A8.5-liter sample of a gas at 2.0 atm and 300.0 k has 1.2 moles of the gas. if 0.65 mole of the gas is added to the sample at the same temperature and pressure, what is the final volume of the gas?

13 liters
14 liters
18 liters
21 liters

13 liters

Explanation:

Avogadro's Law: This law states that volume is directly proportional to the number of moles of the gas at constant pressure and temperature.

  (At constant temperature and pressure)

where,

= initial volume of gas = 8.5 L

= final volume of gas = ?

= initial moles of gas =  1.2 moles

= final moles of gas = 1.2 +0.65 = 1.85 moles

Now put all the given values in the above equation, we get the final pressure of gas.

Therefore, the final volume of the gas will be 13 Liters.

the ideal gas law equation is as follows

pv = nrt

where p - pressure

v - volume

n - number of moles

r - universal gas constant

t - temperature

so if the pressure, volume and temperature are already known

we are left with n and r

since r is the universal gas constant that has a known fixed value then r too is known

so we are left with 'n'

once we know temperature volume and pressure

we can find the number of moles of gas present using the ideal gas law equation

this is not my own answer, this is an answer for the same question by the user blahblahmali. i do not claim ownership of this account.