Question

A gas cylinder contains 2.0 mol of gas X and 6.0 mol of gas Y at a total pressure of 2.1 atm. What is the partial pressure of gas Y? Use StartFraction P subscript A over P subscript T EndFraction equals StartFraction n subscript a over n subscript T EndFraction..

Answer 1

Answer :  The partial pressure of X and Y gases are, 0.525 and 1.575 atm respectively.

Explanation : Given,

Moles of X = 2.0 mole

Moles of Y = 6.0 mole

Total pressure = 2.1 atm

Now we have to calculate the mole fraction of X and Y.

$\text{Mole fraction of }X=\frac{\text{Moles of }X}{\text{Moles of }X+\text{Moles of }Y}$

$\text{Mole fraction of }X=\frac{2.0}{2.0+6.0}=0.25$

and,

$\text{Mole fraction of }Y=\frac{\text{Moles of }Y}{\text{Moles of }X+\text{Moles of }Y}$

$\text{Mole fraction of }Y=\frac{6.0}{2.0+6.0}=0.75$

Now we have to calculate the partial pressure of X and Y.

According to the Raoult's law,

$p_i=X_i\times p_T$

where,

$p_i$ = partial pressure of gas

$p_T$ = total pressure of gas  = 2.1 atm

$X_i$ = mole fraction of gas

$p_{X}=X_{(X)}\times p_T$

$p_{X}=0.25\times 2.1atm=0.525atm$

and,

$p_{Y}=X_{(Y)}\times p_T$

$p_{Y}=0.75\times 2.1atm=1.575atm$

Thus, the partial pressure of X and Y gases are, 0.525 and 1.575 atm respectively.

Answer 2

Answer:

1.6 is the answer

Explanation: