Respuesta :
Explanation:
The given reaction equation is as follows.
[tex]C_{2}H_{2}(g) + 2H_{2}(g) \rightarrow C_{2}H_{6}(g)[/tex]
Let us assume that the partial pressure of [tex]C_{2}H_{2}[/tex] be 'x' atm. Hence, the partial pressure of [tex]H_{2}[/tex] = (0.1 - x) atm
And, amount of [tex]H_{2}[/tex] left unreacted is as follows.
[tex](0.1 - x) - 2 \times x[/tex] = 0.1 - 3x
Now, the pressure of [tex]C_{2}H_{6}[/tex] = partial pressure of reacted [tex]C_{2}H_{2}[/tex] = x
So, the pressure of product will be as follows.
Pressure of the product = partial pressure of [tex]C_{2}H_{6}[/tex] + partial pressure of unreacted [tex]H_{2}[/tex]
0.042 = x + (0.1 - 3x)
2x = 0.058
or, x = 0.029 atm
Therefore, mole fraction of [tex]C_{2}H_{2}[/tex] = partial pressure of [tex]\frac{C_{2}H_{2}}{\text{Total pressure of the gas mixture}}[/tex]
= [tex]\frac{0.029}{0.1}[/tex]
= 0.29
Thus, we can conclude that the mole fraction of acetylene in the original mixture is 0.29.
