chemistry

A sample of a gas (5.0 mol) at 1.0 atm is expanded at constant temperature from 10 L to 15 L. The final pressure is __________ atm.

0.67

The density of ammonia gas in a 4.32 L container at 837 torr and 45.0°C is __________ g/L.

0.719

The molecular weight of a gas that has a density of 7.10 g/L at 25.0°C and 1.00 atm pressure is __________ g/mol.

174

A sample of H2 gas (12.28 g) occupies 100.0 L at 400.0 K and 2.00 atm. A sample weighing 9.49 g occupies __________ L at 353 K and 2.00 atm.

68.2

The volume occupied by 1.5 mol of gas at 35°C and 2.0 atm pressure is __________ L.

19

A balloon originally had a volume of 4.39 L at 44 °C and a pressure of 729 torr. The balloon must be cooled to __________°C to reduce its volume to 3.78 L (at constant pressure).

0

The pressure of a sample of CH4 gas (6.022 g) in a 30.0 L vessel at 402 K is __________ atm.

0.413

The difference in heights of the liquid in the two sides of the manometer is 43.4 cm when the atmospheric pressure is 755 mm Hg. Given that the density of mercury is 13.6 g/mL, the pressure of the enclosed gas is __________ atm.

0.960

The difference in heights of the liquid in the two sides of the manometer is 32.3 cm when the atmospheric pressure is 765 mm Hg. Given that the density of mercury is 13.6 g/mL, the pressure of the enclosed gas is __________ atm.

1.04

A sample of a gas (1.50 mol) is contained in a 15.0 L cylinder. The temperature is increased from 100°C to 150°C. The ratio of final pressure to initial pressure [ ] is __________

1.13

The amount of gas that occupies 60.82 L at 31°C and 367 mm Hg is __________ mol.

1.18

A 0.325 L flask filled with gas at 0.914 atm and 19°C contains __________ mol of gas

1.24 × 10-2

A gas in a 325 mL container has a pressure of 695 torr at 19°C. There are __________ mol of gas in the flask.

1.24 × 10-2

The molecular weight of a gas that has a density of 6.70 g/L at STP is __________ g/mol.

1.50x102

he volume of hydrogen gas at 38.0°C and 763 torr that can be produced by the reaction of 4.33 g of zinc with excess sulfuric acid is __________ L.

1.68

The density of chlorine (Cl2) gas at 25°C and 60. kPa is __________ g/L.

1.7

The mass of nitrogen dioxide contained in a 4.32 L vessel at 48°C and 141600 Pa is __________ g.

10.5

The reaction of 50 mL of Cl2 gas with 50 mL of CH4 gas via the equation: cl2 + Ch4 will produce a total of __________ mL of products if pressure and temperature are kept constant.

100

The reaction of 50 mL of N2 gas with 150 mL of H2 gas to form ammonia via the equation: will produce __________ mL of ammonia if pressure and temperature are kept constant.

100

The National Weather Service routinely supplies atmospheric pressure data to help pilots set their altimeters. The units the NWS uses for atmospheric pressure are inches of mercury. A barometric pressure of 30.51 inches of mercury corresponds to __________ kPa.

103.3

At a temperature of __________ °C, 0.444 mol of CO gas occupies 11.8 L at 889 torr.

106

A closed-end manometer was attached to a vessel containing argon. The difference in the mercury levels in the two arms of the manometer was 12.2 cm. Atmospheric pressure was 783 mm Hg. The pressure of the argon in the container was __________ mm Hg.

122

The molecular weight of a gas that has a density of 5.75 g/L at STP is __________ g/mol.

129

A sample of gas (1.3 mol) occupies __________ L at 22°C and 2.5 atm.

13

The volume of HCl gas required to react with excess magnesium metal to produce 6.82 L of hydrogen gas at 2.19 atm and 35.0 °C is

13.6

A sample of an ideal gas (3.00 L) in a closed container at 25.0°C and 76.0 torr is heated to 300 °C. The pressure of the gas at this temperature is __________ torr.

146

A sample of gas (24.2 g) initially at 4.00 atm was compressed from 8.00 L to 2.00 L at constant temperature. After the compression, the gas pressure was __________ atm.

16.0

Asampleofgas(1.9mol)isinaflaskat21°Cand 697 mm Hg. The flask is opened and more gas is added to the flask. The new pressure is 795 mm Hg and the temperature is now 26°C. There are now __________ mol of gas in the flask.

2.1

A gas at a pressure of 325 torr exerts a force of __________ N on an area of 5.5 m2.

2.4×105

The density of N2O at 1.53 atm and 45.2°C is __________ g/L.

2.58

A sample of a gas originally at 25°C and 1.00 atm pressure in a 2.5 L container is allowed to expand until the pressure is 0.85 atm and the temperature is 15°C. The final volume of the gas is __________ L.

2.8

If 50.75 g of a gas occupies 10.0 L at STP, 129.3 g of the gas will occupy __________ L at STP.

25.5

The pressure exerted by 1.3 mol of gas in a 13 L flask at 22°C is __________ kPa.

250

The Mond process produces pure nickel metal via the thermal decomposition of nickel tetracarbonyl: Ni(CO)4 (l) → Ni (s) + 4CO (g). What volume (L) of CO is formed from the complete decomposition of 444 g of Ni(CO)4 at 752 torr and 22.0°C?

