Gaseous and liquid states Questions and Answers

(1pts) (1pts) 23. Use the ideal gas law to solve for the pressure that is present in 2.34 moles of gas, at a temperature of 285 Kelvin and a volume of 50.0 Liters. 24. Use the ideal gas law to solve for the temperature of a gas that is kept at 1.41 atm and 24.3 Liters, containing 0.85 moles. Report the temperature in °C. (2pts) 25. Examining the ideal gas law, if a sample of gas is kept with constant number of moles and constant temperature, if you increased the pressure what would happen to the volume of the gas? Saved

Match the vocabulary words. 1. mixture that separates into individual components with time 2. composed of dissimilar parts which can be separated easily two or more substances dispersed in one another but each retaining their own identity 3. mixture in which the suspended particles are too small to be seen with the naked eye 5. a homogeneous mixture, usually a liquid with some substance dissolved in it 6. not easily separated into individual components 4. suspension heterogeneous homogeneous colloid mixture solution

- Boyle's law. Let's return our balloon to the room again, where it's 26°C. Now imagine that you take an empty 0.500 L plastic pickle jar and gently push the balloon inside the jar. Now screw on the lid. What will happen to the pressure inside the balloon when you close the lid? (a) Circle the correct words in the parentheses to complete the following sentence. The pressure in the balloon will (increase/decrease) (slightly/dramatically). In this experiment (volume/temperature/amount of gas) (is/are) constant. it. (b) Write an equation using the information from (a) that compares the initial state of the balloon and to its final state. P1V1= P2V2 (c) Calculate the new pressure (in torr) using the ideal gas law or the equation written | from your answer in (b). P=?atm V1=0.500 L (d) Now explain the change in pressure based on the behavior of the gas molecules. (e) Fill in the blank Boyle's law (1662): At constant temperature, the volume of a given amount of a gas is inversely porportional to the pressure exerted on

00432 = 3340 temperature of a sample of an ideal gas in a sealed 5.0 L container is raised from 27 °C to 77 °C. If the initial pressure The of the gas was 3.0 atm, what is the final pressure in torr? -5.0L V6

2. Boyle's law. Let's return our balloon to the room again, where it's 26°C. Now imagine that you take an empty 0.500 L plastic pickle jar and gently push the balloon inside the jar. Now screw on the lid. What will happen to the pressure inside the balloon when you close the lid? (2 pts/0.4 each) (a) Circle the correct words in the parentheses to complete the following sentence. The pressure in the balloon will (increase/decrease) (slightly/dramatically). In this experiment (volume/temperature/amount of gas) (is/are) constant. (b) Write an equation using the information from (a) that compares the initial state of the balloon and to its final state. P1V1= P2V2 Subscripts 1 represent the initial state, and the subscripts 2 represent the final state. (c) Calculate the new pressure (in torr) using the ideal gas law or the equation written from your answer in (b). P=?atm V1=0.500 L

The melting point of benzene is 5.5 °C and its boiling point is 80.1 °C. T Part C What is the state of benzene at 63 °C? boiling solid O O liquid gas melting Submit Part D What is the state of benzene at 98 °C? melting boiling Osolid Ogas liquid Request Answer Submit Request Answer

The flowrate in a 1.50-meter tube is believed to be 1.15 x 10 m³/s at a pressure of 75600 Pa. What is the radius of this vessel? Assume 1-0.00150 Pa.s. Show your work and report your answer to 3 significant figures.

Calculate the total pressure at a depth of 75.0 meters below the surface of the Dead sea. The density of water in this region is 1240 kg/m³, and the average atmospheric pressure is 106658 Pa. Show your work and report your answer to 3 significant figures.

A soda bottle is flexible enough that the volume of the bottle can change even without opening it. If you have an empty soda bottle (volume of 20 cL) at room temperature (25°C), what will the new volume be if you put it in your freezer (-4°C)?

A 10.0-ml solution of H₂SO4 (aq) solution is titrated with 0.254 M NaOH (aq). The equivalence point of the titration is 47.35 mL. a. What is the mass percent of H₂SO4 (aq) in solution? Assuming its density is 1.0 g/mL.

A 5.0-mL sample of aqueous HCl requires 16.52 mL of 0.245 M NaOH to reach the equivalence point. What is the molar concentration of HCl? The equation for the reaction is HCl(aq) + NaOH(aq)⇒NaCl(aq) + H₂O(1)

A teacher gives a student a non-toxic, odorless, white powder to identify. Generate five questions, each regarding a different property of the unknown powder, that could be safely tested and answered in the laboratory.

How many moles of tin atoms are in a pure tin cup with a mass of 40.3 g ? Express your answer in moles to three significant figures.

