Chemistry Chapter 5
How many moles of CO are contained in a 5.00 L tank at 155°C and 2.80 atm?
0.399 moles
Determine the density of NH3 gas at 435 K and 1.00 atm.
0.477 g/L
What pressure (in atm) will a sample of O2 gas occupy at 100.0 mL, if O2 has a volume of 25.00 mL at 2.0 atm?
0.50 atm
What is the temperature of NO2 gas if the average speed (actually the root-mean-square speed) of the molecules is 750 m/s?
1.04 × 10 3 K
A steel bottle contains argon gas at STP. What is the final pressure if the temperature is changed to 145°C?
1.53 atm
What is the total volume of the mixture of hydrogen gas and oxygen gas can be obtained from the electrolysis of 110.0 grams of water at 25.0°C and 1.00 atm pressure according to the chemical equation shown below? 2 H2O(l) → 2 H2(g) + O2(g)
224 L
Ideal Gas Law
PV = nRT
The following reaction is used to generate hydrogen gas in the laboratory. If 243 mL of gas is collected at 25°C and has a total pressure of 745 mm Hg, what mass of hydrogen is produced? A possibly useful table of water vapor pressures is provided below. Mg(s) + 2 HCl(aq) → MgCl2(aq) + H2(g) T (°C) P (mm Hg) 20 17.55 25 23.78 30 31.86
0.0190 g H2
The mole fraction of carbon dioxide in dry air near sea level is 0.000375, where the molar mass of carbon dioxide is 44.010. The partial pressure of carbon dioxide when the total atmospheric pressure (dry air) is 97.5 kPa is ________ kPa.
0.0370
A gas bottle contains 0.250 mol of gas at 730 mm Hg pressure. If the final pressure is 1.15 atm, how many moles of gas were added to the bottle?
0.0493 mol
A gas occupies 22.4 L at STP and 19.0 L at 100°C and 1.50 atm pressure. How many moles of gas did the system gain or lose?
0.07 moles lost
What is the density of hydrogen gas at STP?
0.0899 g/L
How many grams of KCl(s) are produced from the thermal decomposition of KClO3(s) which produces 50.0 mL of O2(g) at 25°C and 1.00 atm pressure according to the chemical equation shown below? 2 KClO3(s) → 2 KCl(s) + 3 O2(g)?
0.102 g
A balloon filled with helium gas at 20°C occupies 4.91 L at 1.00 atm. The balloon is immersed in liquid nitrogen at -196°C, while the pressure is raised to 5.20 atm. What is the volume of the balloon in the liquid nitrogen?
0.25 L
How many moles of Ar are contained in a 5.00 L tank at 155°C and 2.80 atm?
0.399 moles
Calculate the ratio of effusion rates of Cl2 to O2.
0.671
Calculate the ratio of effusion rates of Cl2 to F2.
0.73204
Zinc reacts with aqueous sulfuric acid to form hydrogen gas: Zn(s) + H2SO4(aq) → ZnSO4(aq) + H2(g) In an experiment, 201 mL of wet H2 is collected over water at 27°C and a barometric pressure of 733 torr. The vapor pressure of water at 27°C is 26.74 torr. The partial pressure of hydrogen in this experiment is ________ atm.
0.929
4.00-L flask contains nitrogen gas at 25°C and 1.00 atm pressure. What is the final pressure in the flask if an additional 2.00 g of N2 gas is added to the flask and the flask cooled to -55°C?
1.05 atm
A gas sample contains 0.33 atm of Ne, 0.45 atm of Ar, and 0.32 atm of CO. What is the total pressure?
1.1 atm
A mixture of 10.0 g of Ne and 10.0 g Ar has a total pressure of 1.6 atm. What is the partial pressure of Ne?
1.1 atm
How many molecules of CO2 are contained in a 10.0 L tank at 7.53 atm and 485 K?
1.14 × 1024 molecules
A syringe contains 0.65 moles of He gas that occupy 750.0 mL. What volume (in L) of gas will the syringe hold if 0.35 moles of Ne is added?
1.2 L
The concentration of water vapor in a sample of air that has a partial pressure of water of 0.91 torr and a total pressure of air of 735 torr is ________ ppm.
1.2 × 10 3
If NO and NH3 are allowed to effuse through a porous membrane under identical conditions, the rate of effusion for NH3 will be ________ times that of NO.
