Gaseous and liquid states Questions and Answers

On hot days, you may have noticed that potato chip bags seem to "inflate", even though they have not been opened. If I have a 145 mL bag at a temperature of 23 °C, and I leave it in my car with a temperature of 29° C, what will the new volume, in mL, of the bag be?

Submarines need to be extremely strong to withstand the extremely high pressure of water pushing down on them. An experimental research submarine with a volume of 15,000 liters has an internal pressure of 1.8 atm. If the pressure of the ocean breaks the submarine forming a bubble with a pressure of 354 atm pushing on it, how big will that bubble be in liters?

According to Boyle's Law, the volume of a gas varies directly with its pressure when temperature is held constant. True False

15.1 L N₂ at 25 °C and 125 kPa and 33.5 L O₂ at 25 °C and 125 kPa were transferred to a tank with a volume of 5.25 L. What is the total pressure at 53 °C?

Which of these examples are liquids with high vapor pressure (evaporates easily)? A Rubbing alcohol, acetone, Butane, Propane Motor oil, maple syrup, honey C Mercury, water, glycerin Alcohol, vinegar, acetone

A chemist prepares a solution of nickel(II) chloride (NiCl₂) by measuring out 87. g of nickel(II) chloride into a 250. mL volumetric flask and filling the flask to the mark with water. Calculate the concentration in mol/L of the chemist's nickel(II) chloride solution. Be sure your answer has the correct number of significant digits.

The molar mass of a gas is determined as in the experiment described in Experiment 8. The mass is determined to be 2.01 g. The volume of the water, which is equal to the volume of the gas, is measured to be 243 mL, the boiling water temperature was 99.8°C and the barometric pressure was 755 mm Hg. Calculate the molar mass of the gas. Use 0.0821 L-atm/mol-K as the value of the ideal gas law constant, R. Enter the value of your answer only. The value you enter should be expressed in g/mol.

Multiple Choice: Read each question carefully and choose the letter of the best answer. Write your answer in your answer sheet. 1. What happens when chocolate melts? A. The particles of chocolate lose their orderly arrangement to form gas. B. The particles of chocolate lose their orderly arrangement to form liquid. C. The particles of chocolate keep their orderly arrangement to form liquid. D. None of these. 2. What happens when a chocolate drink freezes? A. It absorbs heat, and the particles lose kinetic energy. B. It releases heat, and the particles lose kinetic energy. C. It absorbs heat, and the particles lose potential energy. D. It releases heat, and the particles lose potential energy. 3. What happens when alcohol evaporates? A. It absorbs energy causing particles to vibrate faster. B. It absorbs energy causing particles to vibrate slower. C. It releases energy causing particles to vibrate faster. D. It releases energy causing particles to vibrate slower. 4. Which is TRUE about deposition? A. It is responsible in cloud formation B. It is responsible in snow formation C. It is the exact opposite of evaporation D. It occurs substance changes directly from solid to gas 5. Which is NOT TRUE about evaporation? A. It occurs when matter absorbs energy B. It occurs when gaseous substance turns to liquid C. It occurs when a substance turns from liquid to gas D. It occurs when the kinetic energy of the particles increases

A chemist prepares a solution of sodium nitrate (NaNO3) by measuring out 184. g of sodium nitrate into a 350. mL volumetric flask and filling the flask to the mark with water. Calculate the concentration in mol/L of the chemist's sodium nitrate solution. Be sure your answer has the correct number of significant digits.

Predict the trend of entropy in the following scenario: Entropy of helium v. entropy of Argon A Entropy is higher B Entropy is lower C No change in entropy

A sample of NO, occupies 16.500 mL at STP. How many NO2 molecules are in the sample? 1. 5.88 x 10 NO₂ molecules 2.9.11 x 1023 NO₂ molecules 3. 7.65 x 10 NO₂ molecules 4. 1. 13 x 10 NO₂ molecules 5.2.00 × 10²4 NO₂ molecules

Select the statements that are TRUE regarding mixing. Polar compounds can mix with polar compounds. Water can mix with non polar propane. Non polar compounds mix with polar compounds. Water can mix with polar HCI

