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

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.

          $\frac{50}{22.4 \times 1000}$      (As 1 L = 1000 ml)

          = $2.23 \times 10^{-3}$ moles

So, according to the given equation $2.23 \times 10^{-3}$ moles of $Cl_{2}$ reacts with $2.23 \times 10^{-3}$ 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 $C_{2}H_{4}Cl_{2}$ = $2.23 \times 10^{-3}$ moles

           1 mole of $C_{2}H_{4}Cl_{2}$ = 22.4 L

   $2.23 \times 10^{-3}$ moles = $22.4 \times 2.23 \times 10^{-3} moles$        

                                = 50 ml of product

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