Practice: What volume will 5.72 x 10^{25} atoms of argon gas occupy at STP?

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In order to accurately study the effect that changes in pressure, temperature and moles have on volume, chemists will often run their experiments under **Standard State conditions**.

Concept #1: Understanding Standard State Conditions

**Transcript**

Welcome back, guys! In this new video, we're going to take a look to see what happens to our gas behavior under standard states. We're going to say sometimes chemists want to understand the influences that pressure, volume or temperature have on a particular gas particle. To do this, they do these experiments under what we call standard conditions.

We're going to say that these standard conditions are sometimes referred to as STP. STP just means standard temperature and pressure. We're going to say standard temperature is zero degrees Celsius. which really is 273.15 Kelvin. Standard pressure is one atmosphere.

Concept #2: Standard Molar Volume

**Transcript**

We're going to say under standard state conditions, the volume of one mole of any gas, an ideal gas just means a gas that behaves as though it's by itself. One mole of any gas under STP will then have the same volume. At STP, one mole of carbon dioxide, one mole of nitrogen gas, or one mole of helium gas – all of these gases look different. Some of them are just atoms by themselves. Others are different elements connected together.

Under standard state conditions, under STP, all moles of gases have the same volume. They all have 22.4 liters. We're going to say that this volume is known as our standard molar volume. Remember, under STP conditions, one mole of any type of gas will have that as their volume.

At **STP**, **1 mole** of any ideal gas will occupy exactly **22.4 Liters** of volume inside a container.

Knowing the meaning of STP allows you to now further manipulate the Ideal Gas Law.

Concept #3: Combined Gas Law

**Transcript**

Let's look at this example which uses our STP concept. We're going to see a sample of Freon-12 occupies 20.7 liters at 25 degrees Celsius and 947 torrs. Now they're saying what is the volume under standard conditions. Remember, what are they asking me? They're asking me to find the volume. But here they already gave me a volume. This must be my volume 1 and this must be my volume 2. They also gave me a temperature and they gave me a pressure. Here, they’re saying under standard conditions. Standard condition means we have a standard pressure and a standard temperature.

Our P2 would be one 1 atmosphere and our standard temperature would be to 273.15 Kelvin. Since we’re deal with a gas, we write PV equals nRT. Again guys, we're dealing with two sets of data. Remember, what have we done when we have two sets of something, two volumes or two pressures? We’d have to check to see who they're talking about. They're talking about pressure, they’re talking about volume and they're talking about temperature. They're not talking about moles because moles are being held constant, so we ignore it. R is our constant as well so we ignore that too. Everything is not on the same side of the equation sign. Divide everything by T to bring it over to the left. PV over T, since we’re dealing with two sets of data, it’s P1V1 over T1 equals P2V2 over T2.

This creates a whole new type of gas law, which we call the combined gas law. We haven't seen that until now. This is our combined gas law P1V1 over T1 equals P2V2 over T2. This is our combined gas law. We're going to plug in the units that we know into this combined gas law. But first, you have to change the temperature into Kelvin and you have to change those 947 torrs into atmospheres. T1 is 25 degrees Celsius, so all we have to do is add 273.15 which gives us 298.15 Kelvin. Pressure 1 is 947 torrs. We just have to change this to atmospheres. For every 1 atmosphere it's 760 torrs. When we do that, we get our answer as 1.24605 atmospheres. All we have to do now is plug it in and solve for our missing variable. Our P1 is 1.24605 atmospheres. Our volume 1 I told you was 20.7 liters. Our temperature 1 was 298.15

Kelvin, equals.

The pressure 2 was 1 atmosphere. That's really not going to change anything, so we plug it in anyways, 1 atmospheres. V2 is what we're looking for over temperature 2 which is 273.15 Kelvin. What we're going to do here is we’re just going to solve for everything on the left. Do the P1 times the V1 divided by T1. When we do all of that, the left side gives me 0.086511 liters times atmospheres over K. This still equals my 1 atmosphere times V2 divided by 273.15 Kelvin. Multiply both sides now by the 273.15 Kelvin. Kelvins cancel out, so then that’s going to give me 23.6305 liters times atmospheres still equals 1 atmosphere times V2. Divide both sides by the 1 atmosphere, which doesn't do anything. All it does is it helps get rid of these atmospheres in the units. So then V2 equals, we're going to just do 3 sig figs here. It's 23.6 liters. That would be the answer for our volume 2.

