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.

Explanation:

The given data is as follows.

      50 ml of ,       50 ml of

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.

               (As 1 L = 1000 ml)

          = moles

So, according to the given equation moles of reacts with moles of .

Hence, moles of is equal to the moles of and .

Therefore, moles of = moles

           1 mole of = 22.4 L

    moles =        

                                = 50 ml of product

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

your answer would be “dry”

it's all four options.