1.3
In the laboratory, hydrogen gas is usually made by the following reaction: Zn(s) + 2 HCl(aq) → H2(g) + ZnCl2(aq) How many liters of H2 gas, collected over water at an atmospheric pressure of 752 mm Hg and a temperature of 21.0°C, can be made from 3.566 g of Zn and excess HCl? The partial pressure of water vapor is 18.65 mm Hg at 21.0°C.
1.36 L
What is the total pressure in a 6.00-L flask which contains 0.127 mol of H2(g) and 0.288 mol of N2(g)
1.66 atm
A gas mixture contains CO, Ar and H2. What is the total pressure of the mixture, if the mole fraction of H2 is 0.35 and the pressure of H2 is 0.58 atm?
1.7 atm
A syringe contains 589 mL of CO at 325 K and 1.2 atm pressure. A second syringe contains 473 mL of N2 at 298 K and 2.6 atm. What is the final pressure if the contents of these two syringes are injected into a 1.00 L container at STP?
1.7 atm
A basketball is inflated to a pressure of 1.90 atm in a 24.0°C garage. What is the pressure of the basketball outside where the temperature is -1.00°C?
1.74 atm
A fixed amount of gas at 25.0°C occupies a volume of 10.0 L when the pressure is 629 torr. Use Charles's law to calculate the volume (L) the gas will occupy when the temperature is increased to 121°C while maintaining the pressure at 629 torr.
13.2 L
Determine the mass of water formed when 12.5 L NH3 (at 298 K and 1.50 atm) is reacted with 18.9 L of O2 (at 323 K and 1.1 atm). 4 NH3(g) + 5 O2(g) → 4 NO(g) + 6 H2O(g)
17.0 g H2O
What volume will 0.780 moles of He occupy at STP?
17.5 L
The mole fraction of argon in dry air near sea level is 1.818 × 10-5 where the molar mass of argon is 39.948. The concentration of argon in the atmosphere is ________ ppm.
18.18
How many liters of O2 gas at 25°C and 1.00 atm pressure are needed to react with 60.25 grams of potassium hydride according to the chemical equation shown below? 2 KH(s) + O2(g) → H2O(l) + K2O(s)
18.4 L
The concentration of carbon monoxide in a sample of air is 9.2 ppm. There are ________ molecules of CO in 1.00 L of this air at 755 torr and 23°C.
2.3 × 10 17
A mixture of He, Ne and Ar has a pressure of 7.85 atm. If the Ne has a mole fraction of 0.47 and Ar has a mole fraction of 0.23, what is the pressure of He?
2.4 atm
What pressure will 2.6 × 1023 molecules of H2 exert in a 3.9 L container at 45°C?
2.9 atm
Determine the theoretical yield and the percent yield if 21.8 g of K2CO3 is produced from reacting 27.9 g KO2 with 29.0 L of CO2 (at STP). The molar mass of KO2 = 71.10 g/mol and K2CO3 = 138.21 g/mol. 4 KO2(s) + 2 CO2(g) → 2 K2CO3(s) + 3 O2(g)
27.1 g, 80.4 % yield
How many liters of hydrogen gas can be generated by reacting 9.25 grams of barium hydride with water at 20°C and 755 mm Hg pressure according to the chemical equation shown below? BaH2(s) + 2 H2O(l) → Ba(OH)2(aq) + 2 H2(g)
3.21 L
How many grams of water are required to produce 5.50 L of hydrogen gas at 25.0°C and 755 mm Hg pressure according to the chemical equation shown below? BaH2(s) + 2 H2O(l) → Ba(OH)2(aq) + 2 H2(g)
4.02 g
What pressure (in atm) will 0.44 moles of CO2 exert in a 2.6 L container at 25°C?
4.1 atm
What pressure will 14.0 g of CO exert in a 3.5 L container at 75°C?
4.1 atm
A sample of air from a home is found to contain 6.2 ppm of carbon monoxide. This means that if the total pressure is 695 torr, then the partial pressure of CO is ________ torr.
4.3 × 10 -3
A 45.0-L steel tank at 20.0°C contains acetylene gas, C2H2, at a pressure of 1.39 atm. Assuming ideal behavior, how many grams of acetylene are in the tank?
67.8 g
The action of some commercial drain cleaners is based on the following reaction: 2 NaOH(s) + 2 Al(s) + 6 H2O(l) → 2 NaAl(OH)4(s) + 3 H2(g) What is the volume of H2 gas formed at STP when 6.32 g of Al reacts with excess NaOH?
