0
A gas occupies a volume of 0.2 L at 176 mm Hg. What volume will the gas occupy at 760 mm Hg?
0.05 L
What else can I help you with?
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.
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
If 7.56 L of a gas are collected at a pressure of 745 mm Hg then what volume will this gas occupy at standard atmospheric pressure if the temperature remains the same?
To find the volume at standard pressure, we can use the combined gas law equation, which states that (P1 x V1) / T1 = (P2 x V2) / T2. Assuming standard pressure is 760 mm Hg, we have: (745 mm Hg x 7.56 L) / T = (760 mm Hg x V2) / T. Solving for V2, we get V2 = (745 x 7.56 x T) / 760. Since the temperature is constant, the volume at standard pressure will be 745 x 7.56 = 5644.2 L.
How will I measure the remaining volume of water in a water tank if it has 760 liters capacity.?
Dip-stick
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
A rectangular prism of volume 84 cm3 has a mass of 760 g. What is the density of the rectangular prism?
9.047619047619048
What is 756 rounded to the nearest 10?
760
What is the boiling point of benzine?
Boiling Point (760 mm Hg); 80.1 deg. C (176 deg. F)
What is 763 rounded to the nearest ten?
760
