Question

A glass container was initially charged with 1.70 moles of a gas sample at 4.00 atm and 21.7 °C. Some of the gas was released as the temperature was increased to 29.1 °C, so the final pressure in the container was reduced to 1.05 atm. How many moles of the gas sample are present at the end?

Answer 1

Answer: 0.435

Step-by-step explanation:

Using the ideal gas law,

`4.00V=(1.70)(0.821)(21.7+273)\\\\V=102.828 \text{ L}`

After the temperature was increased,

`1.05(102.828)=n(0.821)(29.1+273)\\\\n=0.435 \text{ moles}`