Chemistry help

Question

In the fermentation of glucose (wine making), 710 mL of CO2 gas was produced at 35 ∘C and 1.00 atm .

What is the final volume, in liters, of the gas when measured at 20 ∘C and 675 mmHg , when n is constant?

Can't figure out. Please help, thanks!

Answer 1

In this problem, you have a change in temperature, and pressure but moles is constant. And you are asked to find the new volume.  So, using the combined gas law you can determine this.

P₁V₁/T₁ = P₂V₂/T₂

P₁ = 1.00 atm

V₁ =710 ml = 0.710 L

T₁ = 35ºC = 308K

P₂ = 675 mm Hg x1 atm/760 mm Hg = 0.888 atm

V₂ = ?

T₂ = 20ºC = 293K

Using P₁V₁/T₁ = P₂V₂/T₂ and solving for V₂ we have

V₂ = P₁V₁T₂/P₂T₁ = (1.00)(0.710)(293)/(0.888)(308)

V₂ = 0.761 liters

PS.  You may want to check my math as I am half asleep, but this is the general approach.