Dichlorodifluoromethane (CCl₂F2, also known as Freon-12) used to be used as refrigerant, but is banned due to the evidence that it destroys the ozone layer. If the total pressure of a mixture of 14.0 g of Freon-12 gas and 22.0 g of oxygen gas is 846 mm Hg. What is the (a) mole fraction and (b) partial pressure of each gas? [Xfreon-12 = 0.144, Xo₂= 0.856, Pfreon-12 = 122 mm Hg, Po₂ = 724 mm Hg]

Which sentence explains why gases can change volume but liquids cannot? A. Gravity affects liquid atoms more than gas atoms. B. The forces holding a liquid together are more flexible than those in a gas. C. The forces holding atoms together are stronger in a liquid than in a gas. D. Liquid atoms are more like solid atoms than gas atoms.

Given the equation below, how many grams of iron are required to produce 4.50 L of hydrogen gas, measured at 1.15 atm and 29.0° C? Fe + 2HCI- FeCl₂ + H₂

Calculate the root-mean-square velocity, in m/s, for a neon atom at 15.3 °C. The universal gas constant, R=8.314 J/mol K.

An unknown gas effuses at a rate of 2.00 times the rate of Cl₂. What is the molar mass of the unknown gas?

In addition to the heating curve above, you know the following information for this substance: • The Heat of Fusion is 29.8 cal/g • The Heat of Vaporization is 97.3 cal/g • The Specific Heat in the liquid phase is 0.299 cal/g °C Question: If you have 17.5 grams of this substance in the solid state at 14 °C (Point B), how much total heat energy (in calories) is required to completely transform it into a gas at 83 °C (Point E)?

Carbon dioxide gas is collected in a laboratory experiment to determine the molar mass of the compound. At 294 K and 1.01 atm, 1.008 g of CO2 was collected when a 500 mL flask was filled with the evolved CO2. What is the experimental molar mass of CO₂?

For a given ideal gas at constant temperature: Pressure is always constant. The product of pressure and volume always remains constant. Volume is always constant. The difference of pressure and volume always remain constant.

Gases are located in the exterior layer of the earth because they are lighter. false true

Which of the following is not the best explanation for the bursting of a hot air balloon? Both the outside temperature and pressure drop as the balloon rises. A drop in temperature causes the volume of an enclosed gas to decrease. The drop in outside pressure causes the volume to increase. None of the choices

At constant temperature and pressure, if 0.4 mole of a gas A occupies 220 mL and x mole of B gas occupies 120 mL, what is the number of moles of gas in the container that holds them B? 0.29 mol 0.22 mol 22.8 mol 2.2 mol

Perform the following additions and subtractions and express the answer in the correct number of significant figures. (5 point per answer, 10 points total). Show work for partial credit. 47400mL-138.1mL = 34000.mg +25.5g + 35.467g =

Counting Atoms 1. How many atoms in 5.3 moles of gold? 2. How many molecules are there in 5.25 mol of ethanoic acid? 3. How many moles of carbon in 1.5 x 1026 atoms? 4. How many formula units in 3.25 moles of CaCl₂? 5. If you have 8.25x 1025 atoms of iron, how many moles do you have? 6. How many formula units in 6.2 moles Al2(SO4)3? 7. How many atoms in 9.5 moles of copper? 8.4.9 x 10^22 atoms of iron is how many moles? 9. How many molecules in 0.5 moles of oxygen gas ? 10. 7.5 x 10^26 atoms of sulfur is how many moles?

Calculate the number of Li atoms (NLi) in 3.7 mol of Li. Express your answer using two significant figures.

Use the following vapor pressure data to answer the questions: Liquid Vapor Pressure, torr Temperature, °C A C3H7OH 400 82.0 B C2H5NH2 400 2.0 (1) In which liquid are the intermolecular attractive forces the strongest ? (2) The vapor pressure of C3H7OH at 2.0 °C would be ______ than 400 torr.

Now consider whether this relationship holds true for a process more complex than simple gas speed: diffusion. Use the molar masses of NH3 and HCI to calculate the predicted ratio of their molecules' speeds.

What volume of oxygen gas is produced when 22.6 g of mercury(II) oxide reacts completely according to the following reaction at 25 °C and 1 atm?

A Martian visiting planet Zook has a breathing tank pressurized to 240 kPa with a mixture of carbon dioxide, oxygen and hydrogen. The partial pressure of the CO2 is 20 kPa and the partial pressure of the O2 is 50 kPa. What is the partial pressure of the hydrogen? (Answer = 170 kPa)

A sample of neon gas at a pressure of 0.744 atm and a temperature of 27.0 °C, occupies a volume of 13.8 liters. If the gas is atm. allowed to expand at constant temperature to a volume of 22.6 liters, the pressure of the gas sample will be

When a solution of NaOH is neutralized by hydrochloric acid, the solution gets hot. Calculate the temperature change of the solution (in K). Mass of combined solution = 185 g Heat change of the solution=8890 J Specific heat capacity of the solution = 4.18 J/g-K Give your answer to three significant figures.

