Free Printable Gas Laws Quiz Practice, Chemistry, DPHS, Jara

Worksheets

Gas Laws Quiz Practice, Chemistry, DPHS, Jara

Total questions: 50

Worksheet time: 2hrs 40mins

Name

Class

Date

What is Pressure (P) measured in?

liters

atm, kPa, mmHg

Kelvin

mol

What is Volume (V) measured in?

liters

atm, kPa, mmHg

Kelvin

mol

What is Amount (n) measured in?

liters

atm, kPa, mmHg

Kelvin

mol

What is Temperature (T) measured in?

liters

atm, kPa, mmHg

Kelvin

mol

What does STP stand for, and what are the associated values?

Standard Temperature and Pressure - 1 atm and 273 C

Same Temperature and Pressure - 273 atm and 273 K

Standard Temperature and Pressure - 1 atm and 273 K

Same Temperature and Pressure - 1 atm and 1 K

Standard Temperature and Pressure - 2.73 atm and 100 K

Convert $10^oC$ to kelvin

298 K

313 K

283 K

Convert $25^oC$ to kelvin

298 K

313 K

283 K

Convert $40^oC$ to kelvin

298 K

313 K

283 K

Convert 3.3l atmospheres to kilopascals (1 atm=101.3 kPa)

297 kPa

303 kPa

313 kPa

335 kPa

10.

What happens to the pressure of a gas when it is compressed from 8 liters to 4 liters at constant temperature?

As volume decreases by one-half, pressure decreased by one-half.

As volume decreases by one-half, pressure doubles.

As volume decreases by one-half, pressure decreases by one-fourth.

As volume decreases by one-half, pressure triples.

11.

A beach ball is inflated to 20.5 L at standard pressure. A scuba diver then takes the ball underwater, where the pressure exerted on the ball is 303 kPa. Find the volume of the ball.

5.25 liters

6.85 liters

7.21 liters

10.25 liters

12.

Which graph best demonstrates the relationship between pressure and volume of a gas?

13.

A gas occupies 12.3 liters at a pressure of 40.0 mmHg. What is the volume when the pressure is Increased to 60.0 mmHg?

8.20 liters

10.4 liters

12.3 liters

14.6 liters

14.

What happens to the volume of air in a balloon when it is taken outside on a cold, winter day. why?

The volume of the balloon will decrease. As temperature decreases, volume decreases.

The volume of the balloon will increase. As temperature decreases, volume increases.

15.

600.0 Ml of air is at $20.0^oC$ . What is the volume at $60.0^oC$ ?

600 milliliters

621 milliliters

682 milliliters

700 milliliters

16.

Which graph best demonstrates the relationship between volume and temperature of a gas?

17.

The volume of a balloon is 3.6 liters when measured at $35^oC$ Calculate its new volume, when it is cooled to $15^oC$

2.8 liters

3.0 liters

3.4 liters

4.3 liters

18.

Why does heating a gas held in a rigid container increase its pressure?

As temperature increases, gas kinetic energy increases, resulting in greater collisions with container walls.

As temperature increases, gas kinetic energy decreases, resulting in greater collisions with container walls.

As temperature increases, gas kinetic energy remains the same, resulting in greater collisions with container walls.

19.

The gas pressure of a climber's extra oxygen tank is 4.50 atm at base camp on mount everest, which has a temperature of 271 K. If the pressure decreases to 3.87 atm once the climber reaches the summit, what is the temperature at the summit?

200 K

213 K

233 K

298 K

273 K

20.

Which graph best demonstrates the relationship between pressure and temperature of a gas?

21.

A gas has a pressure of 0.370 atm at $50.0^oC$ . What is the pressure at standard temperature?

0.313 atm

0.352 atm

0.399 atm

0.411 atm

22.

Each flask contains the same number of gas molecules at different volumes. In which flask is the pressure the highest?

Flask A

Flask B

Flask C

Flask D

23.

At stp, a gas occupies 20L. What is the volume at 200k and 2.0 atm?

4.1 liters

5.8 liters

6.7 liters

7.3 liters

24.

Explain why tire pressure decreases in cold weather

As temperature decreases, pressure decreases.

As temperature increases, pressure decreases.

As temperature decreases, pressure remains the same.

25.

A balloon has a volume of 30L at 303 K and 152 kPa. What is the volume at STP?

43 liters

40 liters

37 liters

33 liters

26.

Write the mathematical equation for the ideal gas law, including the meaning of each variable.

P1 x V1= P2 x V2; P - pressure, V - volume

P x V = n x R x T; P - pressure, V - volume, n - mol, R - universal gas constant, and T - temperature

(P1 x V1/T10 = (P2 x V2/T2); P - pressure, V- volume, T - temperature

V1/n1 = V2/n2; V - volume, n - amount

27.

At $35^oC$ , the pressure inside a nitrogen-filled tennis ball is 215 kPa. If the volume is 0.148 L, how many mol of nitrogen are there in the tennis ball?

0.0124 mol nitrogen

0.0766 mol nitrogen

0.2014 mol nitrogen

0.3100 mol nitrogen

28.

John's lungs have a volume of 6.0 L. How many mol of air will his lungs contain at a pressure of 102 kPa and a body temperature of $37^oC$ ?