The student collects the H₂(g) produced by the reaction and measures its volume over water at 298 K after carefully equalizing the water levels inside and outside the gas-collection tube, as shown in the diagram below. The volume is measured to be 45.6 mL. The atmospheric pressure in the lab is measured as 765 torr, and the equilibrium vapor pressure of water at 298 K is 24 torr. Calculate the following. (i) The pressure inside the tube due to the H₂(g) (ii) The number of moles of H₂(g) produced in the reaction

215.0 mol of an unknown gas is stored at a temperature of 1110 K in a large, 395 L container. In atm, what is the approximate pressure of the gas? R=0.0821 L-atm/(mol-K) 550 atm 0.020 atm 50.0 atm 180 atm 22.0 atm 7,700 atm

A syringe contains a sample of air at room temperature and pressure. Assuming no leaks in the syringe and no change in temperature, when the volume of the syringe is increased from 16 mL to 32 mL, the gas pressure in the syringe will one option from each menu. An Erlenmeyer flask contains a sample of air at room temperature and pressure. Assuming the flask does not leak, when the temperature of the flask is increased from 20 °C to 60 °C, the gas pressure within the flask will A balloon contains a sample of air at 1.00 atm and 40 °C. Assuming the balloon does not leak, when the temperature of the balloon is decreased from 40 °C to 10 °C at constant pressure, the volume of the balloon will

Gas properties involve four variables: n: amount of gas, in moles V: volume of gas, in liters P: pressure of gas, in atmospheres T: temperature of gas, in kelvins Although all four of these can change, many times it is convenient to compare gases using a set of "standard" conditions. In particular, we use standard temperature and pressure values and label those standard conditions STP. In the USA, most chemists, and most general chemistry texts, use STP = 0 °C and 1 atm, where the molar volume of any gas is 22.4 L/mol. If the reference pressure is chosen to be 1 bar, the molar volume is 22.7 L/mol. Do not confuse the two. This molar volume can be used as a convenient way of calculating amount (mol) from volume (or volume from amount) for gas samples at STP. STP (standard temperature and pressure) is used as a reference point for the molar volume of an ideal gas. In the USA, most chemists, most general chemistry texts, and OWL use STP = 0°C, 1 atm, where the molar volume = 22.4 L/mol. If the reference pressure is chosen to be 1 bar, the molar volume is 22.7 L/mol. Do not confuse the two. A 0.52 mol sample of hydrogen gas occupies a volume of L at STP.

What is the volume occupied by 2.0 moles of neon gas at STP? 5.6 L 44.8 L 22.4 L 11.2 L

The temperature of a flexible container of gas is raised from 100.0 °C to 175 °C and its pressure changes from 650.0 torr to 925 torr causing a new volume of 235 mL. What was the original volume of the container of gas?

A large balloon will burst at a volume of 420. L with a pressure of 0.465 atm. If the balloon is originally has a volume of 255 L with a pressure of 750. mm Hg at 22 °C, at what temperature (in °C) will the balloon burst?

The absorbance of an unknown solution was measured to be 0.315. Calculate the molar concentration of this solution if the path length, I = 1 cm, and & = 0.257 M-1cm-1. Report your answer to 1 DECIMAL PLACE

If I initially have gas at a pressure of 9.2 atm, a volume of 27.5 liters, and a temperature of 280. K, and then I raise the pressure to 12.8 atm and increase the temperature to 400. K, what is the new volume of the gas?

Answer the questions in the table below about the shape of the sulfur tetrabromide (SBr4) molecule. How many electron groups are around the central sulfur atom? Note: one "electron group" means one lone pair, one single bond, one double bond, or one triple bond. What phrase best describes the arrangement of these electron groups around the central sulfur atom? (You may need to use the scrollbar to see all the choices.)

A student obtained a clean, dry, glass stoppered flask. The weight of the flask and stopper was 32.634 g. The student filled the flask with water and obtained a mass for the full, stoppered flask of 59.479 g. The density of water at the temperature of the experiment was 0.9973 g/ml. Find the volume of the stoppered flask.

What is the pressure of the enclosed gas in (iii)? Assume that the gray liquid is mercury. Express your answer in atmospheres using three significant figures. In a closed-end manometer the pressure of the gas (Pgas) is equal to the height of Hg displaced, and thus Pgas Ph, where P is the pressure calculated from the height of the gray liquid.

