I will kiss you if you get all these chem problems right?

Question

Question 1 2 points Save
The temperature of a sample of an ideal gas confined in a 2.0 L container was raised from 27 oC to 77 oC. If the initial pressure of the gas was 1200 mmHg, what was the final pressure of the gas?
300 mmHg
600 mmHg
1400 mmHg
2400 mmHg
3600 mmHg
A sealed container contains 0.20 moles of oxygen gas and 0.10 moles of hydrogen gas. If the temperature is 25 oC throughout the container, which of the following is true?
The partial pressures of the two gases are the same.
The average kinetic energy of the two gases are the same.
The molecular masses of the two gases are the same.
The total masses of the two gases are the same.
The average molecular speeds of the two gases are the same.

A gas sample contains 0.1 mole of oxygen and 0.4 moles of nitrogen. If the sample is at standard temperature and pressure, what is the partial pressure due to nitrogen.
0.1 atm
0.2 atm
0.5 atm
0.8 atm
1.0 atm

A mixture of gases contains 1.5 moles of oxygen, 3.0 moles of nitrogen, and 0.5 moles of water vapor. If the total pressure is 700 mmHg, what is the partial pressure of the nitrogen gas?
70 mmHg
210 mmHg
280 mmHg
350 mmHg
420 mmHg

A mixture of helium and neon gases has a total pressure of 1.2 atm. The mixture contains twice as many moles of helium as neon, what is the partial pressure due to neon?
0.2 atm
0.3 atm
0.4 atm
0.8 atm
0.9 atm

Nitrogen gas was collected over water at 25 oC. If the vapor pressure of water at 25 oC is 23 mmHg, and the toal pressure in the container is measured at 781 mmHg, what is the partial pressure of the nitrogen gas?

23 mmHg
46 mmHg
551 mmHg
735 mmHg
758 mmHg

A 22.0 gram sample of an unknown gas occupies 11.2 liters at standard temperature and pressure. Which of the following could be the identity of the gas?
CO2
SO3
O2
N2
He

Answer 1

The first part is really simple. Assume ideal gas state and use the relationship: T1 / P1 = T2 / P2 (vol. constant).
P2 = (T2 * P1 ) / T1
P2 = ( 77 * 1200 ) / 27
P2 =3422mmHg

The other questions are:
F, F, F, F , T

Answer 2

1)
Volume is constant, therefore the relationship P1/T1 = P2/T2. Using it, we have:
1200/27 = P2/77
P2 = 3422 mmHg, from the choices given 3600mmHg is most suitable

2)
The average kinetic energy of the two gases are the same. As temperature is defined as average kinetic energy, and since temperature is constant, therefore the KE of two gases are same, even though each gas molecular speeds may differ.

3)
Partial pressure due to nitrogen is : mole fraction x total pressure = (0.4/0.5) x 1 = 0.8atm

4)
Again, partial pressure due to nitrogen is :
mole fraction x total pressure = 3/(3+0.5+1.5) x 700mHg =420mmHg

5)
Partial pressure due to neon is:
Moles of neon = x
Moles of helium 2x
Total moles = 3x
Mole fraction for neon = x/3x = 1/3
And partial pressure is; mole fraction x total pressure = 1/3 x 1.2 = 0.4atm

6)
Partial pressure of water be 23mmHg, which is due to water. Now for neon it will be, 781-23 = 758mmHg

7)
One mole of ANY gas occupies at STP 22.4 dm3
1dm3 = 1litre
now, 11.2dm3 is occupied
moles = 0.5 moles
number of moles = m / mr, where m is mass in grams and mr is molecular mass
Mr = m/n = 22/0.5 = 44.
It is CO2, as CO2 has Mr 44 ; (12 + 16x2)

Answer 3

1. In absolute temperature, the final to starting temps are in the ratio of 7:6. With constant volume, the final pressure to starting pressure are in the ratio of 7:6. So the answer is 1400 mm.
2. The speeds are the same (Boltzman Law)
3. Partial pressures are proportional to the mole fraction of gas components. Here, nitrogen comprises 4/5th of the moles, so it comprises 4/5th of the pressure. Answer= 0.8 atm
4. Same deal, nitrogen comprises 3/5th of the moles, so it comprises 3/5th the pressure, 420 mm
5. Same deal. Neon comprises 1/3 of moles, so it comprises 1/3 of pressure, 0.4 atm.
6. In a "wet gas" mixture, the water vapor fraction contributes its vapor pressure to the mixture. So the non-water pressure is 758 mm
7. Since 11.2 liter is one-half the volume of a mole of gas at STP, the gas involved must be present as one-half mole. One mole would weight 44 grams, which is the same as CO2.

Answer 4

aww ur so cute u were waitin 4 da right 1?!?! okay...well seems like she is going thru some stuff right now! b4 she use 2 give signs and now she dosnt give any at all that doesn't sound gud! you should try talking to her 1 on 1 and nt listen 2 what your friends are saing its hard to do but you have to talk to her like if she makes an excuse just be like "just give me a minute i just want to talk to you and know what going on cuz ur kinda keeping me in a roler coster here! she might feel awcuard because she told u bout her ex so now she feels like she cant face u us gurls do that alot! like and then we just cant face the guy she might be embarrassed or something! you should txt her like txtx her rite now and talk 2 her! Well gud luck i would appreciate if you told me how it went! im curious! :)

Answer 5

You would have kissed me 15 yrs ago when I was actively doing this crap. Now I would have to refresh and research. I can tell you however who is likely to win the UEFA champions league in 2008. Do I get a kiss for that?

Answer 6

You look 14. I would go to prison for getting kissed by you.

Answer 7

Show me your original photo, then i might think of answering it. ;)

Answer 8

I love kisses, but I hate chemistry.....what do I better do????? Somebody help me fast!!!!!!!!!

Answer 9

To hell with the homework- let's go to bed ;)

Answer 10

ur nuts. plus ima girl. so plz no kisses