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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.
What volume will 500 mL of gas at 20 c and a pressure of 420 mm Hg occupy if the temperature is reduced to 80 c and the pressure increased to 650 mm Hg?
V = k*T/P Apart from the fact that a change in temperature from 20C to 80C cannot be described as a reduction, V2 = V1 * T2P1/T1P2 = 500*(273.15+80)*420/[(273.15+20)*650] = 500*353.15*420/(293.15*650) = 289.2 mL
Which is lower 500 microns or 7500?
If your talking about vacuum 500 microns of Hg is lower.
What is the atomic mass of hg?
Mercury is a metal element. Atomic mass of it is 200.
What is the mass of mercury Hg?
The atomic mass is 201 (rounded to whole numbers). Is that what you needed?
How many milliliters are in 500grams?
1 gram = 1 mL so;500 g = 500 mL34
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 a volume of 0.2 L at 176 mm Hg. What volume will the gas occupy at 760 mm Hg?
0.05 L
At 1250 mm Hg and 75 degrees Celsius the volume of a sample of ammonia gas is 6.28 L What volume would the ammonia occupy at STP?
8.10 L
What volume will 500 mL of gas at 20 c and a pressure of 420 mm Hg occupy if the temperature is reduced to 80 c and the pressure increased to 650 mm Hg?
V = k*T/P Apart from the fact that a change in temperature from 20C to 80C cannot be described as a reduction, V2 = V1 * T2P1/T1P2 = 500*(273.15+80)*420/[(273.15+20)*650] = 500*353.15*420/(293.15*650) = 289.2 mL
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?
7.41 L
40 liters of gas were collected over water when the barometer read 622.0 mm Hg and temp was 20C what volume wuould dry gas occupy at standard conditions?
The gas would occupy 40 liters of space, by volume. This is only true as long as the conditions were normal.
When a sample of nitrogen has a volume of 3.97 L at 1479 mm Hg and - 42 C what volume will it occupy at standard temperature and pressure?
I'm not going to do all your work. The formula is Pressure1 X Volume 1 X Temperaure 1(in Kelvins)= Pressure 2 X Volume 2 X temperaure 2 So 3.97L X 1479mm Hg X 231.15K = y volume X 760mm Hg (1 atmosphere) X 293.15 (20 degrees C) I'll let you figure out the maths.
How many 50 hg in dg?
500
Which is lower 500 microns or 7500?
If your talking about vacuum 500 microns of Hg is lower.
A container filled with gas has a volume of 185 ml and a pressure of 310 mm Hg The desired new volume is 74.0 ml What is the required new pressure?
the answer is 72.1 Hg
Which element has an atomic mass of about 200.54?
Mercury (Hg) has an atomic mass of 200.59
