Question

the reaction of 50 mL of gas with 50 mL of gas via the equation: Cl2(g) + C2H4(g) ➔ C2H4Cl2 (g) will produce a total of __________ mL of products if pressure and temperature are kept constant.

Answer 1

Step-by-step explanation:

The given data is as follows.

50 ml of
`Cl_(2)`, 50 ml of
`C_(2)H_(4)`

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.

`(50)/(22.4 * 1000)` (As 1 L = 1000 ml)

=
`2.23 * 10^(-3)` moles

So, according to the given equation
`2.23 * 10^(-3)` moles of
`Cl_(2)` reacts with
`2.23 * 10^(-3)` moles of
`C_(2)H_(4)`.

Hence, moles of
`C_(2)H_(4)Cl_(2)` is equal to the moles of
`C_(2)H_(4)` and
`Cl_(2)`.

Therefore, moles of
`C_(2)H_(4)Cl_(2)` =
`2.23 * 10^(-3)` moles

1 mole of
`C_(2)H_(4)Cl_(2)` = 22.4 L

`2.23 * 10^(-3)` moles =
`22.4 * 2.23 * 10^(-3) moles`

= 50 ml of product

Thus, we can conclude that 50 ml of products if pressure and temperature are kept constant.