Question 11 (1 point) What mass of nitrogen is needed to fill an 855 L tank at S

Question

Question 11 (1 point)

What mass of nitrogen is needed to fill an 855 L tank at STP?

Question 11 options:

0.533 kg

0.978 kg

1.07 kg

Question 12 (1 point)

How many mm Hg are in 0.890 atm of pressure?

Question 12 options:

854 mm Hg

676 mm Hg

1.17 x 10-3 mm Hg

Question 13 (1 point)

An air bubble at the bottom of a lake where the pressure is 999 mmHg and the temperature 5oC has a volume of 1.2 mL. What is the volume in mL of the bubble once it has reached the surface of the lake where the pressure is 1.01 atm and the temperature 25oC? The volume of the bubble at the surface is

Question 13 options:

1.66 mL

0.83 mL

5.23 mL

3.65 mL

Question 14 (1 point)

The pressure of a gas in a container is 1.85 atm and occupies a volume of 12.5 L. If the original volume is reduced by half at constant temperature, what would happen to the pressure?

Question 14 options:

the pressure would remain the same

the pressure would double

the pressure would reduce by half

Question 15 (1 point)

Magnesium, an alkaline earth metal reacts with water producing hydrogen gas. If one decides to collect the hydrogen over water at 20oC and the total amount of gas collected is 0.639 L with a pressure of 1.11 atm, what is the amount of hydrogen in g in the sample? Note: the vapor pressure of water at 20oC is 17.5 torr.

The balanced equation is:

Mg(s) + 2 H2O(l) -> Mg(OH)2(aq) + H2(g)

The mass of hydrogen collected over water is _____g.

Question 15 options:

5.77 x 10-2 g

2.89 x 10-2 g

1.16 x 10-2 g

1.31 x 10-2 g

Question 16 (1 point)

On a very cold day, you notice that your tires look a bit deflated than warmer days. This observation can be explained by _____.

Question 16 options:

Boyles law

Charles law

Ideal gas law

Question 17 (1 point)

What is the volume for 1.00 mole of gas at STP?

Question 17 options:

22.4 L

24.5 L

2.05 L

Question 18 (1 point)

The density of carbon dioxide is greater than the density of air and as such it can be used in fire extinguishers to smother the flames by preventing oxygen from the air to feed the fire. What is the density of CO2 at 31oC and 0.98 atm? The density of carbon dioxide under these conditions is ___ g/L.

Question 18 options:

3.66 g/L

5.19 g/L

5.20 g/L

1.73 g/L

Question 19 (1 point)

A sample of nitrogen gas occupies 9.20 L at 21 °C and 0.959 atm. If the pressure is increased to 1.15 atm at constant temperature, what is the newly occupied volume?

Question 19 options:

7.67 L

11.0 L

9.20 L

Question 20 (1 point)

A sample of air has a volume of 5.40 L and a temperature of 25oC, what is the new volume if the temperature increases to 63oC while the pressure is held constant? The final volume is ___ L.

Question 20 options:

5.23

6.09

3.04

33.6

0.533 kg

0.978 kg

1.07 kg

Explanation / Answer

11. mass of nitrogen needed to fill an 855 L tank at STP would be,

0.978 kg

PV = nRT

g = 1 x 855 x 28/298 x 0.08205 = 0.978 kg

12. mmHg in 0.890 atm of pressure would be,

Question 12 options:

676 mmHg

13. The volume of the bubble at the surface is

1.66 ml

n = PV/RT = 1.3145 x 0.0012/0.08205 x 278 = 6.915 x 10^-5 mols

V = nRT/P = 6.915 x 10^-5 x 0.08205 x 298/1.01 = 1.66 ml

14. The pressure of a gas in a container is 1.85 atm and occupies a volume of 12.5 L. If the original volume is reduced by half at constant temperature, the pressure would be,

- the pressure would double

P1V1 = P2V2

P2 = 1.85 x 12.5/6.25 = 3.7 atm

15. Magnesium, an alkaline earth metal reacts with water producing hydrogen gas. If one decides to collect the hydrogen over water at 20oC and the total amount of gas collected is 0.639 L with a pressure of 1.11 atm, the amount of hydrogen in g in the sample would be (Note: the vapor pressure of water at 20oC is 17.5 torr)

The mass of hydrogen collected over water is 2.89 x 10^-2 g.

g = 0.639 x 1.087 x 1.008/0.08205 x 293 = 2.89 x 10^-2 g

16. On a very cold day, you notice that your tires look a bit deflated than warmer days. This observation can be explained by ,

Charles law

V1/T1 = V2/T2

17. The volume for 1.00 mole of gas at STP is,

22.4 L

18. The density of carbon dioxide is greater than the density of air and as such it can be used in fire extinguishers to smother the flames by preventing oxygen from the air to feed the fire. The density of CO2 at 31oC and 0.98 atm would be,

The density of carbon dioxide under these conditions is 1.73 g/L.

density = 0.98 x 44.01/0.08205 x 304 = 1.73 g/ml

19. A sample of nitrogen gas occupies 9.20 L at 21 °C and 0.959 atm. If the pressure is increased to 1.15 atm at constant temperature, the new occupied volume would be,

7.67 L

n = 0.959 x 9.2/0.08205 x 294 = 0.366 mols

V = 0.366 x 0.08205 x 294/1.15 = 7.67 atm

20. A sample of air has a volume of 5.40 L and a temperature of 25oC, the new volume would be if the temperature increases to 63oC while the pressure is held constant 6.09 L.

V1/T1 = V2/T2

V2 = 5.4 x (63+273)/(25+273) = 6.09 L

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