Question

The total pressure for volatile components A and B is 0.02 bar at equilibrium. If the mole fractions of component A is 0.2, then What will be partial pressure of componant B? Select the proper choice from the given multiple choices.
(A) 0.02 bar
(B) 0.04 bar
(C) 0.016 bar
(D) 0.2 bar

Answer 1

c- 0.016
explanation- partial pressure of any gas= molefraction of the gas* total pressure.
mole fraction of A+mole fraction of B= 1
so mole fraction of B is 0.8
hencs the partial pressure of B = 0.8*0.02= 0.016

Answer 2

The partial pressure of component B is 0.016 bar.

Explanation:

According to Raoult's law, the vapor pressure of a component at a given temperature is equal to the mole fraction of that component multiplied by the vapor pressure of that component in the pure state.

$p_1=x_1p_1^0$ and $p_2=x_2P_2^0$

where, x = mole fraction in solution  

$p^0$ = pressure in the pure state

According to Dalton's law, the total pressure is the sum of individual pressures.

$p_{total}=p_A+p_B$

$p_{A}=p_T\times x_{A}$

$x_{A}=0.2$

$p_{A}=0.02\times 0.2=0.004$

$p_{total}=p_A+p_B$

$0.02=0.004+p_B$

$p_B=0.016$

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