I understand some of it but I'm a little confused. Thank u for your help
1. A 1.30 L balloon is taken from room temperature (25.0掳C) and placed into a freezer at -11.5掳C. What is its new volume? (isobaric change)
2. A container of oxygen gas is at STP. If this sample is put into an oven at 280掳C, what would its pressure be, in atmospheres? (isovolumetric change)
3. You have a 2.40 L container of air at STP. From out of nowhere, Bigfoot stomps on it, decreasing the container's volume down to 0.500 L and increasing the pressure to 8.00 atmospheres. How hot, in 掳C, is the air in the container now?
4. You're at the zoo and have a big red 1.80 L helium balloon. The barometric pressure today is 785 mmHg. Then you hear the roar of a lion. Startled, you accidentally release the balloon. It flies away. By the time it reaches the clouds, the atmospheric pressure that high is only 0.300 atmospheres. What would be the volume of the balloon up there? (isothermal change)
5. a) You fill your car's tires to 35 psi when they were cold (12掳C). After driving for 3 hours, your car's tires warm up to 38掳C. What would be the pressure inside your tires now, in psi? (isovolumetric change) b) What is this pressure in atmospheres?
6. A 12.0 L sample of NO2 gas is at STP. What would be its new volume if its pressure was decreased to 575 mmHg and its Kelvin temperature was doubled?
7. A 5.75 gram sample of nitrogen gas is at STP. What would be its volume if its temperature was increased to 317掳C? (isobaric change)
8. a) A sample of Cl2 gas occupies a volume of 11.4 L at 3.50 atmospheres. When the Cl2 is changed to STP conditions, what will be its volume?isothermic b) How many molecules of Cl2 are there?
Partial Pressures
9. A flask contains Ne at 542 mmHg together with Ar at 234 mmHg. What will the total pressure be?
10. A tank is filled with oxygen and nitrogen. The total pressure of the tank is 6.45 atm, and the partial pressure of the nitrogen is 2.07 atm. What is the partial pressure of the oxygen?
11. A tank with a total pressure of 4.7 atm has a mixture of gases that is 72% nitrogen, and the rest is oxygen. What is the partial pressure of the nitrogen? The oxygen?Chemistry. I need a little help?looks like most of these questions can be answered using the ideal gas equation and dalton's law of partial pressures.
i'm only going to answer one question
1:
PV= nRT =%26gt; V = nRT/P
if the P is the same (balloon will change volume, but keep same pressure), so is n R then taking the ratio is easy:
V1/V2 = (nRT1/P)/nRT2/P)
cancel n, R and P you get:
V1/V2 = T1/T2
you have to convert temperatures to kelvin - add 273.2 degrees
V1/V2 = 25+273.2/(273.2-11.5)
= 1.139
V1 = 1.30L
that means that
1.30L/V2 = 1.139
turn it upside down
V2/1.30 = 1/ 1.139
V2 = 1.30 / 1.139
= 1.14 L
it shrank!