7.87 L
How many liters of oxygen gas can be produced at STP from the decomposition of 0.250 L of 3.00 M H2O2 in the reaction according to the chemical equation shown below? 2 H2O2(l) → 2 H2O(l) + O2(g)
8.41 L
If a sample of 0.29 moles of Ar occupies 3.8 L under certain conditions, what volume will 0.66 moles occupy under the same conditions?
8.6 L
How many mL of O2 gas at 25°C and 755 mm Hg pressure can be produced from the thermal decomposition of 0.300 grams of KClO3(s) according to the chemical equation shown below? 2 KClO3(s) → 2 KCl(s) + 3 O2(g)
90.4 mL
Why does hot air rise?
As air is heated, it expands and becomes less dense (the same mass of air fills a larger volume). This lower density warm air will "float" to the top of cooler, more dense air.
Which of the following samples will have the greatest average speed at 355 K?
CH4
Rank the following in order of decreasing rate of effusion. F2 SF6 CO Kr
CO > F2 > Kr > SF6
Which of the following gases has the lowest average speed at 25°C?
Kr
Why does the rate of effusion increase with a decrease in the molar mass?
The rate of effusion depends on the speed of the gas particles. As the molar mass decreases at a given temperature, the average speed of the particles increases, increasing the rate of effusion.
The volume of 350. mL of gas at 25°C is decreased to 135 mL at constant pressure. What is the final temperature of the gas?
-158°C
A 2.75-L container filled with CO2 gas at 25°C and 225 kPa pressure springs a leak. When the container is re-sealed, the pressure is 185 kPa and the temperature is 10°C. How many moles of gas were lost?
0.0335 mol
What is the mole fraction of CO in a container with a H2 mole fraction of 0.22 and an O2 mole fraction of 0.58?
0.20
A mixture of 0.220 moles CO, 0.350 moles H2 and 0.640 moles He has a total pressure of 2.95 atm. What is the pressure of CO?
0.536 atm
Zinc reacts with aqueous sulfuric acid to form hydrogen gas: Zn(s) + H2SO4(aq) → ZnSO4(aq) + H2(g) In an experiment, 225 mL of wet H2 is collected over water at 27°C and a barometric pressure of 748 torr. How many grams of Zn have been consumed? The vapor pressure of water at 27°C is 26.74 torr.
0.567
A sample of 0.300 moles of nitrogen occupies 0.600 L. Under the same conditions, what amount of moles occupies 1.200 L?
0.600 moles
A mixture of 0.220 moles CO, 0.350 moles H2 and 0.640 moles He has a total pressure of 2.95 atm. What is the pressure of H2?
0.853 atm
A mixture of N2, O2 and Ar has mole fractions of 0.25, 0.65, and 0.10, respectively. What is the pressure of N2 if the total pressure of the mixture is 3.9 atm?
0.98 atm
The density of nitric oxide (NO) gas at 1.21 atm and 54.1°C is ________ g/L.
1.35
What volume will 4.91 × 1022 atoms of Ne occupy at STP?
1.83 L
Determine the density of CO2 gas at STP.
1.96 g/L
A sample of gas initially has a volume of 859 mL at 565 K and 2.20 atm. What pressure will the sample have if the volume changes to 268 mL while the temperature is increased to 815 K?
10.2 atm
What is the volume of 30.0 g of argon gas at 157°C and 2.50 kPa pressure?
1070 L
How many grams of XeF6 are required to react with 0.579 L of hydrogen gas at 6.46 atm and 45°C in the reaction shown below? XeF6(s) + 3 H2(g) → Xe(g) + 6 HF(g)
11.7 g
Convert 1.50 atm to torr.
1140 torr
Determine the volume of SO2 (at STP) formed from the reaction of 96.7 g of FeS2 and 55.0 L of O2 (at 398 K and 1.20 atm). The molar mass of FeS2 is 119.99 g/mol. 4 FeS2(s) + 11 O2(g) → 2 Fe2O3(s) + 8 SO2(g)
32.9 L
Determine the volume of O2 (at STP) formed when 50.0 g of KClO3 decomposes according to the following reaction. The molar mass for KClO3 is 122.55 g/mol. 2 KClO3(s) → 2 KCl(s) + 3 O2(g)
13.7 L
How many liters of hydrogen gas are needed to produce 100.0 grams of water at 25.0°C and 1.00 atm pressure according to the chemical equation shown below? 2 H2(g) + O2(g) → 2 H2O(l)
136 L
A balloon contains 0.76 mol N2, 0.18 mol O2, 0.031 mol He and 0.026 mol H2 at 749 mm Hg. What is the partial pressure of O2?
