A gas has a volume of 6.00 liters at a temperature of 27° C and a pressure of 1,00 atm. What is the volume of the gas, in liters, at a temperature of 327°C and a pressure of 3.00 atm?

We are given:

P1 = 1 atm                 P2 = 3 atm

T1 = 300 K               T2 = 600 K

V1 = 6 L                    V2 = v L

Finding the final Volume:

From the ideal gas equation:

PV = nRT

since in the given scenario, the universal gas constant (R) and number of moles(n) are constant

So, for both the cases, the value of n*R will be a constant k

Hence, we can write that:

PV / T = k        [where k is a constant]

Since the constant 'k' is the same for both the cases, we can write that:

P1V1 / T1 = P2V2 / T2

replacing the variables

1 * 6 / 300 = 3 * v / 600

1/50 = v / 200

v = 200/50

v = 4 L

Therefore, the volume of the gas at 600K and 3 atm will have a volume of 4 L

i think it is true since you can test the answer and can use observations to complete it.