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A gas occupies a volume of 0.2 L at 176 mm Hg. What volume will the gas occupy at 760 mm Hg?
Brian Gonzalez
0.05 L
Greyson Swaniawski
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When a gas occupies a volume of 0.2 L at 176 mm Hg. What volume will the gas occupy at 760 mm Hg?
The volume is 0,046 L.
A gas occupies 30 L at 760 mm Hg what is its volume at 350 mm Hg?
The phrase "760 mm Hg" is physicists' shorthand for "an atmospheric pressure equal to that needed to support a column of mercury [chemical symbol Hg] of length 760 mm". This is approximately average atmospheric pressure at sea level. As the pressure decreases from "760 mm Hg" to "350 mm Hg", the volume of the gas will increase (assuming a constant temperature). The new volume can be determined using Boyle's Law: New Volume = 30 x 760 / 350 = 65.143 Litres
A gas occupies a volume of 0.2 L at 176 mm Hg What volume will the gas occupy at 760 mm Hg?
At a constant temperature, V1 * P1 = P2 * V2 (4.00 L) * (700 Torr) = (1000 Torr) * (V2) V2 = 2.80 L This is presuming that the first pressure is, in fact, 700. Torr, and not just 700 Torr, and that the second pressure is 1000. Torr and not 1000 Torr (that the zeroes are significant). If the zeroes are not significant, then the answer should be rounded to 3 L.
A sample of gas occupies 2.78 x 103 mL at 25oC and 760 mm Hg What volume will the gas sample occupy at the same temperature and 475 mm Hg?
The volume that the gas sample will occupy at the same temperature and 475 mmHg is 4448 mL. In significant figures, the answer would be 4400 mL To find this, you can use the Combined Gas Law, (P1V1)/T1=(P2V2)/T2. First, you need to convert your temperature from degrees Celsius to Kelvin. You can do this by adding 273 to 25, which gives you 298 K. Then you can plug in the given values for volume, pressure, and temperature. The equation should look like this: (760 mmHg * 2.78 x 103 ml) / 298 K = (475 mmHg * V2) / 298 K Then you can solve for V2 to find the unknown volume.
Does 1ml of water weigh 1g?
Yes. It is the standard for density. # 1 gram of pure water at 25 oC and 760 mmHg (STP) occupies a volume of 1 mL. All other densities are measured against this standard.
What is the boiling point of benzine?
Boiling Point (760 mm Hg); 80.1 deg. C (176 deg. F)
How many mL are in 1000 grams of water?
At 4 deg C and at a pressure of 760 mm of mercury, when water is at its highest density, 1000 grams of water will occupy 1000.028 mL. At all other temperatures (pressure = one atmosphere), it will occupy a greater volume. At 100 deg C it will occupy 1043 mL. However, most people will say 1000 grams of water equals 1000 mL.
What is the volume of a gas if 8.24 moles of the gas exerts a pressure of 1720 torr at 43C?
There are a couple of ways to do this, so i'll just pick one. 1 mole of gas occupies 22.4 L at 760 torr and 0C (standard temp and press) (PV/nT)a = (PV/nT)b <-- temp must be kelvin (760 x 22.4L)/(1 x 273) = (1720 x V)/(8.24 x 316) rearrange to solve for volume V = (760 x 22.4L)/(1 x 273) x (8.24 x 316)/1720 V = 94.4 Liters
How will I measure the remaining volume of water in a water tank if it has 760 liters capacity.?
Dip-stick
As the pressure of a gas at 760 torr is changed to 380 torr at a constant temperature the volum of the gas will?
Boyle's law states that pressure is indirectly proportional to the volume. There fore as the pressure of a gas at 760 torr is changed to 380 torr, the volume will increase. Boyle's Law: P1 x V1 = P2 x V2 Rearranging leads to: P1 / P2 = V2 / V1 Substituting our values: 760 / 380 = V2 / V1 Thus the final volume will be twice the initial volume.
What volume will ml of gas at 20 degree celsius and a pressure of 355 mm hg occupy if the temperature is reduced to 80 degree celsius and pressure increased to 760 mm hg?
Let's see if I have the question correct?Initial volume = 1 mLInitial Temp = 20 oC ie 293 KInitial Pressure = 355 mmHg or 47.3 kPaFinal values -Final volume = ? or unknownFinal Temp = 80 oC ie 353KFinal Pressure = 760 mmHg or 101.3 kPaAssuming the gas is acting as an ideal gas. That is the gas has no extra attraction to other molecules of the gas in the sample.The Gas Law states thatP1V1/T1 = P2V2/T2355 x 1 /293 = 760 x ? /80V2 = 9.5 mL
What is the volume of this cylinder that has a radius of 5.5 inches and a height of 8 inches?
Volume = pi*radius2*height Volume = pi*5.5*8 = just over 760 cubic inches