Again guys, remember even though we started out with the ideal gas law, because we have two sets of data again, we have to manipulate the ideal gas law. Doing that helped us isolate our answer here for V2. Now that you’ve seen this and now that you understand what STP is, I want you guys to attempt the next question.

Practice: What volume will 5.72 x 10^{25} atoms of argon gas occupy at STP?

Concept #4: Using the Ideal Gas Law to find density or molar mass

**Transcript**

We're going to say that we're used to seeing the ideal gas law as PV equals nRT. But we should realize that we can manipulate this equation further in order to find the molar mass of the gas, or the density of a gas. Here, to find the molar mass of a gas, we change it. This capital M is not molarity, it's molar mass. Remember, the units for molar mass or molecular mass are grams per mole. We’re going to say the molar mass of a gas is equal to mRT over PV. We're going to say m represents the mass of the gas in grams, and then all the other variables stay the same. R is still our gas constant. Temperature is still in Kelvin. P is still in atmospheres and volume is still in liters.

If we want to find the density of a gas, we could say the density of a gas is equal to pressure times the molar mass divided by RT. This can become our equation. We could also further manipulate if we wanted the second equation. We could have combined mass and volume together to give us one thing. Remember, mass over volume helps us find density. We could have manipulated this further by saying molar mass of a gas is equal to density times RT over P. We could have used this as well. But then again, if we have a question dealing with the density of a gas, we know we could use this one and we could just manipulate it.

Even though this is a potential equation, we can get to it by just manipulating this third one. I’d recommend just remembering these three. If you're dealing with a question that gives you density and wants the molecular weight, you just use the third one. Manipulate it to find your answer.

The Ideal Gas Law can be further manipulated into new equations. These new equations can help us find the density or molar mass of a gas.

When calculating the density of a gas it is essentially to also recall the formula of that gas in order to find the molar mass, M.

Practice: What is the density of chlorine gas at STP?

Remember that units for molar mass are grams of compound divided by the moles of that compound.

Practice: An unknown gas sample weighs 3.12 g. If it has a volume of 0.206 µL when the temperature is 45^{o}C and the pressure is 957 torr. What is its molar mass?

0 of 7 completed

Concept #1: Understanding Standard State Conditions

Concept #2: Standard Molar Volume

Concept #3: Combined Gas Law

Practice #1: What volume will 5.72 x 1025 atoms of argon gas...

Concept #4: Using the Ideal Gas Law to find density or molar...

Practice #2: What is the density of chlorine gas at STP?

Practice #3: An unknown gas sample weighs 3.12 g. If it has ...

What is the volume occupied at STP by a mixture of 4.00 g of He(g), 2.00 g of H2(g) and 32.0 g of O2(g)?
A. 6.15 L
B. 11.2 L
C. 22.4 L
D. 44.8 L
E. 67.2 L

What volume will 3.12 grams of helium occupy at STP?

Which of the following gases has the highest density at STP?
A. sulfur trioxide, SO 3
B. carbon dioxide
C. NO 2
D. argon
E. nitrogen

What volume will 0.780 moles of Xe occupy at STP?

For the combustion of sucrose, C12H22O11, shown below:
a) How many moles of oxygen are required to react with 1.00g of sucrose?
C12H22O11 + 12O2 → 12CO2 + 11H2O
b) If the CO2 produced from the combustion of 1.00g of sucrose is trapped in a balloon, what volume will it occupy at STP?

A sample of N2 gas occupies a volume of 746 mL at STP. What volume would N 2 gas occupy at 155°C at a pressure of 368 torr?
1. 983 mL
2. 566 mL
3. 3295 mL
4. 312 mL
5. 588 mL
6. 323 mL
7. 2415 mL
8. 1792 mL

Which gas sample has the greatest volume at STP?
a. 5g Ar
b. 5g Rn
c. 5g Ne
d. 5g Kr
e. 5g Xe

Determine the theoretical yield of K 2CO3 when 0.392 moles of KO 2 react with 29.0 L CO2 (at STP – 0°C, 1 atm). The molar mass of KO 2 = 71.10 g/mol and K 2CO3 = 138.21 g/mol.
4KO2(s) + 2CO2(g) → 2K2CO3(s) + 3O2(g)
a. 27.1 g
b. 179 g
c. 91.7 g
d. 206 g
e. 61.0 g

At STP what volume of N 2 will react completely with 22.2 L H 2 to produce NH3?
N2(g) + 3H2 (g) → 2NH 3 (g)
a. 7.4 L
b. 14.8 L
c. 22.2 L
d. 44.4 L
e. 66.6 L

Use the molar volume of a gas at STP to determine the volume (in L) occupied by 33.6 g of neon at STP.

