Question

If pressure and temperature are kept constant, the reaction of 38 mL of Cl2 gas with 22 mL of CH4 gas via the equation: Cl2 (g) + CH4 (g) →HCl (g) + CH3Cl (g) will produce a total of ________ mL of products

Answer 1

Answer:

There is a total of 60 mL of products produced

Explanation:

Step 1: Data given

8 mL of Cl2 gas with 22 mL of CH4

Pressure and temperature are kept constant

Step 2: The balanced equation

Cl2 (g) + CH4 (g) →HCl (g) + CH3Cl (g)

Step 3: Calculate the volume of the products

The ideal gas law is  PV = nRT

Since the pressure and temperature are kept constant, and R is a constant.

V is directly proportional to n

the ratio of moles in an equation is proportional to the number of liters  of gases

1 mol of Cl2 (g) + 1 mole of CH4 (g) ----------- 1 mole of HCl (g) + 1 mole of CH3Cl (g)

since n is directly proportional to V

1 litre of Cl2 (g) + 1  litre of CH4 (g) ----------- 1  litre of HCl (g) + 1  litre of CH3Cl (g)

V1n1 = V2n2

⇒ with V1 = the volume of the reactants = 22 + 38 = 60 mL

⇒ with n1 = the number of moles of reactants = 1+1 = 2 moles

⇒ with V2 = the volume of products = TO BE DETERMINED

⇒ with n2 = the number of moles of products = 1+1 = 2

60 mL * 2 = V2 * 2

V2 = 60 mL

This means :

38 mL + 22 mL produces a total of 60 mL of products