The given question is incomplete. The complete question is:
A 3.9 L volume of ideal neon gas (monatomic) is at a pressureof 5.6 atmospheres and a temperature of 330 K. The atomic mass of neon is 20.2g/mol. In this situation, the temperature of the gas is increased to 430 and the volume is increased to 5.9L. What is the final pressure of the gas?
Answer: The final pressure of the gas is 4.8 atm
Explanation:
Combined gas law is the combination of Boyle's law, Charles's law and Gay-Lussac's law.
The combined gas equation is,
[tex]\frac{P_1V_1}{T_1}=\frac{P_2V_2}{T_2}[/tex]
where,
[tex]P_1[/tex] = initial pressure of gas = 5.6 atm
[tex]P_2[/tex] = final pressure of gas = ?
[tex]V_1[/tex] = initial volume of gas = 3.9 L
[tex]V_2[/tex] = final volume of gas = 5.9 L
[tex]T_1[/tex] = initial temperature of gas = 330 K
[tex]T_2[/tex] = final temperature of gas = 430 K
Now put all the given values in the above equation, we get:
[tex]\frac{5.6\times 3.9}{330}=\frac{P_2\times 5.9}{430}[/tex]
[tex]P_2=4.8atm[/tex]
The final pressure of the gas is 4.8 atm