A gas of unknown molecular mass was allowed to effuse through a small opening under constant- pressure conditions. It required 125 s for 1.0 L of the gas to effuse. Under identical experimental conditions it required 33 s for 1.0 L of O2 gas to effuse. Calculate the molar mass of the unknown gas. (Remember that the faster the rate of effusion, the shorter the time required for effusion of 1.0 L; that is, rate and time are inversely proportional.) Express your answer using two significant figures.

This question refers to the balanced equation below: 16 HCl(aq) + 2 K₂Cr₂O7(aq) + 3 CH₂OH(l)→ 4 CrC13(aq) + 3 CHO₂H(l) + 4 KCl(aq) + 11 H₂O(l) What is the mole ratio of CrCl3 to CHO₂H?

Calcium oxide reacts with water in a combination reaction to produce calcium hydroxide: CaO (s) + H₂O (l) → Ca(OH)2 (s) In a particular experiment, a 5.00-g sample of CaO is reacted with excess water and 6.11 g of Ca(OH)2 is recovered. What is the percent yield in this experiment? 122 1.22 7.19 92.5 81.9

Aqueous sulfuric acid (H₂SO4) will react with solid sodium hydroxide (NaOH) to produce aqueous sodium sulfate (Na₂SO) and liquid water (H₂O). Suppose 91.2 g of sulfuric acid is mixed with 38. g of sodium hydroxide. Calculate the maximum mass of sodium sulfate that could be produced by the chemical reaction. Be sure your answer has the correct number of significant digits.

A 114 mg sample of a non-electrolyte isolated from throat lozenges was dissolved in enough water to make 14.0 mL of solution at 21.7°C. The osmotic pressure of the resulting solution was 4.10 atm. Calculate the molar mass of the compound.

As you sit on the beach, you notice that the breeze, which had been blowing toward the water from the land, shifts so that it is blowing off the water toward land. What event has just occurred? The temperature over the water has become higher than the temperature over the land. The temperature over the land has become higher than the temperature over the water. Clouds have begun to form over the water. The temperature over the land has reached its highest point for that day.

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? a. The temperature is increased to 210°C. Average kinetic energy Average velocity The collision frequency b. The temperature is decreased to -30°C. Average kinetic energy Average velocity The collision frequency c. The volume is decreased to 0.7 L. Average kinetic energy Average velocity The collision frequency d. The number of moles of neon is doubled. Average kinetic energy Average velocity The collision frequency

An organic chemist measures the temperature T' of a solution in a reaction flask. Here is the result... T= 48.7 °C Convert T to SI units. Be sure your answer has the correct number of significant digits.

According to the ideal gas law, a 1.048 mol sample of xenon gas in a 1.042 L container at 273.4 K should exert a pressure of 22.56 atm. What is the percent difference between the pressure calculated using the van der Waals' equation and the ideal pressure? For Xe gas, a = 4.194 L²atm/mol² and b=5.105x10-2 L/mol.

Little amount of H₂O(l) is taken in a 2 litre vessel along with N₂(gas) (PN₂ = 0.5 atm ) now volume of vessel is doubled and total pressure is found to be 0.4 atm then find amount H₂O(l) liquid present initially in vessel? Given : Vapour pressure of water = 0.3 atm, temperatúre = 27°C (Constant) (neglect volume occupied by H₂O(e), R=1/12 Latm mol-¹ K-¹) 0.432 gram 0.23 gram 0.94 gram 1.23 gram

A reaction between liquid reactants takes place at 2.0 °C in a sealed, evacuated vessel with a measured volume of 30.0 L. Measurements show that the reaction produced 39. g of boron trifluoride gas. Calculate the pressure of boron trifluoride gas in the reaction vessel after the reaction. You may ignore the volume of the liquid reactants. Round your answer to 2 significant digits.

Determine the volume (L) of nitrogen monoxide gas that is created at STP when 32.2 g of solid copper reacts with excess nitric acid. 3Cu(s) + 8HNO3(aq) → 3Cu(NO3)2 (aq) + 4H₂O(l) + 2NO(g)

A weather balloon containing helium with a volume of 410.0 L rises in the atmosphere and is cooled from 170C to -270C. The pressure on the gas is reduced from 110.0 kPa to 25.0 kPa. What is the volume of the gas at the lower temperature and pressure? What law did you use to solve? Make sure to show all work, for partial credit if your answer happens to be incorrect.

