Chemistry: Post your doubts here!

[My Name]

The density of ice is 1.00 g cm–3.
What is the volume of steam produced when 1.00 cm3 of ice is heated to 323 °C (596 K) at a pressure of one atmosphere (101 kPa)?

[1 mol of a gas occupies 24.0 dm3 at 25 °C (298 K) and one atmosphere.]

A 0.267 dm3 B 1.33 dm3 C 2.67 dm3 D 48.0 dm3

Can someone help me with this !

 

[My Name]

Would be glad if anyone out there could help me with these questions.
( I need simple explanations)

Which gas is likely to deviate most from ideal gas behaviour?
A HCl B He C CH4 D N2

The answer is A NOT C .....Why?



Flask X contains 5 dm3 of helium at 12 kPa pressure and flask Y contains 10 dm3 of neon at 6 kPa pressure.
If the flasks are connected at constant temperature, what is the final pressure?(The answer is A)
A 8 kPa B 9 kPa C 10 kPa D 11 kPa

I don't get this!!

Q9 Use of the Data Booklet is relevant to this question.
The volume of a sample of ammonia is measured at a temperature of 60 °C and a pressure of 103 kPa. The volume measured is 5.37 × 10–3 m3.
What is the mass of the sample of ammonia, given to two significant figures?
A 0.00019 g B 0.0034 g C 0.19 g D 3.4 g

No matter how many times I try it my answer is None of the above!


Section B
An ideal gas obeys the gas laws under all conditions of temperature and pressure.
Which of the following are true for an ideal gas?
1 The molecules have negligible volume.
2 There are no forces of attraction between molecules.
3 The molecules have an average kinetic energy which is proportional to its absolute
temperature.

Third point states
The molecules have an average kinetic energy which is proportional to its absolute
temperature.
The kinetic energy and temperature are related and as one increases so does the other....is this what it says ?

When a sample of a gas is compressed at constant temperature from 1500 kPa to 6000 kPa, its volume changes from 76.0 cm3 to 20.5 cm3.
Which statements are possible explanations for this behaviour?
1 The gas behaves non-ideally.
2 The gas partially liquefies.
3 Gas is adsorbed on to the vessel walls.

Second point;2 The gas partially liquefies.
Why isn't this correct?

 

[My Name]

princess Anu

Can you help?Plz.

 

[RoOkaYya G]

My Name which one?

 

[My Name]

My Name which one?

the two posts above

 

[My Name]

My Name which one?

1=
The density of ice is 1.00 g cm–3.
What is the volume of steam produced when 1.00 cm3 of ice is heated to 323 °C (596 K) at a pressure of one atmosphere (101 kPa)?

[1 mol of a gas occupies 24.0 dm3 at 25 °C (298 K) and one atmosphere.]

A 0.267 dm3 B 1.33 dm3 C 2.67 dm3 D 48.0 dm3

Can someone help me with this !

 

[My Name]

RoOkaYya G

Would be glad if anyone out there could help me with these questions.
( I need simple explanations)

Which gas is likely to deviate most from ideal gas behaviour?
A HCl B He C CH4 D N2

The answer is A NOT C .....Why?



Flask X contains 5 dm3 of helium at 12 kPa pressure and flask Y contains 10 dm3 of neon at 6 kPa pressure.
If the flasks are connected at constant temperature, what is the final pressure?(The answer is A)
A 8 kPa B 9 kPa C 10 kPa D 11 kPa

I don't get this!!

Q9 Use of the Data Booklet is relevant to this question.
The volume of a sample of ammonia is measured at a temperature of 60 °C and a pressure of 103 kPa. The volume measured is 5.37 × 10–3 m3.
What is the mass of the sample of ammonia, given to two significant figures?
A 0.00019 g B 0.0034 g C 0.19 g D 3.4 g

No matter how many times I try it my answer is None of the above!


Section B
An ideal gas obeys the gas laws under all conditions of temperature and pressure.
Which of the following are true for an ideal gas?
1 The molecules have negligible volume.
2 There are no forces of attraction between molecules.
3 The molecules have an average kinetic energy which is proportional to its absolute
temperature.

