Question

The chlorination of methane occurs in a number of steps that results in the formation of chloromethane and hydrogen chloride. The overall reaction is

2CH4(g)+3Cl2(g)⟶2CH3Cl(g)+2HCl(g)+2Cl−(g)

Suppose that a chemist combines 283 mL of methane and 701 mL of chlorine at STP in a 2.00 L flask. The flask is then allowed to stand at 298 K. If the reaction reaches 66.6% completion, what is the total pressure in the flask?

total=
atm
What is the partial pressure of CH4?
CH4=
atm
What is the partial pressure of Cl2?
Cl2=
atm
What is the partial pressure of CH3Cl?
CH3Cl=
atm
What is the partial pressure of HCl?
HCl=
atm
What is the partial pressure of Cl−?
Cl−=
atm

PLEASE HELP NEED STEP BY STEP SIMPLE EXPLANATION!!!! :(

Answer 1

Explanation:

The chlorination of methane occurs in a number of steps that results in the formation of chloromethane and hydrogen chloride. The overall reaction is : 2CH4(g)+3Cl2(g)⟶2CH3Cl(g)+2HCl(g)+2Cl−(g) Suppose that a chemist combines 295 mL of methane and 725 mL of chlorine at STP in a 2.00 L flask

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