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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.

1 Answer

1 vote

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.

User Hellopat
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