One mole of neon, a monatomic gas, starts out at conditions of standard temperature and pressure. The gas is h?
One mole of neon, a monatomic gas, starts out at conditions of standard temperature and pressure. The gas is heated at constant volume until its pressure is tripled, then further heated at constant pressure until its volume is doubled. Assume that neon behaves as an ideal gas. For the entire process, find the heat added to the gas.
So confused- any help explaining this would be great!
- Peter HLv 78 years agoFavorite Answer
First, revise the ideal gas equation in the form P1V1/T1 = P2V2/T2 where the temperatures T1, T2 are in Kelvins rather than degrees C. Second, make sure you know what standard temperature and pressure is. Finally, you need to know the specific heat of neon. This is usually quoted as calories/g for a 1 degree C rise, but you have a mole of gas here, so you also need to know the molecular weight of neon (= atomic weight, since neon is monatomic).
Then calculate the temperature rise for each manoeuvre, and, from the specific heat, calculate the heat added in each case. Good luck.
- baltripLv 44 years ago
it is completely in conformance with Avagadro. For any gases, as long as they are all on the comparable situations of temperature and tension, mols could be examine as volumes. it is real under all equivalent situations, no longer in basic terms at STP. occasion:( it is in basic terms theoretical, that the reaction is going to of completion, which it would not.) N2+ 3H2 ? 2NH3 you are able to examine this as: 1mol of nitrogen will react with 3mol of hydrogen to offer 2 mol ammonia. or you are able to the two wisely say: 1volume of nitrogen reacts with 3 volumes of nitrogen to offer 2 volumes of ammonia. tension and temperature are irrelevant, as long as all 3 gases are on the comparable situations.
- 7 years ago
2.38e4 is what you are looking for
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- Anonymous7 years ago
How did you do that??