255

10. A pressure of 1.00 atm is the same as a pressure of __________ of mm Hg.

29.9

What volume (L) of NH3 gas at STP is produced by the complete reaction of 7.5 g of H2O according to the following reaction? Mg3N2 (s) + 6H2O (l) → 3Mg(OH)2 (aq) + 2NH3 (g)

3.1

A gas originally at 27°C and 1.00 atm pressure in a 3.9 L flask is cooled at constant pressure until the temperature is 11°C. The new volume of the gas is __________ L.

3.7

The molecular weight of a gas is __________ g/mol if 3.5 g of the gas occupies 2.1 L at STP.

37

The volume of 0.65 mol of an ideal gas at 365 torr and 97°C is __________ L.

41

The reaction of 50 mL of Cl2 gas with 50 mL of CH4 gas via the equation: cl2+ c2h4 will produce a total of __________ mL of products if pressure and temperature are kept constant.

50

A gas at a pressure of 10.0 Pa exerts a force of __________ N on an area of 5.5 m2.

55

What volume (mL) of sulfur dioxide can be produced by the complete reaction of 3.82 g of calcium sulfite with excess HCl (aq), when the final SO2 pressure is 827 torr at 44.0°C?

7.60x102

Automobile air bags use the decomposition of sodium azide as their source of gas for rapid inflation: 2NaN3 (s) → 2Na (s) + 3N2 (g). What mass (g) of NaN3 is required to provide 40.0 L of N2 at 25.0°C and 763 tor

71.1

Ammonium nitrite undergoes thermal decomposition to produce only gases: NH4NO2 (s) → N2 (g) + 2H2O (g) What volume (L) of gas is produced by the decomposition of 35.0 g of NH4NO2 (s) at 525°C

72

In a Torricelli barometer, a pressure of one atmosphere supports a 760 mm column of mercury. If the original tube containing the mercury is replaced with a tube having twice the diameter of the original, the height of the mercury column at one atmosphere pressure is __________ mm.

760

The volume of fluorine gas required to react with 2.67 g of calcium bromide to form calcium fluoride and bromine at 41.0°C and 4.31 atm is __________ mL.

79.9

The volume of 0.25 mol of a gas at 72.7 kPa and 15°C is __________ m3.

8.2×10-3

A sample of He gas (2.35 mol) occupies 57.9 L at 300.0 K and 1.00 atm. The volume of this sample is __________ L at 423 K and 1.00 atm.

81.6

If 3.21 mol of a gas occupies 56.2 L at 44°C and 793 torr, 5.29 mol of this gas occupies __________ L under these conditions.

92.6

he pressure in a 12.2 L vessel that contains 2.34 g of carbon dioxide, 1.73 g of sulfur dioxide, and 3.33 g of argon, all at 42°C is __________ mm Hg.

a.263

A gas mixture of Ne and Ar has a total pressure of 4.00 atm and contains 16.0 mol of gas. If the partial pressure of Ne is 2.75 atm, how many moles of Ar are in the mixture?

b. 5.00

Sodium hydride reacts with excess water to produce aqueous sodium hydroxide and hydrogen gas: NaH(s) + H2O(l)→NaOH(aq) + H2(g) A sample of NaH weighing __________ g will produce 982 mL of gas at 28.0°C and 765 torr, when the hydrogen is collected over water. The vapor pressure of water at this temperature is 28 torr.

c. 0.925

A mixture of He and Ne at a total pressure of 0.95 atm is found to contain 0.32 mol of He and 0.56 mol of Ne. The partial pressure of Ne is __________ atm.

c.0.60

The thermal decomposition of potassium chlorate can be used to produce oxygen in the laboratory. 2KClO3 (s) → 2KCl (s) + 3O2 (g) What volume (L) of O2 gas at 25°C and 1.00 atm pressure is produced by the decomposition of 7.5 g of KClO3 (s)?

c.2.2

In a gas mixture of He, Ne, and Ar with a total pressure of 8.40 atm, the mole fraction of Ar is __________ if the partial pressures of He and Ne are 1.50 and 2.00 atm, respectively.

d. 0.583

A flask contains a mixture of He and Ne at a total pressure of 2.6 atm. There are 2.0 mol of He and 5.0 mol of Ne in the flask. The partial pressure of He is __________ atm.

d. 0.74

A vessel contained N2, Ar, He, and Ne. The total pressure in the vessel was 987 torr. The partial pressures of nitrogen, argon, and helium were 44.0, 486, and 218 torr, respectively. The partial pressure of neon in the vessel was __________ torr.

d. 239

SO2 (5.00 g) and CO2 (5.00 g) were placed in a 750.0 mL container at 50.0°C. The total pressure in the container was __________ atm.

d. 6.78

A sample of H2 gas (2.0 L) at 3.5 atm was combined with 1.5 L of N2 gas at 2.6 atm pressure at a constant temperature of 25°C into a 7.0 L flask. The total pressure in the flask is __________ atm. Assume the initial pressure in the flask was 0.00 atm and the temperature upon mixing was 25°C

d.1.6

A sample of He gas (3.0 L) at 5.6 atm and 25°C was combined with 4.5 L of Ne gas at 3.6 atm and 25°C at constant temperature in a 9.0 L flask. The total pressure in the flask was __________ atm. Assume the initial pressure in the flask was 0.00 atm and the temperature upon mixing was 25°C.

d.3.7

Since air is a mixture, it does not have a "molar mass." However, for calculation purposes, it is possible to speak of its "effective molar mass." (An effective molar mass is a weighted average of the molar masses of a mixture's components.) If air at STP has a density of 1.285 g/L, its effective molar mass is __________ g/mol.

e. 28.80