Determine the volume of O2 (at STP) formed when 50.0 g of KClO 3 decomposes according to the following reaction.
2 KClO3 (s) → 2 KCl (s) + 3 O2 (g)
A) 8.22 L
B) 9.14 L
C) 14.6 L
D) 12.3 L
E) 13.7 L

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 H 2 (g)
What is the volume of H2 gas formed at STP when 6.32 g of Al reacts with excess NaOH?
A) 8.59 L
B) 3.50 L
C) 5.25 L
D) 7.87 L

Automobile air bags inflate following a serious impact. The impact triggers the chemical reaction:
2 NaN3(s) → 2Na(s) + 3 N2(g)
If an automobile air bag has a volume of 11.8 L, what mass of NaN 3 (in g) is required to fully inflate the air bag upon impact? Assume STP conditions.

Hydrogen gas (a potential future fuel) can be formed by the reaction of methane with water according to the equation:
CH4(g) + H2O(g) → CO(g) + 3 H2(g)
In a particular reaction, 25.5 L of methane gas (measured at a pressure of 732 torr and a temperature of 25 °C) mixes with 22.8 L of water vapor (measured at a pressure of 702 torr and a temperature of 125 °C). The reaction produces 26.2 L of hydrogen gas at STP. What is the percent yield of the reaction?

An ideal gas occupies 49.0 L at 994 torr and 41.0°C.
What volume would it occupy at STP?
1. 0.0136 L
2. 73.7 L
3. 55.7 L
4. 58.7 L
5. 105 L
6. 39.1 L
7. 69.9 L
8. 0.0179 L
9. 22.4 L

Methane, CH4(g), reacts with steam to give synthesis gas, a mixture of carbon monoxide and hydrogen.
CH4 (g) + H2O(g) → CO(g) + H2(g) [unbalanced]
What mass of hydrogen is formed if 275 L of methane (measured at STP) is converted to synthesis gas?

Consider three 1-L flasks at STP. Flask A contains NH 3 gas, flask B contains NO2 gas, and flask C contains N2 gas. In which flask are the molecules least polar and therefore most ideal in behavior?

The density of a gas is 1.43 g/L at STP. Calculate its density under a pressure of 743 torr and 26°C

A gas has a density of 3.214 g/L at 728 torr and 24°C. What would be its density at STP?

One mole of nitrogen and one mole of neon are combined in a closed container at STP.How big is the container?

What volume will 40.0 L of He at 50.00°C and 1201 torr occupy at STP?A. 26.7 LB. 18.6 LC. 12.8 LD. 53.4 LE. 31.1 L

Calculate the density of nitrogen gas at STP.A. 0.625 g/LB. 1.25 g/LC. 6.83 g/LD. 13.7 g/LE. Cannot be calculated with this information (undefined)

A balloon filled with helium occupies 20.0 L at 1.50 atm and 25°C. How many moles of helium will there be in the balloon at STP?A. 22.4 molesB. 1.12 molesC. 0.0446 molesD. 0.893 molesE. 1.23 molesF. 4.55 moles

If 250 mL of a gas at STP weighs 2 g, what is the molar mass of the gas?A. 179 g • mol-1B. 8.00 g • mol-1C. 56.0 g • mol-1D. 28.0 g • mol-1E. 44.8 g • mol-1

Find out the volume contained by 6.8 g of ammonia at STP. (N=14, H=1)

Consider the following gas phase reaction:2NO(g) + O2(g) → 2NO2(g)400. mL of NO at STP is reacted with 500. mL of O2 at STP. Calculate the volume of the reaction mixture at STP after the reaction goes to completion.a. 700 mLb. 800 mLc. 900 mLd. 1300 mLe. 100 mL

If sufficient acid is used to react completely with 21.0 grams of Mg
Mg(s) + 2HCl(aq) → MgCl2(aq) + H2(g)
what volume of hydrogen at STP would be produced?
1. 9.68 liters
2. 19.37 liters
3. 10.60 liters
4. 22.40 liters
5. 4.84 liters

A hypothetical rock was harvested from another planet. Trapped inside was a diatomic gas. A volume of 1.25 mL of the gas was extracted from the rock at STP. The mass of the gas sample was determined to be 2.12 mg. Identify the gas.1. oxygen2. None of these3. hydrogen4. nitrogen5. fluorine

Standard conditions (STP) is defined as1. 273.15 K, 760 torr.2. 0 K, 250 atm.3. 100 K, 1 torr.4. 273.15 K, 250 torr.5. 0 K, 1 atm.