Third point states
The molecules have an average kinetic energy which is proportional to its absolute
temperature.
The kinetic energy and temperature are related and as one increases so does the other....is this what it says ?

When a sample of a gas is compressed at constant temperature from 1500 kPa to 6000 kPa, its volume changes from 76.0 cm3 to 20.5 cm3.
Which statements are possible explanations for this behaviour?
1 The gas behaves non-ideally.
2 The gas partially liquefies.
3 Gas is adsorbed on to the vessel walls.

Second point;2 The gas partially liquefies.
Why isn't this correct?

 

[RoOkaYya G]

1=
The density of ice is 1.00 g cm–3.
What is the volume of steam produced when 1.00 cm3 of ice is heated to 323 °C (596 K) at a pressure of one atmosphere (101 kPa)?

[1 mol of a gas occupies 24.0 dm3 at 25 °C (298 K) and one atmosphere.]

A 0.267 dm3 B 1.33 dm3 C 2.67 dm3 D 48.0 dm3

Can someone help me with this !

use pV=nRT equation n replace

 

[RoOkaYya G]

RoOkaYya G

https://www.xtremepapers.com/community/members/rookayya-g.47655/

*_* i forgot my theory
sorry

 

[My Name]

use pV=nRT equation n replace

i know that
idk i m not getting the answer
can u solve it ?

 

[My Name]

*_* i forgot my theory
sorry

It's ok,thnx anyway

 

[RoOkaYya G]

It's ok,thnx anyway

sorry

 

[My Name]

sorry

You said that already.
It's oka!

 

[♣♠ Magnanimous ♣♠]

http://papers.xtremepapers.com/CIE/Cambridge International A and AS Level/Chemistry (9701)/9701_s10_qp_21.pdf
question 2 part c-ii
Where and why would C be ?

can some one answer this
Plz and thanku

here you go --> just see this type of graph in coursebook . Well when we use catalyst it's main FUNCTION IS TO LOWER THE ACTIVATION ENERGY. So as shown in graph it lowers the activation energy. Also the particles having energy to react increases in presence of catalyst.
I hope you got it

 

[♣♠ Magnanimous ♣♠]

Would be glad if anyone out there could help me with these questions.
( I need simple explanations)

Which gas is likely to deviate most from ideal gas behaviour?
A HCl B He C CH4 D N2

The answer is A NOT C .....Why?



Flask X contains 5 dm3 of helium at 12 kPa pressure and flask Y contains 10 dm3 of neon at 6 kPa pressure.
If the flasks are connected at constant temperature, what is the final pressure?(The answer is A)
A 8 kPa B 9 kPa C 10 kPa D 11 kPa

I don't get this!!

Q9 Use of the Data Booklet is relevant to this question.
The volume of a sample of ammonia is measured at a temperature of 60 °C and a pressure of 103 kPa. The volume measured is 5.37 × 10–3 m3.
What is the mass of the sample of ammonia, given to two significant figures?
A 0.00019 g B 0.0034 g C 0.19 g D 3.4 g

No matter how many times I try it my answer is None of the above!


Section B
An ideal gas obeys the gas laws under all conditions of temperature and pressure.
Which of the following are true for an ideal gas?
1 The molecules have negligible volume.
2 There are no forces of attraction between molecules.
3 The molecules have an average kinetic energy which is proportional to its absolute
temperature.

Third point states
The molecules have an average kinetic energy which is proportional to its absolute
temperature.
The kinetic energy and temperature are related and as one increases so does the other....is this what it says ?

When a sample of a gas is compressed at constant temperature from 1500 kPa to 6000 kPa, its volume changes from 76.0 cm3 to 20.5 cm3.
Which statements are possible explanations for this behaviour?
1 The gas behaves non-ideally.
2 The gas partially liquefies.
3 Gas is adsorbed on to the vessel walls.

Second point;2 The gas partially liquefies.
Why isn't this correct?

1) Umm, you just read the topic "The kinetic theory of gases"(on page 99 of coursebook written by Roger Norris). Do you observe that all points are related to GASES while HCl IS A LIQUID. So it can be clearly said that IT IS THE ONE WHICH MOST DEVIATE FROM IDEAL GAS BEHAVIOUR.
You got na?

