Q:Under which conditions of temperature and pressure would a sample of H2(g) behave most like an ideal gas?
554328
Munir is right.  H2 will behave most like an ideal gas in a condition with Highest temperature and lowest pressure, making your Choice 3.
963461
Assuming both gasses are ideal, and the mixture is ideal, we know from Dalton's Law P1+P2=Ptotal.  We can find the individual pressures by P1V1=n1RT1 and P2V2=n2RT2.  Since the two gases are in the same volume at the same temperature we can combine the above equations  to get P2/P1=n2/n1 this P1=Ptotal*n1/(n1+n2)\n\nMoles of H2 = 7.20g * 1mole/2.016g= 3.57 moles H2\nMoles of Kr = 10.3g * 1mole/83.80g= 0.123 moles Kr\n\nSo the partial pressure of H2 is 0.585 atm.  Sorry for skipping some steps above, its just ratios but I don't have much time.
525073
An isobar shows regions of similar air pressure.\n\nAn isotherm shows regions of similar temperature.
631965
generally gases react differently in changing pressure, they react faster in high pressure and is inhibited by low pressure. the most reactive gas due to pressure and everything elese is FLUORINE (F2), coz its the most electronegative diatomic gas molecule and has smallest bond distance.
743246
Not sure I understand what you are asking.\nYou can choose to specify either temperature or pressue at the saturation point, but not both.\n\nIf the refrigerant is boiling, that's a 2-phase solution. The mixture will range from all liquid to all gas without a change in pressure or temperature. It will be saturated vapor by definition.\n\nFor common refrigerants it is probably simpler to look up the information - it should be published or at least available from the manufacturer.
1153522
The quantities you have listed are in fact related via the ideal gas law.  So, assuming you aren't in huge temperature or pressure extremes, you can use the ideal gas law with decent results.\n\nIdeal Gas Law\nPV = nRT\n\nwhere P = pressure (N/m^2)\nV = volume (m^3)\nn = number of moles of gas\nR = universal gas constant = 8.3145 J/(mol*K)\nT = temp (in Kelvins)\n\nSo, by looking at the equation you can not convert air pressure directly to volume without also knowing the temperature and number of moles of gas.
826041
The answer to your question would depend on (1) whether "empty" means a "perfect vacuum" or filled with air? (2) how is this 1 joule of energy initially distributed inside this box? (3) how large is this box? (4) how much time is allowed to elapse before the termperature is determined? (5) can energy leak out or into the box? (6) is the box under the influence of a gravitational field?\n\nThe temperature of an object is proportional to the average kinetic energy of the molecules in it. In a pure vacuum, there are no molecules. There is nothing to measure the kinetic energy of, and temperature is undefined. If a thermometer were placed in a vacuum, the reading would be a measurement of the internal temperature of the thermometer, not of the vacuum which surrounds it. So having 1 joule of energy inside a box containing pure vacuum would have NO temperature. And if it contained air, then we would need to know the initial temperature, pressure of the air inside the box and also the volume of the box. Then we can approximate the air as an ideal gas and use the following equation to compute the temperature:\n\nPV=nRT\n\nwhere T is the temperature, n is the number of moles of gas and R is the gas constant. Since we know the initial temperture and pressure, and the volume of the box. Then\n\nP(i)V(i)/T(i) = P(f)V(f)/T(f)\n\nT(f) = T(i) [P(f)/P(i)]\n\nSince pressure is dfined as P = F/A (force per unit area) and\n\nE = Fd (force times distance), then\n\nP = E/Ad, where Ad = V volume of the box (here we are assuming that the 1 joule of energy is uniformly distributed inside the box and the volume of the box does not change)\n\nHence, T(f) = T(i) [E/P(i)V(i)]
474897
This is going to depend on a lot of different things. Barometric pressure, atmospheric conditions, relative humidity, altitude, amount of fuel, fuel pressure...all these things come in to effect when looking for the "exact" temperature. However, i think on average its somewhere between 700-750F.
544724
are you talking about the ideal gas law? if so...\n\nThe ideal gas law is the equation of state of an ideal gas. The state of an amount of gas is determined by its pressure, volume, and temperature. The equation has the form\n\n    pV = nRT\n\nwhere\n\n    p:is the pressure (kPa),\n    V:is the volume (L),\n    n:is the number of moles of gas (mol),\n    R:is the gas constant, and\n    T:is the temperature (K).\n\nR is commonly approximated to 8.31 J·K-1·mol-1 when using Pa for pressure. However this can vary if using a different unit for pressure (see gas constant).\n\nso...\nV=nRT/p\nn=pV/RT\n\n\n\nor do you need density?\n\nDensity=Mass/Volume\n\n\n\nor\n\nVolume=length*width*height
12892
well, all plasma is is gas when all of the atoms are ionized, so it's not like something special happens, so nothing can really happen after it.  I mean, at a substance's coldest, the particles have no movement, and it's solid, then as temperatures increase they get more movement and can slide around each other, becoming liquid, and finally when it gets hot enough, the particles are moving so fast that they separate from each other and fly every which way, which is a gas.  No matter how hot it gets, the particles are still going to be seperate, and will just move faster and faster, still being a gas.  Plasma isn't even just solely a result of temperature, other conditions have to occur as well, and all of the atoms are ionized (meaning that they have complete electron shells and they do this by losing or gaining electrons. They are most stable when they have completely filled orbitals.)  Now you have a bunch of very fast ionized particles. Nothing more can really happen to them... hmmm, wait, actually, unless protons start shooting out and they become other elements... Who knows what happens at such extreme temperatures? Well with larger radioactive elements, there is decay that goes on over time converting one element into another, so maybe that would be influenced by temperature and pressure.  well there still wouldn't be another state of matter, it would just be different elements at either gas or plasma state.