A sample of helium (He) occupies 4 liters at STP. What pressure is necessary to change the volume to 2 liters at 20°C?
1. 2.1464 atm
2. 2.0 atm
3. 2.36 atm
4. 4.361 atm
5. 4.0 atm

Assuming ideal behavior, what is the density of argon gas at STP, in g/L?a) 0.0176 g/Lb) 0.0250 g/Lc) 1.63 g/Ld) 1.78 g/Le) 181. g/L

A 574cm3 volume of Na2CO3 solution was warmed with an excess of sulfuric acid until all action ceased. A 9.0 L volume of dry CO2 gas measured at STP was given off and collected. What was the molarity of the sodium carbonate solution?a) 0.30b) 0.40c) 0.50d) 0.60e) 0.70

What is the density of Xe gas at STP? Give your result in g/L.a. 0.00156b. 64.0c. 5.86d. 5.37e. 0.178

A mixture of hydrogen and helium is 25.0% hydrogen by mass. What is the partial pressure of hydrogen (in atm) in the mixture at STP?a) 0.460b) 0.399c) 0.520d) 0.250e) 0.380

Which of the following gases has the greatest density at STP?A) NO2 (molar mass = 46.01 g/mol)B) Xe (molar mass = 131.3 g/mol)C) SO2 (molar mass = 64.07 g/mol)D) SF6 (molar mass = 146.07 g/mol)E) All of these samples have the same density at STP.

Which of the following samples will have the greatest volume at STP?a. 22 g Neb. 22 g Hec. 22 g O2d. 22 g Cl2 e. All have the same V at STP

Arrange the following gases in order of decreasing density at STP. Rank from largest to smallest.F2O2Cl2Ne

Using the graph below, determine the gas that has the lowest density at STP.A) AB) BC) CD) DE) All of the gases have the same density at STP.

Use the molar volume of a gas at STP to calculate the density (in g/L) of nitrogen gas at STP.

If the density of a gas 1.43 g/L at STP, what is the molecular weight of the gas?

Which of the following gases has the largest density at STP?a. Heb. C2H2 c. F2d. N2e. H2

When aluminum is placed in concentrated hydrochloric acid, hydrogen gas is produced.
What volume of H2(g) is produced when 6.2g of Al(s) reacts at STP?

How many grams of phosphorus react with 35.5 L of O 2 at STP to form tetraphosphorus decoxide?P4(s) + 5O2(g) ⟶P4O10(s)

Air bags are activated when a severe impact causes a steel ball to compress a spring and electrically ignite a detonator cap. This causes sodium azide (NaN3) to decompose explosively according to the following reaction:2NaN3(s) → 2Na(s) + 3N2(g)What mass of NaN3(s) must be reacted to inflate an air bag to 70.0 L at STP?

Ethanol, C2H5OH, is produced industrially from ethylene, C2H4, by the following sequence of reactions:3C2H4 + 2 H2SO4 ⟶ C2H5HSO4 + (C2H5)2SO4 C2H5HSO4 + (C2H5)2SO4 + 3 H2O ⟶ 3 C2H5OH + 2 H2SO4What volume of ethylene at STP is required to produce 1.000 metric ton (1000 kg) of ethanol if the overall yield of ethanol is 90.1%?

An unknown diatomic gas has a density of 3.164 g/L at STP. What is the identity of the gas?

An organic compound contains C, H, N, and O. Combustion of 0.1023 g of the compound in excess oxygen yielded 0.2766 g CO2 and 0.0991 g H2O. A sample of 0.4831 g of the compound was analyzed for nitrogen by the Dumas method (see Exercise 129). At STP, 27.6 mL of dry N2 was obtained. In a third experiment, the density of the compound as a gas was found to be 4.02 g/L at 127°C and 256 torr. What are the empirical and molecular formulas of the compound?

At STP, 1.0 L Br2 reacts completely with 3.0 L F2, producing 2.0 L of a product. What is the formula of the product? (All substances are gases.)