The average lung capacity of a human is 5.9 L. How many moles of air are in your lungs when you are in the following situations? Assume air behaves ideally and has an average molar mass of 29.0 g/mol. a. At sea level (T = 298 K, P = 1.00 atm). b. 10 m below water (T = 298 K, P = 1.97 atm). c. At the top of Mount Everest (T= 199 K, P = 0.294 atm).

When it became too hot to stay outside during a summer birthday party, the party was moved inside to an air-conditioned porch. If a latex balloon has a volume of 5.00 L at 37 °C, what would be the volume of this balloon at 21 °C? Assume that the pressure does not change.

At 280 K, a gas has a volume of 1.5 L., and a pressure of 1.0 atm. The gas is heated to 490 K, and the pressure of the gas increases to 3.1 atm. What is the volume of the gas under these new conditions? a) 0.85 L b) 0.000034 L C) 1.2 L d) 1.4 L

2NaN3 (s) 3 N₂(g) + 2Na(s) The equation above is part of the reaction that occurs when an airbag inflates during a collision. The bag fills with nitrogen due to the decomposition of sodium azide. If an airbag fills with 3.75 mol of nitrogen gas, 1) how many moles of sodium azide decomposed? Answer: 2) what mass of pure sodium is also created? Answer: [Select]

Methane gas, CH4, effuses through a barrier at a rate of 0.433 mL/minute. If an unknown gas effuses through the same barrier at a rate of 0.261 ml/minute, what is the molar mass of the gas? 5.83 g/mol 0.172 g/mol 26.6 g/mol 9.67 g/mol 44.1 g/mol

2. An aerosol spray can with a volume of 250 mL contains 2.30 g of propane gas (C3H8) as a propellant. a. If the can is at, what is the pressure in the can? b. What volume would the propane occupy at STP? c. The can's label says that exposure to temperatures above may cause the can to burst. What is the pressure in the can at this temperature?

In an experiment, 2.000 grams of an unknown gas exert a pressure of 0.8876 atm in a 1.250 L container at 25.00°C. a. What is the molar mass of the gas? b. Is the gas propane (C3H8) or propylene (C3H6), explain your reasoning?

What is the density, in grams per liter, of a gas with a molar mass of 17.02 L atm at 285 K and 1.80 atm?

A sample of oxygen, O₂, occupies 38.1 mL at 41.0 °C and 489 torr. What volume, in milliliters, will it occupy at -72.0 °C and the same pressure? • Use -273.15 °C for absolute zero. • Report your answer using three significant figures.

A gas mixture contains 0.150 mol of oxygen (O₂) gas, 0.419 mol of nitrogen (N₂) gas. and 0.211 mol of argon (Ar) gas in a 0.250 L flask at 298 K. What is the total pressure of the mixture? • Report your answer with three significant figures.:

Combustion of hydrocarbons such as ethane (C₂H) produces carbon dioxide, a "greenhouse gas." Greenhouse gases in the Earth's atmosphere can trap the Sun's heat, raising the average temperature of the Earth. For this reason there has been a great deal of international discussion about whether to regulate the production of carbon dioxide. 1. Write a balanced chemical equation, including physical state symbols, for the combustion of gaseous ethane into gaseous carbon dioxide and gaseous water. 2. Suppose 0.400 kg of ethane are burned in air at a pressure of exactly 1 atm and a temperature of 17.0 °C. Calculate the volume of carbon dioxide gas that is produced. Round your answer to 3 significant digits.

A 5.00 L tank at 29.1 °C is filled with 16.8 g of boron trifluoride gas and 19.3 g of chlorine pentafluoride gas. You can assume both gases behave as ideal gases under these conditions. Calculate the mole fraction of each gas. Round each of your answers to 3 significant digits.

A sample of an unknown compound is vaporized at 170. °C. The gas produced has a volume of 1760. mL at a pressure of 1.00 atm, and it weighs 4.60 g. Assuming the gas behaves as an ideal gas under these conditions, calculate the molar mass of the compound. Round your answer to 3 significant digits.