Chemistry alevel homework help.
I dont get this question.
Use the ideal gas equation of state to answer this question. In SI units, the equation is pV=nRT, where R=8.31JK ^−1 mol ^−1
When 2.0moles of a gas mixture at 1atm and 296K is compressed to half its original volume, the temperature rises to 312K and the pressure rises to 1.7atm. Some of the gas slowly leaks out during compression.
Calculate the amount of gas present in the smaller volume.
Use the ideal gas equation of state to answer this question. In SI units, the equation is pV=nRT, where R=8.31JK ^−1 mol ^−1
When 2.0moles of a gas mixture at 1atm and 296K is compressed to half its original volume, the temperature rises to 312K and the pressure rises to 1.7atm. Some of the gas slowly leaks out during compression.
Calculate the amount of gas present in the smaller volume.
Original post by dont_get_things
I dont get this question.
Use the ideal gas equation of state to answer this question. In SI units, the equation is pV=nRT, where R=8.31JK ^−1 mol ^−1
When 2.0moles of a gas mixture at 1atm and 296K is compressed to half its original volume, the temperature rises to 312K and the pressure rises to 1.7atm. Some of the gas slowly leaks out during compression.
Calculate the amount of gas present in the smaller volume.
Use the ideal gas equation of state to answer this question. In SI units, the equation is pV=nRT, where R=8.31JK ^−1 mol ^−1
When 2.0moles of a gas mixture at 1atm and 296K is compressed to half its original volume, the temperature rises to 312K and the pressure rises to 1.7atm. Some of the gas slowly leaks out during compression.
Calculate the amount of gas present in the smaller volume.
Forget my initial instructions, I misread.
Start by calculating the volume of gas when 2.0 mol are stored at 296 K under 1 atm of pressure (you can assume 1 atm is about 101 kPa of pressure)
(edited 5 months ago)
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