The effect of chlorofluorocarbons (such as CCl2F2) on the depletion of the ozone layer is well known. The use of substitutes, such as CH3CH2F(g), for the chlorofluorocarbons, has largely corrected the problem. Calculate the volume occupied by 10.0 g of each of these compounds at STP:(a) CCl2F2(g)

A 4.0-L vessel containing N2 at STP and a 2.0-L vessel containing H2 at STP are connected by a valve. If the valve is opened allowing the two gases to mix, what is the mole fraction of hydrogen in the mixture?

A mixture of 0.200 g of H2, 1.00 g of N2, and 0.820 g of Ar is stored in a closed container at STP. Find the volume of the container, assuming that the gases exhibit ideal behavior.

A sample of Freon-12 (CF2Cl2) occupies 25.5 L at 298 K and 153.3 kPa. Find its volume at STP.

How many moles of gaseous arsine (AsH 3) occupy 0.0400 L at STP? What is the density of gaseous arsine?

Consider a 1.0-L container of neon gas at STP. Will the average kinetic energy, average velocity, and frequency of collisions of gas molecules with the walls of the container increase, decrease, or remain the same under each of the following conditions?b. The temperature is decreased to -50°C.

At STP, what is the mass 13.0 L of methane, CH 4?a. 0.580 gb. 16.0 gc. 9.31 gd. 27.6 ge. 22.4 g

How many moles of neon occupy a volume of 14.3L at STP?

Standard temperature and pressure (STP), in the context of gases, refers to __________.a. 298.15 K and 1 atmb. 273.15 K and 1 atmc. 298.15 K and 1 torrd. 273.15 K and 1 pascale. 273.15 K and 1 torr

What is the molar mass of an unknown hydrocarbon whose density is measured to be 1.97 g/L at STP?

Lithium reacts with nitrogen gas according to the reaction: 6 Li(s) + N2(g) → 2 Li3N(s)What mass of lithium (in g) reacts completely with 58.5 mL of N2 gas at STP?

How many grams of phosphine (PH 3) can form when 37.5 g of phosphorus and 83.0 L of hydrogen gas react at STP?P4(s) + H2(g) ⟶ PH3(g) [unbalanced]

If a reaction occurs in the gas phase at STP, we can determine the
mass of a product from the volumes of reactants. Explain.

When aluminum is placed in concentrated hydrochloric acid, hydrogen gas is produced.2Al (s) + 6HCl (aq) → 2AlCl3 (aq) + 3H2 (g) What volume in L of H2 (g) is produced when 7.40 g of Al (s) reacts at STP?

Consider the reaction between Mg(s) and HCl(aq) to produce aqueous magnesium chloride and hydrogen gas. What volume of hydrogen at STP will be produced when 12.15 g of magnesium reacts with an excess of hydrochloric acid?A. 1.00 LB. 2.00 LC. 5.6 LD. 11.2 LE. 22.4 L

How many moles of O 2 (molar mass = 32.00 g/mol) are needed to react completely with 52.0 L of CH4(g) at STP to produce CO 2 and H2O? (molar mass (CH 4) = 16.04 g/mol)a) 11.6b) 2.32c) 4.64d) 52.0e) 104

At STP, what is the volume of 4.50 moles of nitrogen gas?A) 167 LB) 3420 LC) 101 LD) 60.7 L

Use the molar volume of a gas at STP to calculate the density (in g/L) of oxygen gas at STP.

An open flask sitting in a lab fridge looks empty, but we know that actually it is filled with a mixture of gases called air. If the flask volume is 1.50 L, and the air is at standard temperature and pressure, how many gaseous molecules does the flask contain?

What volume will 0.543 moles of He occupy at STP?(A) 41.3 L (B) 13.3 L (C) 12.2 L (D) 22.4 L (E) 1.11 L

Calculate the volume occupied by 56.5 g of argon gas at STP. a) 22.4 L b) 31.7 L c) 34.6 L d) 1, 270 L e) 1, 380 L

The density of a gas is 1.96 g/L at STP. What would the mass of 2.00 moles of the gas be at STP?1. 87.8 g2. There is not enough information to solve.3. 44.8 g4. 0.0875 g5. 43.9 g6. 0.510 g

An herbicide is found to contain only C, H, N, and Cl. The complete combustion of a 100.0-mg sample of the herbicide in excess oxygen produces 83.16 mL of CO2 and 73.30 mL of H2O vapor at STP. A separate analysis shows that the sample also contains 16.44 mg of Cl.Calculate its empirical formula.