0.012 mol air

0.24 mol air

0.36 mol air

0.48mol air

29.

Determine the mol of propane in a 17.8 L tank with a pressure of 9.9 atm at $70^oC$

2.7 mol propane

3.6 mol propane

6.3 mol propane

8.5 mol propane

10.7 mol propane

30.

If the number of particles In a sample of gas is doubled, what happens to the volume of the gas?

As amount of a gas is doubled, the volume the gas occupies will decrease by one-half.

As amount of a gas is doubled, the volume the gas occupies will double.

As amount of a gas is doubled, the volume the gas occupies will triple.

As amount of a gas is doubled, the volume the gas occupies will decrease by one-third.

31.

5.00 L of a gas is known to contain 0.965 mol. If the amount of gas is increased to 1.80 mol, what new volume will result?

8.97 liters

9.33 liters

10.1 liters

11.5 liters

32.

Which graph best demonstrates the relationship between amount and volume of a gas?

33.

If 0.0l mol neon gas at a particular temperature and pressure occupies a volume of 0.225 L, what volume would 0.05 mol neon gas occupy under the same conditions?

0.6755 liters

1.125 liters

2.250 liters

3.750 liters

34.

In a mixture of gases, how is the total pressure related to the partial pressures of the gases in the mixture?

Total pressure is the sum of all partial pressures.

Total pressure is the product of all partial pressures.

Total pressure is the difference of all partial pressures.

Total pressure is the quotient of all partial pressures.

35.

A gas mixture contains oxygen, nitrogen, and helium. The partial pressures are 20.0 kPa, 46.7 kPa, and 26.7 kPa, respectively. Calculate the total pressure of the mixture.

89.5 kPa

91.7 kPa

93.5 kPa

100.0 kPa

36.

A gas mixture containing oxygen, argon, and carbon dioxide exerts a pressure of 2.73 atm. If the pressures of oxygen and carbon dioxide are 1.55 atm and 0.72 atm, calculate the pressure of argon.

0.46 atm

0.53 atm

0.61 atm

0.74 atm

37.

Heliox is a helium-oxygen gas mixture used in deep compression scuba dives. a heliox tank contains 80% helium and 20% oxygen. If the total pressure is 650 kPa, calculate the partial pressures of helium and oxygen.

470 kPa; 180 kPa

480 kPa; 170 kPa

500 kPa; 150 kPa

520 kPa; 130 kPa

38.

What is STP

Stoichiometry's Total Presence; Stands for the effect stoichiometry has on gas laws

Standard Temperature and pressure; temp: $1^oC$ pressure: 273 atm

Standard Temperature and Pressure;

temp: 273 K pressure: 1 atm

A Substances Total Pressure; Pressure: $\frac{P1}{T1}=\frac{P2}{T2}$

39.

If a gas is at STP then what will be the volume if there is only 1 mole?

8.315 L

40.1 L

22.4 L

35.0 L

40.

What pressure will 5 mol of gas experience in a 2L tank at $75^oC$ ?

71.4 atm

54.1 atm

75.2 atm

21.9 atm

41.

Calculate the temperature of gas if 40g of $O_2$ is under 5 kPa while occupying 3.5L.

5.01 K

10.1 K

7.92 K

1.68 K

42.

How many grams of $O_2$ is in a 10 L tank if the pressure is 20 atm and the temperature is $20^oC$

9.10 mol

8.31 mol

6.32 mol

2.02 mol

43.

How many moles of gas is there if the gas occupies 140L at STP?

1.02 mol

6.24 mol

9.34 mol

5.50 mol

44.

If the pressure of 1 mole of gas is 15 kPa, then how much space will it take up at $80^oF$ ?

$166.1\ dm^3$

$132.0\ dm^3$

$192.3\ dm^3$

$145.3\ dm^3$

45.

Calculate the temperature (in celcius) of a 5 mol gas that's under 200 mmHg of pressure when the volume is 4.25L

−464.1oC-464.1^oC

−464.1o

−109.2oC-109.2^oC

−109.2o

−207.3oC-207.3^oC

−207.3o

−245.8oC-245.8^oC

−245.8o

46.

What mass of chlorine gas is present if the pressure is 760 mmHg on a volume of 22.4L at $32^oF$ ?

$34g\ Cl_2$

$70g\ Cl_2$

$93g\ Cl_2$

$10g\ Cl_2$

47.

What will be the pressure of 5 mol of gas in a 750 ml bottle at $100^oC$ ?

204.2 atm

105.1 atm

269.1 atm

354.0 atm

48.

Solve for the temperature of 100g HCL(g) if its under a pressure of 10 atm while occupying 30L.

990.0 K

1,315.5 K

750.1 K

1,124.6 K

49.

How much space would be needed for 3 mol gas at a pressure of 0.75 atm at 100K?

32.8 L

50.0 L

12.9 L

22.4 L

50.

How many moles of $CH_4$ is in a 10L tank under a pressure of 20 kPa at $80^oF$ ?

11.04 mol

0.623 mol

9.40 mol

0.0802 mol

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Gas Laws Quiz Practice, Chemistry, DPHS, Jara

Total questions: 50

Worksheet time: 2hrs 40mins

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