how can I calculate the total pressure of one day?
361711
You have to know the pressure for each hour and then divide by 24\nand you have your average.
290343
The pressure on the surface is roughly 14.7 PSI. Each 10m of depth is equivalent to 1 atmosphere. Therefore, at 120m, it must withhold 12 atmospheres or 176.4 PSI.
1187434
I think that's dalton's law.  Whoever came up with it, the pressure is additive.  So convert so everything is in the same units, multiply by the percent, add, and then compare to the answers.  I bet it's more fun than you predict.  Whooo!  Conversion factors!  I don't want to take that kind of enjoyment away, so get cracking!
984213
http://en.wikipedia.org/wiki/Pressure_gradient_force\nhttp://en.wikipedia.org/wiki/Temperature_gradient\nHope this helps, good luck!
821966
Not sure where the 600 came from, but it sounds like the question wants the total pressure of all the gases combined.  So you would just add together all the partial pressures, and the total pressure is 330 mm Hg.\n\nDividing the total pressure by the number of gases would give you the average partial pressure, but I don't think that's very useful.
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.
736070
If you know the volume and density of the liquid you can calculate the number of moles n.\n\nOnce you have n and if you assume that the gas will behave like and ideal gas and you fix the temperature and pressure, the volume will be given by:\n\nV = nRT/P.
1034583
For example, the density of water is 1000 kilograms per cubic meter (in SI units), so the weight of a cubic meter of water is 1000 kg times g, the acceleration of gravity (9.8 m/sec2), or 9800 newtons. This force is exerted over 1 m2, so the pressure produced by a 1-meter depth of water is 9800 pascals (the Pa is the SI unit of pressure, equal to 1 newton per square meter). \n\nThe unit of pressure used in atmospheric work on Earth is the hectopascal; 1 hPa = 100 Pa. So the pressure 1 m below the surface of water (ignoring the pressure exerted by the atmosphere on top of it) is 98 hPa. Standard atmospheric pressure is 1013.25 hPa, so it takes 1013.25/98 = 10.33 meters of water to produce a pressure of 1 atmosphere. (That's about 34 feet, for those who like obsolete units.) \n\nThe pressure in the ocean increases by about 1 atmosphere for every 10 meters of depth. The average depth of the ocean is about 4 km, so the pressure on the sea floor is about 400 atmospheres.
497026
Lol, trying to get people to do your chemistry homework?\nUse PV=NRT \nP = Pressure in ATM (1 ATM in STP)\nV = Volume in liters (convert 65cc to liters)\nN = number of moles (will be constant)\nR = gas constant (0.0821 L.ATM/ Mol.K)\nT = temp in Kelvin (273 + degrees C) (STP = 273 K or 0 C)\n\nwith moles being held constant, and the gas constant being constant, your equation should look like;\n\nPV/T (initial) = PV/T (final). solve for P (final)\n\nIf you can't solve this in an hour, i'll post the answer.\n\n....... i was hoping you'd try to solve this and post your answer.....\n\ni got .9383 ATM as the new pressure. mind, that answer is not in sig fig.
501191
There is a formula...but this is much easier\n\nhttp://www.onlineconversion.com/temperature.htm
765689
Yes you are right to subtract the water pressure from the total pressure.\n\nThen use p1v1/t1 = p2v2/t2\n\nSTP is p2v2/t2\n\nSTP = 1 atm and 0C or 273K\n\nSolve for V2.\n\nKeep units the same on both sides!
920577
actualy it depends on the pressure because the formula is:\nQ=m*Cp*Delta(T)\nAnd Cp for water is dependant on Temprature you are giving heat to the water. you can find the analytical method for finding Cp in Thermodynamics  van wylan ed 6
339441
1 atm of pressure is about 14.7 psi,\nso 2175 psi would be about 148 atm.
66340
drink 2 gallons of water and hold it for 1 day then push real hard when going peepee
133134
Pressure is force per unit area. \n\nThe rest of your question is not clear. \n\nPressure is used to forecast weather. \n\nPressure is used to float boats. \n\nPressure is used to power steam engines. \n\nand so on.
569322
Use the ideal gas law \n\nPV/T = constant for the final and initial states.
854810
Since benabean took the absolute difference in the periods, the value of K IS relevant; in fact, crucial to the solution.  My solution:\nTake the ratio of the 2 periods: T2/T1 = √(g1/g2) = 1.00095426\nMultiply this by the seconds in a day (86400)→ 86482.4\n\nSo, a difference of 82.4 sec lost per day.