Home
Class 11
CHEMISTRY
A mixture of a mol of C(3) H(8) and b mo...

A mixture of a mol of `C_(3) H_(8)` and `b` mol of `C_(2) H_(4)` was kept is a container of `V L` exerts a pressure of 4.93 atm at temperature `T`. Mixture was burnt in presence of `O_(2)` to convert `C_(3) H_(8)` and `C_(2) H_(4)` into `CO_(2)` in the container at the same temperature. The pressure of gases after the reaction and attaining the thermal equilirium with atomsphere at temperature `T` was found to be 11.08 atm.
The mole fraction of `C_(2)H_(4)` in the mixture is

A

0.25

B

0.75

C

0.45

D

0.55

Text Solution

Verified by Experts

The correct Answer is:
B
`chi_(C_(2)H_(4))` or `chi_(b) = 1 - 0.25 = 0.75`
Promotional Banner

Similar Questions

Explore conceptually related problems

How will you convert C_(2)H_(5)OH" to "C_(2)H_(5)OC_(2)H_(5) ?

100 mL of O_(2) and H_(2) are kept at same temperature and pressure. What is true about their number of molecules ?

0.5 mol each of H_(2), SO_(2) and CH_(4) are ketp in a container. A hole was made in the container. After 3 hours, the order of partial pressure in the container will be :

If V_(1) mL of a gas at 37^(@)C and 1.2 atm pressure contains N_(1) molecules and V_(2) ml of the gas contains N_(2) molecules at the same temperature and pressure, then :

For the reaction : C_(3)H_(8)(g) + 5O_(2) rarr 3CO_(2)(g) + 4H_(2)O(l) a constant temperature, Delta H - Delta U is

2.8 g of N_(2) , 0.40 g of H_(2) and 6.4g of O_(2) are placed in a container of 1.0 L capacity at 27^(@)C . The total pressure in the container is :