The pressure of a gas in a container is 1.85 atm and occupies a volume of 12.5 l. if the original volume is reduced by half at constant temperature, what would happen to the pressure?

3.7 atm i.e., pressure doubles

Explanation:

P₁ = Initial pressure = 1.85 atm

P₂ = Final pressure

V₁ = Initial volume = 12.5 L

V₂ = Final volume = 0.5V₁

T = Temperature is constant

From ideal gas law

P₁V₁ = P₂V₂

∴ Final pressure is 3.7 atm i.e., pressure doubles

- measure reactants precisely. ( first choice)

- stir to the reaction take place. ( second choice)

- wait patiently until the reaction completes. ( fourth choice)

- make sure to recover as much copper as possible. ( last choice)

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