For this you would use Boyle's Law, P1V1 = P2V2. The first pressure and volume variables are before the change, while the second set are after the change. In this case, the volume is being changed and the pressure has to be solved for.
P1 = 1.30 ATM
V1 = 31.4 L
P2 = Unknown
V2 = 15.0 L
P1V1 = P2V2
1.30(31.4)=15.0P
P= 2.72 ATM
Looking at the question simply, you can get an estimate on the pressure because you can see that pressure and volume vary indirectly (if volume goes up, pressure goes down). If the volume is cut in half (roughly), then the pressure should increase by half.
You can use the Ideal Gas law which says that for an ideal gas the pressure times the volume divided by the temperature must be a constant number. And in this case since you are given that the temperature is a constant number then the gas law becomes "the pressue times the volume is a constant number". This means whatever their product is at one time , it will equal their product at a different time. The equation would be: Pf x Vf = Pi x Vi where the i & f mean initial & final. You solve this for the unknown final pressure ,Pf as: Pf = ( Pi x Vi )/Vf = ( 655 x 10 )/1.5 = 4367 mm of Hg
Equa; amounts of all gasses have the same volume at the same conditions
Egg Sucked into Bottle (Heating Variation)The variable is the temperature of the air inside the bottle, which determines its pressure and volume. When air is heated, it has higher pressure or takes up more volume. When cooled, it becomes more dense and takes up less space. With less volume in the bottle, the only way for the pressure to equalize is by pushing the egg in.Part 1: We were heating an open system "the flask." Temperature and moles were changing. Pressure and volume are being held constant. As the open system is being heated the particles speed up, have limited space to move and moles leave the flask.Part 2: We took the flask off the heater, set it on the counter and put the egg on top. Pressure and temperature are changing. Volume and moles are being held constant. When the egg was put on the flask the temperature decreased causing the molecules to slow down. This decreased the inside pressure of the flask causing the atmospheric pressure to suck the egg into the flask because it was trying to balance with the inside pressure.Egg Sucked into Bottle (Combustion Variation)There is a finite amount of gas in the bottle, nitrogen and oxygen. When combustion occurs (a burning piece of paper), the oxygen in the air combines to form solid oxides and carbon dioxide, both of which occupy less space than the initial free oxygen. Less oxygen in the bottle means lower pressure, and again the outside pressure can force the egg into the bottle.
No, you do not need to define a problem. The steps of the scientific method are: 1. Having a Question For example, "Does water boil at different temperatures depending on air pressure?" 2. Coming up with a Hypothesis A hypothesis is your best guess as to the answer of the question. In this example, it could be, "Water will boil at a lower temperature if air pressure is lower." 3. Performing an Experiment In this case, you would try testing the temperature of boiling water at two different air pressure levels, and record your observations. 4. The Conclusion This is when you determine whether your hypothesis is correct or incorrect. In this case, your hypothesis would have been correct. Water does boil at a lower temperature when air pressure is lower. Answer 2 Interesting question here are some initial thoughts. If you think of a typical scientific observation like at what temperature does water boil, and then note that this varies depending on how much atmospheric pressure is on it, what constitutes a problem? The problem might be how to measure it or to understand the mechanism whereby the pressure affects the temperature. But strictly speaking there are no problems as such, a problem is constituted in relationship to a desired outcome. So I have a problem only if I want something. Nothing in the inanimate world wants anything, so a scientific problem is artificial. I desire a solution to understanding some physical process therefore I observe it measure it and study it and the process of studying it will throw up problems.
The amount of heat required to increase the temperature of the substance to 1 degree greater than that of the initial temperature of the body!
If pressure is held constant, volume and temperature are directly proportional. That is, as long as pressure is constant, if volume goes up so does temperature, if temperature goes down so does volume. This follows the model V1/T1=V2/T2, with V1 as initial volume, T1 as initial temperature, V2 as final volume, and T2 as final temperature.
You can calculate pressure and temperature for a constant volume process using the combined gas law.
BOYLES LAW The relationship between volume and pressure. Remember that the law assumes the temperature to be constant. or V1 = original volume V2 = new volume P1 = original pressure P2 = new pressure CHARLES LAW The relationship between temperature and volume. Remember that the law assumes that the pressure remains constant. V1 = original volume T1 = original absolute temperature V2 = new volume T2 = new absolute temperature P1 = Initial Pressure V1= Initial Volume T1= Initial Temperature P2= Final Pressure V2= Final Volume T2= Final Temperature IDEAL GAS LAW P1 = Initial Pressure V1= Initial Volume T1= Initial Temperature P2= Final Pressure V2= Final Volume T2= Final Temperature Answer BOYLES LAW The relationship between volume and pressure. Remember that the law assumes the temperature to be constant. or V1 = original volume V2 = new volume P1 = original pressure P2 = new pressure CHARLES LAW The relationship between temperature and volume. Remember that the law assumes that the pressure remains constant. V1 = original volume T1 = original absolute temperature V2 = new volume T2 = new absolute temperature P1 = Initial Pressure V1= Initial Volume T1= Initial Temperature P2= Final Pressure V2= Final Volume T2= Final Temperature IDEAL GAS LAW P1 = Initial Pressure V1= Initial Volume T1= Initial Temperature P2= Final Pressure V2= Final Volume T2= Final Temperature
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When air is compressed at the same temperate and volume space, pressure will increase in accordance with Boyle's Law which states: PV/T (initial) = PV/T (final) where P is pressure, V is volume and T is temperature.
The initial pressure is halved. Use Boyle's law that relates pressure & volume at a constant temperature. P1V1 = P2V2 In this case the V1(initial volume) is doubled so V2 = 2V1 P2 = P1V1/V2 = P1V1/2V1 P2 = (1/2)*P1
This cannot be answered without an initial volume or pressure. But the final pressure of an expansion of a gas can be determined by the following formula. PV/T = P'V'/T' where P = pressure absolute V = volume T = temperature absolute ( ' ) indicates the new pressure, volume and temperature because the temperature is constant this can be reduced to PV = P'V' or P' = PV/V'
Pressure is halved when ONLY volume is doubled (n and T are constant).Remember the General Gas Law:p.V = n.R.T(in which R=general gas constant)
P V = k T, so at constant temperature, PV is constant Initial PV = (102.5 x 3.67) = 376.175 ====> At constant temp, V = (376.175 / P) Final P = 100.9. Final V = (376.175 / 100.9) = 3.7282 L (rounded)
500. mmHg
Assuming the amount of gas remains constant, we can use the ideal gas law to calculate the final absolute pressure. The initial pressure (P1) is 200 kPa and the final volume (V2) is 250 cm3. The initial temperature (T1) is 40 degrees Celsius or 313.15 Kelvin, and the final temperature (T2) is 20 degrees Celsius or 293.15 Kelvin. Using the equation (P1 * V1) / T1 = (P2 * V2) / T2, we can solve for the final absolute pressure (P2), which is approximately 400 kPa.
Assuming a fixed amount of an ideal gas kept at constant temperature, then the volume is reduced to a third of its former amount when the pressure is tripled. P V = n R T = constant = k P1 V1 = k = P2 V2 P2 = 3 P1 3 P1 V2 = P1 V1 V2 V1 / 3