Two containers contain the same gas at different temperatures and pressures, as

Question

Two containers contain the same gas at different temperatures and pressures, as indicated in the figure. The small container has a volume of 2 L, and the large container has a volume of 4 L. The two containers are then connected to each other using a thin tube, and the pressure and temperature in both containers are allowed to equalize. If the final temperature is 394 K, what is the final pressure? Assume that the connecting tube has negligible volume and mass

Explanation / Answer

let V be the final volume,P be the final pressure ,T be the final temperature of gas after two containers are connected . V= volume of container 1 +volume of container 2 = 4+2=6L it is Given that T=394 K let n1 be number of moles of gas in container1 and n2 be number of moles of gas in container1 applying ideal gas equation(PV=nRT) container1 we get (3*10^5)*(4)=n1*R*600 =>n1=2*10^3/R applying ideal gas equation(PV=nRT) container we get (2*10^5)*(2)=n1*R*200 =>n2=2*10^3/R applying ideal gas eq for final conditions we get P*V=(n1+n2)*R*T =>P=(4*10^3/R)*R*394/6 =2.62*10^5 Pa therefore final pressure is 2.62*10^5 Pa

Related Questions

Navigate

• Browse (All)
• Browse T
• Subjects

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.