 

[♣♠ Magnanimous ♣♠]

Would be glad if anyone out there could help me with these questions.
( I need simple explanations)

Which gas is likely to deviate most from ideal gas behaviour?
A HCl B He C CH4 D N2

The answer is A NOT C .....Why?



Flask X contains 5 dm3 of helium at 12 kPa pressure and flask Y contains 10 dm3 of neon at 6 kPa pressure.
If the flasks are connected at constant temperature, what is the final pressure?(The answer is A)
A 8 kPa B 9 kPa C 10 kPa D 11 kPa

I don't get this!!

Q9 Use of the Data Booklet is relevant to this question.
The volume of a sample of ammonia is measured at a temperature of 60 °C and a pressure of 103 kPa. The volume measured is 5.37 × 10–3 m3.
What is the mass of the sample of ammonia, given to two significant figures?
A 0.00019 g B 0.0034 g C 0.19 g D 3.4 g

No matter how many times I try it my answer is None of the above!


Section B
An ideal gas obeys the gas laws under all conditions of temperature and pressure.
Which of the following are true for an ideal gas?
1 The molecules have negligible volume.
2 There are no forces of attraction between molecules.
3 The molecules have an average kinetic energy which is proportional to its absolute
temperature.

Third point states
The molecules have an average kinetic energy which is proportional to its absolute
temperature.
The kinetic energy and temperature are related and as one increases so does the other....is this what it says ?

When a sample of a gas is compressed at constant temperature from 1500 kPa to 6000 kPa, its volume changes from 76.0 cm3 to 20.5 cm3.
Which statements are possible explanations for this behaviour?
1 The gas behaves non-ideally.
2 The gas partially liquefies.
3 Gas is adsorbed on to the vessel walls.

Second point;2 The gas partially liquefies.
Why isn't this correct?

2) Of that Flask X and Y wala --->
let P1V1 refer to the He, and P2V2 refer to the Ne, and P3V3 refer to the mixed gases

P*V = constant in all cases

P1V1 + P2V2 = P3V3
12*5 + 6*10 = P3*15
60 + 60 = P3*15
P3 = 120/15
P3 = 8kPa

Final pressure = 8kPa.
I hope now no confusion in this one right?

 

[♣♠ Magnanimous ♣♠]

Would be glad if anyone out there could help me with these questions.
( I need simple explanations)

Which gas is likely to deviate most from ideal gas behaviour?
A HCl B He C CH4 D N2

The answer is A NOT C .....Why?



Flask X contains 5 dm3 of helium at 12 kPa pressure and flask Y contains 10 dm3 of neon at 6 kPa pressure.
If the flasks are connected at constant temperature, what is the final pressure?(The answer is A)
A 8 kPa B 9 kPa C 10 kPa D 11 kPa

I don't get this!!

Q9 Use of the Data Booklet is relevant to this question.
The volume of a sample of ammonia is measured at a temperature of 60 °C and a pressure of 103 kPa. The volume measured is 5.37 × 10–3 m3.
What is the mass of the sample of ammonia, given to two significant figures?
A 0.00019 g B 0.0034 g C 0.19 g D 3.4 g

No matter how many times I try it my answer is None of the above!


Section B
An ideal gas obeys the gas laws under all conditions of temperature and pressure.
Which of the following are true for an ideal gas?
1 The molecules have negligible volume.
2 There are no forces of attraction between molecules.
3 The molecules have an average kinetic energy which is proportional to its absolute
temperature.

Third point states
The molecules have an average kinetic energy which is proportional to its absolute
temperature.
The kinetic energy and temperature are related and as one increases so does the other....is this what it says ?

When a sample of a gas is compressed at constant temperature from 1500 kPa to 6000 kPa, its volume changes from 76.0 cm3 to 20.5 cm3.
Which statements are possible explanations for this behaviour?
1 The gas behaves non-ideally.
2 The gas partially liquefies.
3 Gas is adsorbed on to the vessel walls.

Second point;2 The gas partially liquefies.
Why isn't this correct?

9)Well I am getting 3397.8 now convert it into significant figures you will get answer
Either it B or D as answer
Am I right?

