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Heureux · May 19, 2009, 11:21 PM

The lowest borometric pressure recorded to date on Earth was furing Typhoon Tip in the Western atmospheric pressure into the units indicated below. Gor this problem was 870.0 mbar (millibar). Convert this atmospheric pressure into the units indicated. Bar, torr, in. Hg, atm, PSI, mm Hg. Write answers to three sig figs, please show me how to solve...

2. pressure of a 1.50 L sample of an ideal gas is increased from 56 torr to 150 torr at constant temperature. What is the new volume of the gas?

3.The standard car engines in mid-perfomance street cars typically have compression ratios of about 8.50 to 1, whicle most diesel engines have compression ratios of about 21.5 to 1. Assuming that 1) both types of engines are operating at sea level, 2) the fuel/air mixture forms an ideal gas in both engines, 3) the temperature of the fuel air mixture remains constant in both engines and 4) the uncompressed volume of the cylinders in both a typical street car engine and a typical diesel engine, when the fuel units of atmospheres, in both a typical street car engine and a typical diesel, engine, when the fuel/air mixture is compressed ignition. As an example of what "compression ration" means, if the uncompressed ratio of 7.25 to 1, then the volume of the cylinder when the furl/ air mixture is compressed for ignition is equel t (1.60 L/ 7.25= 0.221L)
(STREET CAR---------------- (DIESEL...

4. The temperature of an ideal gas is increased from 15.0 C to 38.0 C at constant pressure. The dinal volume of the gas is 2.79 L. what was the initial volume of the gas.

5. A weather ballon contains 1.10x10 to the 5th power moles of He, and ideal gas. At standard pressure volume of the balloon is 2.70x 10 to the 6th powerL. What is the temperature of the He in the balloon in C

5.Scuba divers breathe a mixture of helium and oxygen gassed for dives in excess of 150 feet. If 15.68 grams of oxygen gas and 7.60 grams of helium gas are both added to a 5.00 L Scuba tank at room temperature, what will be the total pressure in the tank, assuming ideal behavior?

61417x10 to 3 power mg of a homoatomic diatomic ideal gas occupies a volume of 1.37x 10 to the 3 power cc at a temperature of 25 C and a pressure of 16.14 in. Hg. What is the identity of the gas?

these types of problem trouble me because instructor doesn't discuss much about them. Thanks for your help.

Perito · May 20, 2009, 08:03 AM

Convert 870.0 mbar (millibar) into the units indicated. Bar, torr, in. Hg, atm, PSI, mm Hg. Write answers to three significant figures.

This is just a matter of changing the units.

$870\,mbar\,\times\,\frac {number\,of\,desired\,units}{1\,mbar}=desired\,uni ts$

You can look up the unit conversions. For example, 1 bar = 1000 millibar. The equation becomes

$870\,mbar\,\times\,\frac {0.001\,bar}{1\,mbar}=0.870\,bar$ (note: 3 significant figures)

For Torr, Google "millibar to torr" Let me google that for you

1 millibar = 0.750061683 torr

$870\,mbar\,\times\,\frac {0.750061683\,torr}{1\,mbar}=653\,Torr$ (note: 3 significant figures)

2. pressure of a 1.50 L sample of an ideal gas is increased from 56 torr to 150 torr at constant temperature. What is the new volume of the gas?

$\frac {P_1V_1}{T_1}=\frac {P_2V_2}{T_2}$

T1 = T2, so

$P_1V_1=P_2V_2$

Plug in the values and solve for V2.

3.The standard car engines in mid-perfomance street cars typically have compression ratios of about 8.50 to 1, while most diesel engines have compression ratios of about 21.5 to 1.

Assuming that
1) both types of engines are operating at sea level,
2) the fuel/air mixture forms an ideal gas in both engines,
3) the temperature of the fuel air mixture remains constant in both engines and
4) the uncompressed volume of the cylinders in both a typical street car engine and a typical diesel engine, when the fuel units of atmospheres, in both a typical street car engine and a typical diesel, engine, when the fuel/air mixture is compressed ignition.

As an example of what "compression ration" means, if the uncompressed ratio of 7.25 to 1, then the volume of the cylinder when the furl/ air mixture is compressed for ignition is equal to (1.60 L/ 7.25= 0.221L)
(STREET CAR---------------- (DIESEL...

Except for the fact that there doesn't seem to be a question here, this is what I see:
This is just like #2, even with T1=T2 (assumption 3) so it uses the same equations. All you have to do is figure out the ratio of the pressures and solve for volumes or volume ratios (I guess -- since there's no question).

4. The temperature of an ideal gas is increased from 15.0 C to 38.0 C at constant pressure. The final volume of the gas is 2.79 L. what was the initial volume of the gas.

This equation also applies, except that the pressure is constant (P1=P2), so divide that out. Put the equation in a form where you can solve for V2/V1 and solve it.

$\frac {P_1V_1}{T_1}=\frac {P_2V_2}{T_2}$

5. A weather balloon contains $1.10\times10^5$ moles of He, and ideal gas. At standard pressure volume of the balloon is $2.70\times10^6$ . What is the temperature of the He in the balloon in C

Now, you need the full-blown ideal gas equation

$PV=nRT$

You can look up the ideal gas constant (R) here: Gas constant - Wikipedia, the free encyclopedia. Use the units that will work with the equation. "Standard Pressure" is 1 atmosphere.

5.Scuba divers breathe a mixture of helium and oxygen gassed for dives in excess of 150 feet. If 15.68 grams of oxygen gas and 7.60 grams of helium gas are both added to a 5.00 L Scuba tank at room temperature, what will be the total pressure in the tank, assuming ideal behavior?

Use the full-blown ideal gas equation, PV=nRT. You'll have to figure out the number of moles of helium by dividing the weight by the atomic weight of helium. You figure out the number of moles of oxygen by dividing the weight by the molecular weight of oxygen (oxygen forms O2, not O. The molecular weight is approx 32, not 16). And solve.

$6.1417x10^3$ mg of a homoatomic diatomic ideal gas occupies a volume of 1.37x 10 to the 3 power cc at a temperature of 25 C and a pressure of 16.14 in. Hg. What is the identity of the gas?

A "homoatomic" ideal gas would mean it has only one atom. A "diatomic" ideal gas would mean it would have two atoms like O2, N2, or H2. I have no idea what a "homoatomic diatomic" gas would be.

You are given the weight, $6.1417\times\10^3$ , volume, $1.37\times\10^3\,cc$ , the temperature (298 K), and you know the pressure (16.14 in. Hg). You can solve for the number of moles using the latter 3 pieces of information. With the weight, you can calculate the molecular weight or the atomic weight. With that, you should be able to figure out what gas it is -- although you need to know whether it's monatomic or diatomic.