Question

The reaction of 50 mL of Cl2 gas with 50 mL of C2H4 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

Answer:

50 mL

Explanation:

According to Avogadro's law, the volume of an ideal gas is proportional to the number of moles. Then, if we have 50 mL of Cl₂ and 50 mL of C₂H₄, we can affirm that we have the same number of moles of both.

The balanced equation is:

Cl₂(g) + C₂H₄(g) → C₂H₄Cl₂(g)

The molar ratio Cl₂:C₂H₄:C₂H₄Cl₂ is 1:1:1. Then, when x moles of Cl₂ react with x moles of C₂H₄, they produce x moles of C₂H₄Cl₂. Assuming pressure and temperature are kept constant, the volume corresponding to x moles is 50 mL.

Answer 2

Answer:

There will be produced a total of 50 mL of products (C2H4Cl2)

Explanation:

Step 1: Data given

Volume of Cl2 = 50 mL

Volume of C2H4 = 50 mL

Step 2: The balanced equation:

Cl2(g) + C2H4(g) → C2H4Cl2(g)

For 1 mol of Cl2 we need 1 mole of C2H4 to produce 1 mole of C2H4Cl2

Step 3: Calculate volume of C2H4Cl2

Since pressure, temperature are kept cosntant, we can calculate the final volume as following:

(5There will be produced a total of 50 mL of products (C2H4Cl2)0 mL Cl2) * (1 mol C2H4Cl2 / 1 mol Cl2) = 50 mL C2H4Cl2