A 2.45-L flexible flask at 15°C contains a mixture of N2, He, and Ne at partial pressures of 0.283 atm for N2, 0.151 atm for He, and 0.425 atm for Ne. (a) Calculate the total pressure of the mixture in atm.(b) Calculate the volume in liters at STP occupied by He and Ne if the N 2 is removed selectively.

Which of the following samples has the greatest density at STP?a. SO2b. Arc. SF6d. NOe. He

Consider a 1.0-L container of neon gas at STP. Will the average kinetic energy, average velocity, and frequency of collisions of gas molecules with the walls of the container increase, decrease, or remain the same under each of the following conditions?c. The volume is decreased to 0.5 L.

Consider the following questions:(a) What is the total volume of the CO2(g) and H2O(g) at 600 °C and 0.888 atm produced by the combustion of 1.00 L of C2H6(g) measured at STP?

What volume of O2 at STP is required to oxidize 8.0 L of NO at STP to NO2? What volume of NO2 is produced at STP?

Which gas sample has the greatest volume at STP?a. 20g of Neb. 2g of H2c. 8g of Hed. 20 g of N2

When 35.6 L of ammonia and 40.5 L of oxygen gas at STP burn, nitrogen monoxide and water form. After the products return to STP, how many grams of nitrogen monoxide are present? NH 3(g) + O2(g) ⟶NO(g) + H2O(l) [unbalanced]

The density of a certain gaseous fluoride of phosphorus is 3.93 g/L at STP. Calculate the molar mass of this fluoride and determine its molecular formula.

A student adds 4.00 g of dry ice (solid CO2) to an empty balloon. What will be the volume of the balloon at STP after all the dry ice sublimes (converts to gaseous CO2)?

If 6.00 mol of an ideal gas at STP were confined to a cube, what would be the length in cm of an edge of this cube?

An herbicide is found to contain only C, H, N, and Cl. The complete combustion of a 100.0-mg sample of the herbicide in excess oxygen produces 83.16 mL of CO2 and 73.30 mL of H2O vapor at STP. A separate analysis shows that the sample also contains 16.44 mg of Cl.Determine the percent composition of the substance.

Consider the following reaction:4Al(s) + 3O2(g) → 2Al2O3(s)It takes 2.00 L of pure oxygen gas at STP to react completely with a certain sample of aluminum. What is the mass of aluminum reacted?

A gas sample at STP contains 1.26 g oxygen and 1.76 g nitrogen.What is the volume of the gas sample?

An aerosol spray can with a volume of 250 mL contains 2.30 g of propane gas (C3H8) as a propellant.What volume would the propane occupy at STP?

A sample of oxygen gas has a volume of 2.50 L at STP. How many grams of O2 are present?

Calculate the volume of 63.5 g of carbon monoxide at STP. Report your answer to one decimal place!

If the density of an ideal gas at STP if found to be 0.716 g/L, what is its molar mass?

Calculate the density of oxygen, O2, under each of the following conditions: STP1.00 atm and 35.0°C Express your answers numerically in grams per liter. Enter the density at STP first and separate your answers by a comma. density at STP, density at 1 atm and 35.0°C = _____

A sample of carbon dioxide gas (CO2) has a volume of 2.5 L at standard temperature and pressure (STP). How many molecules of carbon dioxide gas are in the sample?

Be sure to answer all parts.How many moles of gaseous arsine (AsH3) occupy 0.273 L at STP? What is the density of gaseous arsine?

Enter your answer in the provided box.A sample of Freon-12(CF2Cl2) occupies 10.0 L at 293 K and 128.00 kPa. Find its volume at STP.

Dilute aqueous hydrogen peroxide is used as a bleaching agent and for disinfecting surfaces and small cuts. Its concentration is sometimes given as a certain number of “volumes hydrogen peroxide,” which refers to the number of volumes of O2 gas, measured at STP, that a given volume of hydrogen peroxide solution will release when it decomposes to O2 and liquid H2O. How many grams of hydrogen peroxide are in 0.100 L of “20 volumes hydrogen peroxide” solution?

A 1-L sample of CO initially at STP is heated to 546 K, and its volume is increased to 2 L.(a) What effect do these changes have on the number of collisions of the molecules of the gas per unit area of the container wall?

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