140 mm Hg
Which of the following samples will have the lowest pressure if they are all at the same temperature and in identical containers (same V)?
15 g Kr
A gas mixture consists of N2, O2, and Ne, where the mole fraction of N2 is 0.55 and the mole fraction of Ne is 0.25. If the mixture is at STP in a 5.0 L container, how many molecules of O2 are present?
2.7 × 1022 molecules O2
How many molecules of XeF6 are formed from 12.9 L of F2 (at 298 K and 2.60 atm) according to the following reaction? Assume that there is excess Xe. Xe(g) + 3 F2(g) → XeF6(g)
2.75 × 1023 molecules XeF6
What is the total volume of hydrogen gas and oxygen gas that can be produced from the thermal decomposition of 0.0425 grams of H2O2 at 700°C and 755 mm Hg according to the chemical equation shown below? H2O2(l) → H2(g) + O2(g)?
201 mL
Which of the following samples will have the greatest volume at STP?
22 g He
What is the Celsius temperature of 100.0 g of chlorine gas in a 55.0-L container at 800 mm Hg?
228°C
What volume will a balloon occupy at 1.0 atm, if the balloon has a volume of 7.6 L at 3.8 atm?
29 L
Determine the volume of H2S (at 375 K and 1.20 atm) needed to produce 55.0 g of S. Assume that there is excess SO2 present. 2 H2S(g) + SO2(g) → 3 S(s) + 2 H2O(g)
29.3 L
The density of chlorine gas at 1.21 atm and 34.9°C is ________ g/L.
3.39
The density of krypton gas at 1.21 atm and 50.0°C is ________ g/L.
3.82
How many grams of calcium hydride are required to produce 4.56 L of hydrogen gas at 25.0°C and 0.975 atm pressure according to the chemical equation shown below? CaH2(s) + 2 H2O(l) → Ca(OH)2(aq) + 2 H2(g)
3.82 g
Which statement is true about kinetic molecular theory?
The collisions of particles with one another is completely elastic.
For 1 mol of an ideal gas, both the pressure and temperature are quadrupled. What is the final volume of the gas?
The final volume of the gas is the same as the initial volume.
A sample of nitrogen gas at 25°C has a pressure of 200 torr. If the volume of the container is increased by a factor of two, what will happen to the pressure? You may assume the temperature remains constant.
The pressure will decrease by a factor of two.
Consider a container of gas under a particular P, V, T set of conditions. Describe how the pressure would change if the volume were doubled while the absolute temperature was doubled.
The pressure would stay constant. The doubling of the volume would, by itself, decrease the pressure by a factor of 2. However, the temperature is also decreasing by a factor of 2. These two changing variables will cancel one another.
Charles's Law
V1/T1 = V2/T2
Avogadro's Law
V1/n1=V2/n2
If the pressure in a gas container that is connected to an open-end U-tube manometer is 116 kPa and the pressure of the atmosphere at the open end of the tube is 752 mm Hg, the level of mercury in the tube will
be 118 mm higher in the arm open to the atmosphere.
Given three cylinders containing O2 gas at the same volume and pressure. Cylinder A is at -15°C, cylinder B is at -5°F, cylinder C is at 255 K. Which cylinder contains the largest mass of oxygen?
cylinder B
Which of the following will cause the volume of an ideal gas to triple in value?
lowering the pressure by a factor of 3 while the temperature stays constant
gases are filled in three containers of same size. The properties of gases are given below. He N2 O2 Pressure (atm) 1 1 1 Temperature (°C) 0 0 0 Mole 1 1 1 What is different in these containers?
mass of gas
The reason why a hot air balloon goes up in the air is that
the hot air inside the balloon is less dense.
In Boyle's Law,
volume is inversely proportional to pressure.