917314
A real gas is a form of matter that will conform to the sides of its container.  As it is compressed its temperature increases.  It is the only form of matter than can be compressed at all.  Gas is the least organized form of matter.
499971
When gas is compressed in a thermally insulated vessel the gas is heated.\n\nWhen pressure increases temperature increases.\n\nSimilarly if the gas is expanded in a thermally insulated vessel the gas is cooled.\n\nWhen the pressure decreases the temperature decreases. \n\nNear earth’s surface, the atmospheric pressure is very high.\n\nAt a height of 30km from the surface, the pressure of air is almost zero.\n\nThough the hot air goes up; as it goes up the pressure decreases and volume increases (density decreases) and as per the  gas equation the temperature decreases.
649470
If you consider "pressure" as the force of molecules striking the surface and the molecules are randomly moving about, then they will strike all surfaces equally.  Since gas molecules are very free in their motion, they quickly react to equilize any changes in the system.  So if temperature rises, the molecules move faster, strike the walls harder and pressure rises.
879693
An ideal gas\n\nAn ideal gas or perfect gas is a hypothetical gas consisting of identical particles of zero volume, with no intermolecular forces. Additionally, the constituent atoms or molecules undergo perfectly elastic collisions with the walls of the container. Real gases do not exhibit these exact properties, although the approximation is often good enough to describe real gases. The approximation breaks down at high pressures and low temperatures, where the intermolecular forces play a greater role in determining the properties of the gas. There are basically three types of ideal gas:\n\n    * the classical or Maxwell-Boltzmann ideal gas,\n    * the ideal quantum Bose gas, composed of bosons, and\n    * the ideal quantum Fermi gas, composed of fermions.\n\nThe classical ideal gas can be separated into two types: The classical thermodynamic ideal gas and the ideal quantum Boltzmann gas. Both are essentially the same, except that the classical thermodyamic ideal gas is based on classical thermodynamics alone, and certain thermodynamic parameters such as the entropy are only specified to within an undetermined additive constant. The ideal quantum Boltzmann gas overcomes this limitation by taking the limit of the quantum Bose gas and quantum Fermi gas in the limit of high temperature to specify these additive constants. The behavior of a quantum Boltzmann gas is the same as that of a classical ideal gas except for the specification of these constants. The results of the quantum Boltzmann gas are used in a number of cases including the Sackur-Tetrode equation for the entropy of an ideal gas and the Saha ionization equation for a weakly ionized plasma.\n\nreal gas \n\nA gas is one of the four major phases of matter (after solid and liquid, and followed by plasma, that subsequently appear as a solid material is subjected to increasingly higher temperatures. Thus, as energy in the form of heat is added, a solid (e.g., ice) will first melt to become a liquid (e.g., water), which will then boil or evaporate to become a gas (e.g., water vapor). In some circumstances, a solid (e.g., "dry ice") can directly turn into a gas: this is called sublimation. If the gas is further heated, its atoms or molecules can become (wholly or partially) ionized, turning the gas into a plasma.
167746
At STP, 1 mole of any ideal gas will have a volume of 22.4 Liters.\nUsing this logic, we can deduce that at STP, and equal volumes of (what we will assume are ideal gasses) gasses will each contain the same number of moles.\nIf each flask contains the same number of moles, then they much each contain the same number of molecules.\n\nBy saying that the flasks are at STP, we are given all the information we need to solve this.  STP (Standard temperature and pressure) implies a temperature of 273 K and a pressure of 1 atm.
397453
number 4 is partially right. By Gay Lussac's Gas Law, pressure DOES affect temperature directly - more pressure, more temp.
730643
All gases are compressible to some degree. This is part of the definition of a gas.\n\nFor some practical problems, the compressibility of the gas can be neglected and sufficiently accurate results are still obtained. This is the case when the changes in pressure and temperature are relatively small, such that the density of the gas does not change by more than a few percent.\n\nThis situation is usually encountered in low-speed gas flows at atmospheric pressure. Two examples would be HVAC, and wind tunnel studies at < 0.1 Mach.