A gas is originally contained within a container of volume 100 m3 and is held at

Question

A gas is originally contained within a container of volume 100 m3 and is held at a pressure of 1 ATM and temperature 15°C. Due to equipment failure, the temperature rises to 66°C, but safety systems do not allow the pressure to exceed 1.1 atmospheres. During the repair, it is noticed that the safety systems have vented gas into the air to maintain the pressure at a safe level. Part

A How many moles of gas were originally contained?

Part B How much gas has been lost into the atmosphere during this process? Give your answer to two significant figures.

Explanation / Answer

Given that

The volume of the gas contained in the container is (V) =100m3

The pressure is (P) =1atm

The initial temperature is (T1) =15degrees =288K

The temperature increased to (T2) =339K

Now from the ideal gas law

PV=nRT

For the first part of the question is

1(100)=nR(288K)

For the second part, that is increase in temperature and pressure

1.1(100) =n'R(339)

From the above equations we get

1/1.1 =n/n'(288/339) =0.849(n/n')

0.909 =0.849(n/n')

n' =0.934n

Then the number of moles left is 93.4%

or the original moles left to the atmosphere is 100-93.4 =6.6%

Related Questions

Navigate

• Browse (All)
• Browse A
• Subjects

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