A 1.44-g sample of an unknown pure gas occupies a volume of 0.335 L at a pressure of 1.00 atm and a temperature of 100.0°C. The unknown gas is ________.
xenon
Calcium hydride (CaH2) reacts with water to form hydrogen gas: CaH2(s) + 2H2O(l) → Ca(OH)2(aq) + 2H2(g) How many grams of CaH2 are needed to generate 48.0 L of H2 gas at a pressure of 0.888 atm and a temperature of 32°C?
35.8 g
A 0.465 g sample of an unknown compound occupies 245 mL at 298 K and 1.22 atm. What is the molar mass of the unknown compound?
38.0 g/mol
Which gas sample has the greatest volume at STP?
4 g of H2
The concentration of ozone in a sample of air that has a partial pressure of O3 of 0.33 torr and a total pressure of air of 735 torr is ________ ppm.
4.5 × 10 2
When 14.0 g of zinc metal reacts with excess HCl, how many liters of H2 gas are produced at STP?
4.80 L
The mole fraction of oxygen in dry air near sea level is 0.20948. The concentration of oxygen is ________ molecules per liter, assuming an atmospheric pressure of 739 torr and a temperature of 29.5°C.
4.93 × 10 21
A sample of N2 effuses in 255 s. How long will the same size sample of Cl2 take to effuse?
406 s
How many grams of F2 gas are there in a 5.00-L cylinder at 4.00 × 103 mm Hg and 23°C?
41.1 g
A 0.600 g sample containing Ag2O and inert material is heated, causing the silver oxide to decompose according to the following equation: 2 Ag2O(s) → 4 Ag(s) + O2(g). If 13.8 mL of gas are collected over water at 27°C and 1.00 atm external pressure, what is the percentage of silver oxide in the sample? The partial pressure of water is 26.7 mm Hg at 27°C.
41.8%
A large balloon is initially filled to a volume of 25.0 L at 353 K and a pressure of 2575 mm Hg. What volume of gas will the balloon contain at 1.35 atm and 253 K?
45.0 L
What pressure would a gas mixture in a 10.0 L tank exert if it were composed of 48.5 g He and 94.6 g CO2 at 398 K?
46.6 atm
container filled with gas is connected to an open-end manometer that is filled with mineral oil. The pressure in the gas container is 753 mm Hg and atmospheric pressure is 724 mm. How high will the level rise in the manometer if the densities of Hg and mineral oil are 13.6 g/mL and 0.822 g/mL respectively?
480 mm
What volume (in mL) will a sample of F2 gas occupy in a syringe at 5.5 atm, if the F2 has a volume of 25.0 mL at 1.2 atm?
5.5 mL
To what volume will a sample of gas expand if it is heated from 50.0°C and 2.33 L to 500.0°C?
5.58 L
How many grams of zinc metal are required to produce 2.00 liters of hydrogen gas at STP according to the chemical equation shown below? Zn(s) + 2 HCl(aq) → ZnCl2(aq) + H2(g)
5.83 g
Calculate the root mean square velocity of nitrogen molecules at 25°C.
515 m/s
A 1.000 kg sample of nitroglycerine, C3H5N3O9, explodes and releases gases with a temperature of 1985°C at 1.100 atm. What is the volume of gas produced? 4 C3H5N3O9(s) → 12 CO2(g) + 10 H2O(g) + 6 N2(g) + O2(g)
5378 L
How many milliliters of ozone gas at at 25.0°C and 1.00 atm pressure are needed to react with 45.00 mL of a 0.100 M aqueous solution of KI according to the chemical equation shown below? O3(g) + 2 I-(aq) + H2O(l) → O2(g) + I2(s) + 2 OH-(aq)
55.0 mL
How many liters of oxygen are needed to exactly react with 19.8 g of methane at STP? CH4(g) + 2 O2(g) → CO2(g) + 2 H2O(l)
55.5 L
Determine the total pressure of all gases (at STP) formed when 50.0 mL of TNT (C3H5(NO3)3, d = 1.60 g/mL, molar mass = 227.10 g/mol) reacts according to the following reaction. 4 C3H5(NO3)3(l) → 6 N2(g) + O2(g) + 12 CO2(g) + 10 H2O(g)
57.2 L
What is the average speed (actually the root-mean-square speed) of a neon atom at 27°C?
609 m/s
Calculate the temperature, in K, of 2.20 moles of gas occupying 3.50 L at 3.30 atm.
64.0 K
What is the pressure in a gas container that is connected to an open-end U-tube manometer if the pressure of the atmosphere is 742 torr and the level of mercury in the arm connected to the container is 8.60 cm higher than the level of mercury open to the atmosphere?
