If 375 grams of CO2 are placed in a vessel whose volume is 34.5 liters at a temperature of 20 degrees celsius, what will the pressure be? PLEASE, ANYONE HELP!

the pressure is P = 5,94 atm ≈ 6 atm

Explanation:

Following the equation corresponding to the Ideal Gas Law, it is possible to find the system pressure in the silver problem.

From this equation, we find the pressure

where:

P is the pressure of the gas,

V is the volume of the gas,

n is the amount of substance of gas (also known as number of moles),

R is the ideal, or universal, gas constant.

Now we find the moles of CO2

We have 375g of CO2 and its molecular weight is 44g/mol

Using.

R = 0,082

T = 20ºC = 293,15 K

We substitute in the equation

P = 5,94 atm ≈ 6 atm

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