Convert the following pressure into atmospheres.
781 mm Hg
At conditions of constant temperature and pressure, the volume of a sample of ideal gas is proportional to the number of moles of gas present.
If 3.25 mol of argon gas occupies a volume of 100L at a particular temperature and pressure, what volume does 14.15 mol of argon occupy under the same conditions.
Suppose a 24.3-ml sample of helium gas at 25 degrees C and 1.01 atm is heated to 50 degrees C and compressed to a volume of 15.2 ml. What will the pressure of the sample be.© BrainMass Inc. brainmass.com October 24, 2018, 10:15 pm ad1c9bdddf
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convert the following pressure into atmospheres.
1. 1 torr = 1 mmHg
1 atm = 760 mmHg
So 1 mmHg = atm
Then 781 torr = 781 mmHg = 781 * atm = 1.0276 atm
2. A 1.04-L sample of gas at 759 mm Hg pressure is expanded until its volume is 2.24 L. What will be the pressure in the expnaded gas sample at ...
It provides several applications of the ideal gas law. The solution is detailed and has a '5/5' rating.
Problem involving the application of ideal gas law
Mole and Mass relationship in chemical equation:
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The combined Gas Law:
1.If the gas present in 4.65L at STP is changed to a temperature of 15C and pressure of 756mmHg, what will be new volume?
The Ideal Gas Law:
1. Calculate the volume, in liters, of 1.12mol of H2S(g) at 62C and 1.38atm.
2. Calculate the pressure, in atmospheres, of 4.46mol of CO(g) in a 3.96-L tank at 29C.
3. How many moles of Kr(g) are there in 2.22L of the gas at 698mmHg and 45C?
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