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

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

< > according to newton's third law of motion, forces always act in equal but opposite pairs. another way of saying this is for every action, there is an equal but opposite reaction.< >

b. is the answer hoped i