How many grams of carbon disulfide are needed to completely consume 85.3 L of chlorine gas according to the following reaction at 25 °C and 1 atm? carbon disulfide (s) + chlorine (g) carbon tetrachloride (1) + sulfur dichloride (s)

Consider the following five gases: Gas 1: H₂Se(g) Gas 2: CH3NH₂(g) Gas 3: C₂H6(g) Gas 4: NO₂F(g) Gas 5: CH3PF₂(g) Which gas would have the highest rate of effusion? Which gas would have the lowest rate of effusion? For each answer, explain how you know.

Milk of magnesia is a suspension of magnesium hydroxide in water. Although Mg(OH)2 is relatively insoluble, a small amount does dissolve in the water, which makes the mixture slightly basic and gives it a pH of 10.08. How many grams of Mg(OH)2 are actually dissolved in 4.5 tablespoons of milk of magnesia?

Which compound has a greater mass percent of oxygen, Na₂CO3 or Fe(NO3)3? What information do we need to find the mass percent of oxygen in each compound? total number of atoms in each compound mass of each element (use 1 mol of each compound) Avogadro's number, 6.022 x 1023 oxygen atoms 1 mol oxygen atoms molar mass of each compound number of protons in each element of the compound

An equilibrium mixture contains 0.350 mol of each of the products (carbon dioxide and hydrogen gas) and 0.200 mol of each of the reactants (carbon monoxide and water vapor) in a 1.00 L container. CO(g) + H₂O(g) = CO₂(g) + H₂(g) How many moles of carbon dioxide would have to be added at constant temperature and volume to increase the amount of carbon monoxide to 0.300 mol once equilibrium has been reestablished?

What volume of hydrogen gas is produced when 45.0 g of iron reacts completely according to the following reaction at 25 °C and 1 atm? iron (s) + hydrochloric acid(aq)→iron(II) chloride (aq) + hydrogen (g)

A solution is made using 65.1 g of hexane (MM = 86.18 g/mol) and 60.0 g of octane (MM = 114.2 g/ mol). What is the mole fraction of the hexane in the solution?

A sample of helium gas at a pressure of 0.890 atm and a temperature of 148°C, occupies a volume of 425 mL.If the gas is heated at constant pressure until its volume is 721 mL, the temperature of the gas sample will be °C

Aluminum sulfate, Al2(SO4)3, is used in some antiperspirants. Part B How many moles of aluminum ions (A1³+) are present in 0.50 mol of Al2(SO4)3? Express the number of moles to two significant figures. Part C How many moles of sulfate ions (SO4²-) are present in 2.0 mol of Al2(SO4)3?

A balloon is filled to a volume of 7.25 x 102 mL at a temperature of 23.0°C. The balloon is then cooled at constant pressure to a temperature of 1.24 x 10² K. What is the final volume of the balloon?

For the following reaction, 28.6 grams of carbon disulfide are allowed to react with 93.6 grams of chlorine gas carbon disulfide(s) + chlorine(g) - → carbon tetrachloride(1) + sulfur dichloride(s) What is the maximum amount of carbon tetrachloride that can be formed? What is the FORMULA for the limiting reagent? What amount of the excess reagent remains after the reaction is complete?

Ba(OH)2 8H₂O(s) + NH4SCN(s) → Ba(SCN)2 (8) + H₂O(l) +SH3(g) In this equation, the 8H₂O in Ba(OH)2 8H₂O indicates the presence of eight water molecules. This compound i barium hydroxide octahydrate. a. Balance the equation. (Use the lowest possible coefficients for the reaction.) Ba(OH)2 8H₂O(s) + NH4SCN(S) H₂O(l) + Ba(SCN)2 (s) + NH3(g) b. What mass of ammonium thiocyanate (NH4SCN) must be used if it is to react completely with 7.7 g bax hydroxide octahydrate? Mass= g

Liquid hexane (CH₂(CH₂) CH₂) reacts with gaseous oxygen gas (O₂) to produce gaseous carbon dioxide (CO₂) and gaseous water (H₂O). If 107. g of carbon dioxide is produced from the reaction of 85.31 g of hexane and 487.5 g of oxygen gas, calculate the percent yield of carbon dioxide.

When 5.738 grams of a hydrocarbon, CxHy, were burned in a combustion analysis apparatus, 18.00 grams of CO₂ and 7.372 grams of H₂O were produced. In a separate experiment, the molar mass of the compound was found to be 28.05 g/mol. Determine the empirical formula and the molecular formula of the hydrocarbon. Enter the elements in the order presented in the question.

A helium-filled weather balloon has a volume of 684 L at 16.9°C and 755 mmHg. It is released and rises to an altitude of 6.00 km, where the pressure is 428 mmHg and the temperature is -19.1°C. The volume of the balloon at this altitude is L

A gaseous system has an initial volume of 59.0 L and an initial pressure of 204.3 kPa. The system is compressed to 179 L. What is the new pressure of the system? Do not include units in your answer, it is presumed to be in kPa. Ensure that you answer accurately and round your answer to the nearest hundredth. Your Answer:

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? 58.6 L 45.0L 87.5L 11.4L 22.2 L