Respuesta :
Explanation:
The given data is as follows.
50 ml of [tex]Cl_{2}[/tex], 50 ml of [tex]C_{2}H_{4}[/tex]
And, it is known that at STP 1 mole of a gas occupies 22.4 L. Hence, moles present in 50 ml of gas are as follows.
[tex]\frac{50}{22.4 \times 1000}[/tex] (As 1 L = 1000 ml)
= [tex]2.23 \times 10^{-3}[/tex] moles
So, according to the given equation [tex]2.23 \times 10^{-3}[/tex] moles of [tex]Cl_{2}[/tex] reacts with [tex]2.23 \times 10^{-3}[/tex] moles of [tex]C_{2}H_{4}[/tex].
Hence, moles of [tex]C_{2}H_{4}Cl_{2}[/tex] is equal to the moles of [tex]C_{2}H_{4}[/tex] and [tex]Cl_{2}[/tex].
Therefore, moles of [tex]C_{2}H_{4}Cl_{2}[/tex] = [tex]2.23 \times 10^{-3}[/tex] moles
1 mole of [tex]C_{2}H_{4}Cl_{2}[/tex] = 22.4 L
[tex]2.23 \times 10^{-3}[/tex] moles = [tex]22.4 \times 2.23 \times 10^{-3} moles[/tex]
= 50 ml of product
Thus, we can conclude that 50 ml of products if pressure and temperature are kept constant.
