Home
Class 12
CHEMISTRY
The reaction A(g)toB(g)+2C(g) is a first...

The reaction `A(g)toB(g)+2C(g)` is a first order reaction with rate constant `2.772xx10^(-3)sec^(-1)` reaction is started with only 0.1 mol of A in a container with volume 2 litre and is allowed to take place at constant volume and at constant temperature `300K[R=0.082` litre atm `mol^(-1)K^(-1)]`
`(log2=0.30)`
Q. Select the correct statement (s)

A

Concentration of C after 250 sec will be 0.05 M

B

concentration of C after 250 sec will be 0.1 M

C

Partial pressure of C after 250 will be 2.46 atm

D

Partial pressure of C after 250 will be 1.23 atm

Text Solution

Verified by Experts

The correct Answer is:
A, D
`underset((0.1)/(2))(A(g))tounderset(0)(B(g))+underset(0)(2C(g))`
`t=250sec`
`t_((1)/(2))=(0.693)/(2.772xx10^(-3))=250sec`
Hence after 250 sec.
`[A]=(0.1)/(2xx2)=0.025M,[C]=2xx(0.1)/(2xx2)=(0.1)/(2)M=0.05M`
`impliesP_(C)=(0.1)/(2)xx0.082xx300=1.23atm`.
Promotional Banner

Similar Questions

Explore conceptually related problems

The reaction A(g)toB(g)+2C(g) is a first order reaction with rate constant 2.772xx10^(-3)sec^(-1) reaction is started with only 0.1 mol of A in a container with volume 2 litre and is allowed to take place at constant volume and at constant temperature 300K[R=0.082 litre atm mol^(-1)K^(-1)] (log2=0.30) Q. Concentration of A after 250 sec will be:

The reaction A(g) to B(g) + 2C(g) is a first-order reaction with a rate constant of 2.303 xx 10^(-3)s^(-1) . Strating with 0.1 moles of 'A' in a 2 litre vessel, find the concentration of A after 301 sec when the reaction is allowed to take place at constant pressure at 300 K.

The reaction A (g) rarr B(g) + 2C (g) is a first order reaction with rate constant 3465 xx 10^(–6) s^(–1) . Starting with 0.1 mole of A in 2 litre vessel, find the concentration of A after 200 sec., when the reaction is allowed to take place at constant pressure and temperature.

The reaction : A(g) rarr 2B(g)+C(g) is first order reaction w.r.t. A, with rate constant 1.386xx10^(-4)sec^(-1) . If initially 0.1 mole/litre of A was taken and the reaction is occurring at constant pressure and temperture then the concentration of A after 5000 sec will be:

A first order reaction has a rate constant of 15 xx 10^(-3) s^(-1) . How long will 5.0 g of this reaction take to reduce to 3.0 g ?

The osmotic pressure of 0.2 molar solution of urea at 300 K(R = 0.082) litre atm mol^(-1)K^(-1) is

The volume of 2.8g of CO at 27^(@)C and 0.821 atm pressure is (R=0.0821 lit. atm mol^(-1)K^(-1))

Identify the reaction order from the following rate constant : k=2.3xx10^(-5)" litre mol"^(-1)"sec"^(-1)

Identify the reaction order from the rate constant value = 3.2 xx 10^(-5) litre mol^(-1)sec^(-1)