656 mm Hg
How many molecules of N2 are in a 400.0 mL container at 780 mm Hg and 135°C?
7.38 × 10 21 molecules
A 0.286-g sample of gas occupies 125 mL at 60. cm of Hg and 25°C. What is the molar mass of the gas?
71 g/mol
A syringe initially holds a sample of gas with a volume of 285 mL at 355 K and 1.88 atm. To what temperature must the gas in the syringe be heated/cooled in order to have a volume of 435 mL at 2.50 atm?
721 K
A fixed amount of gas at 25.0°C occupies a volume of 10.0 L when the pressure is 667 torr. Use Boyle's law to calculate the pressure (torr) when the volume is reduced to 7.88 L at a constant temperature of 25.0°C.
846 torr
What mass of NO2 is contained in a 13.0 L tank at 4.58 atm and 385 K?
86.7 g
To what temperature must a balloon, initially at 25∘C and 2.00 L, be heated in order to have a volume of 6.00 L?
894 K
Using the graph below, determine the gas that has the lowest density at STP. (see graph)
A
Which container has the lowest pressure? All containers have same volume and temperature. Assume that the mass does not affect pressure. A B C (see picture)
A and B
Three identical flasks contain three different gases at standard temperature and pressure. Flask A contains C2H4, flask B contains O3, and flask C contains F2. Which flask contains the largest number of molecules?
All contain same number of molecules
Which of the following statements is true?
At low temperatures, intermolecular forces become important and the pressure of a gas will be lower than predicted by the ideal gas law.
Which of the following statements is true?
At very high pressures, a gas will occupy a larger volume than predicted by the ideal gas law.
A mixture of 1.0 mol He and 1.0 mol Ne are at STP in a rigid container. Which of the following statements is true?
Both gases have the same average kinetic energy.
Identify the molecule that effuses the fastest.
CH4
The volume of a gas is proportional to the temperature of a gas is known as
Charles's Law.
A 0.334 g sample of an unknown halogen occupies 109 mL at 398 K and 1.41 atm. What is the identity of the halogen?
Cl2
Which of the following is not true when air is inhaled in the lungs?
Concentration of air molecules in the lungs increases.
Which of the gases in the graph below has the largest molar mass? (see graph)
D
Define diffusion.
Diffusion is the process by which gas molecules spread out in response to a concentration difference.
Define effusion
Effusion is the process by which a gas escapes from a container into a vacuum through a small hole.
Which is not an assumption in the kinetic molecular theory for gases?
Gas molecules attract each other
Under identical conditions of temperature and pressure, which of the following gasses is the lightest?
H2
Why doesn't Dalton's Law of Partial Pressures depend on the identity of the gases present?
It is assumed that all gas particles are behaving ideally and not interacting with one another. If that is true, the only difference between particles is associated with their mass. Since all of the gases are at the same temperature and have the same average kinetic energy, their masses don't have to be taken into account. The different gas particles exert the same force on the walls of the container, no matter what their mass.
Explain what the term "mean free path" describes. How does it change with decreasing pressure?
Mean free path describes the distance that a gas particle can travel before hitting another particle. As pressure decreases, the distance between particles increases, therefore increasing the mean free path of the particles.
The rate of effusion of oxygen to an unknown gas is 0.935. What is the other gas?
N2
Which of the following gases has the highest average speed at 400K?
N2
A compound is found to be 30.45% N and 69.55 % O by mass. If 1.63 g of this compound occupy 389 mL at 0.00°C and 775 mm Hg, what is the molecular formula of the compound?
N2O4
Place the following gases in order of increasing density at STP. N2 NH3 N2O4 Ar
NH3 < N2 < Ar < N2O4
Which of the following gas samples would be most likely to behave ideally under the stated conditions?
Ne at STP
What is the major component in dry air?
Nitrogen
The density of a gas is 1.43 g/mole at STP. What is the gas?
O2
Which of the following would have a density of 1.37 g/L at 7.0°C and 0.987 atm?
O2
Boyle's Law
P1V1 = P2V2
Dalton's Law
PT = PA + PB + PC ...
What is the SI unit of pressure?
Pascal (Pa)
Which of the following samples has the greatest density at STP?
SF6
Which of the following compounds will behave least like an ideal gas at low temperatures?
SO2