 

[♣♠ Magnanimous ♣♠]

9) (1) here edit 5730 as 5.37 dm3
(2) (3)

 

[♣♠ Magnanimous ♣♠]

Would be glad if anyone out there could help me with these questions.
( I need simple explanations)

Which gas is likely to deviate most from ideal gas behaviour?
A HCl B He C CH4 D N2

The answer is A NOT C .....Why?



Flask X contains 5 dm3 of helium at 12 kPa pressure and flask Y contains 10 dm3 of neon at 6 kPa pressure.
If the flasks are connected at constant temperature, what is the final pressure?(The answer is A)
A 8 kPa B 9 kPa C 10 kPa D 11 kPa

I don't get this!!

Q9 Use of the Data Booklet is relevant to this question.
The volume of a sample of ammonia is measured at a temperature of 60 °C and a pressure of 103 kPa. The volume measured is 5.37 × 10–3 m3.
What is the mass of the sample of ammonia, given to two significant figures?
A 0.00019 g B 0.0034 g C 0.19 g D 3.4 g

No matter how many times I try it my answer is None of the above!


Section B
An ideal gas obeys the gas laws under all conditions of temperature and pressure.
Which of the following are true for an ideal gas?
1 The molecules have negligible volume.
2 There are no forces of attraction between molecules.
3 The molecules have an average kinetic energy which is proportional to its absolute
temperature.

Third point states
The molecules have an average kinetic energy which is proportional to its absolute
temperature.
The kinetic energy and temperature are related and as one increases so does the other....is this what it says ?

When a sample of a gas is compressed at constant temperature from 1500 kPa to 6000 kPa, its volume changes from 76.0 cm3 to 20.5 cm3.
Which statements are possible explanations for this behaviour?
1 The gas behaves non-ideally.
2 The gas partially liquefies.
3 Gas is adsorbed on to the vessel walls.

Second point;2 The gas partially liquefies.
Why isn't this correct?

Section B
1) See page 76. Topic "The kinetic theory of gases"
In that last point ---> THE TEMPERATURE OF THE GAS IS RELATED TO THE AVERAGE KINETIC ENERGY OF THE MOLECULES

It means that third point is also correct and the answer is A
The sentence( I wrote above) clearly says everything and also clears your doubt.

I hope you got it. If any doubt quote this again

 

[♣♠ Magnanimous ♣♠]

Would be glad if anyone out there could help me with these questions.
( I need simple explanations)

Which gas is likely to deviate most from ideal gas behaviour?
A HCl B He C CH4 D N2

The answer is A NOT C .....Why?



Flask X contains 5 dm3 of helium at 12 kPa pressure and flask Y contains 10 dm3 of neon at 6 kPa pressure.
If the flasks are connected at constant temperature, what is the final pressure?(The answer is A)
A 8 kPa B 9 kPa C 10 kPa D 11 kPa

I don't get this!!

Q9 Use of the Data Booklet is relevant to this question.
The volume of a sample of ammonia is measured at a temperature of 60 °C and a pressure of 103 kPa. The volume measured is 5.37 × 10–3 m3.
What is the mass of the sample of ammonia, given to two significant figures?
A 0.00019 g B 0.0034 g C 0.19 g D 3.4 g

No matter how many times I try it my answer is None of the above!


Section B
An ideal gas obeys the gas laws under all conditions of temperature and pressure.
Which of the following are true for an ideal gas?
1 The molecules have negligible volume.
2 There are no forces of attraction between molecules.
3 The molecules have an average kinetic energy which is proportional to its absolute
temperature.

Third point states
The molecules have an average kinetic energy which is proportional to its absolute
temperature.
The kinetic energy and temperature are related and as one increases so does the other....is this what it says ?

When a sample of a gas is compressed at constant temperature from 1500 kPa to 6000 kPa, its volume changes from 76.0 cm3 to 20.5 cm3.
Which statements are possible explanations for this behaviour?
1 The gas behaves non-ideally.
2 The gas partially liquefies.
3 Gas is adsorbed on to the vessel walls.

Second point;2 The gas partially liquefies.
Why isn't this correct?

Section B
2) Of liquefies --->
Well I don't know the exact reason so I think you should remember it
Sorry in this question I was not able to help you