{- 1}

2

5

A (g)

27^{o} C

A (g) ⇌ 2 B (g)

1.5 \times 10^{- 3} s^{- 1}

10^{- 5}

A_{(g)} \to B_{(g)}

l^{- 1}

l^{- 1}

Join BYJU'S Learning Program