Gaseous and liquid states Questions and Answers

If you inflate a balloon from an initial volume of 5 mL to a final volume of 455 mL against an atmospheric pressure of 754 torr, how much work is done by the gas (in Joules)? (1 atm = 760 torr)

A cylinder contains 27.5 L of oxygen gas at a pressure of 1.7 atm and a temperature of 301 K. Part A How many moles of gas are in the cylinder?

A gas sample with a volume of 5.3 L has a pressure of 745 mm Hg at 26 °C. Part A What is the pressure of the sample if the volume remains at 5.3 L but the temperature rises to 96 °C?

What change in pressure occurs in a party balloon that is squeezed to one-third its volume with no change in temperature?

Your friend of mass 60 kg can just barely float in fresh water. Y Part A Calculate her approximate volume.

An open flask sitting in a lab refrigerator looks empty, but it is actually filled with a mixture of gases called air. If the flask volume is 4.00 L, and the air is at standard temperature and pressure, how many gaseous molecules does the flask contain? number of gaseous molecules:

A gas cylinder that contains argon has an internal volume of 6.88 L. A pressure gauge attached to the cylinder reads 1890 psi (1 atm = 14.7 psi) at 20.4 °C. What mass of argon is contained in the cylinder? mass= 6.1) g

A flexible container at an initial volume of 6.13 L contains 8.51 mol of gas. More gas is then added to the container until it reaches a final volume of 11.1 L. Assuming the pressure and temperature of the gas remain constant, calculate the number of moles of gas added to the container. number of moles of gas: mol

A mixture of argon and neon has a measured gas density of 1.145 g/L at STP. Assuming ideal-gas behavior, what is the average molar mass of the mixture? average molar mass of the mixture : g/mol

How many moles of gas must be forced into a 3.1 L ball to give it a gauge pressure of 9.6 psi at 21 °C? The gauge pressure is relative to atmospheric pressure. Assume that atmospheric pressure is 14.7 psi so that the total pressure in the ball is 24.3 psi. Express your answer in moles to two significant figures.

How many moles of gas does the cylinder contain? (Hint: You must convert each quantity into the correct units (L, atm, mol, and K) before substituting the ideal gas law.) Express your answer with the appropriate units. 72= HA Value Units ?

Identify the statement that describes Dalton's law of partial pressures. The total pressure exerted by a mixture of gases is equal to the quotient of the partial pressures of the individual gases. The total pressure exerted by a mixture of gases is equal to the product of the partial pressures of the individual gases. O The total pressure exerted by a mixture of gases is equal to the difference between the partial pressures of the individual gases. The total pressure exerted by a mixture of gases has no relation to the partial pressures of the individual gases. O The total pressure exerted by a mixture of gases is equal to the sum of the partial pressures of the individual gases.

Adding helium to a balloon increased its volume from 483.4 mL to 3.668 L. If the final number of moles of helium in the balloon is 31.7 mol, what was the initial number of moles of helium in the balloon? Assume the balloon contained only helium initially. n= mol

A sample of gas contains equal moles of helium, neon and krypton gases, at a particular temperature. a) Which gas has the greatest partial pressure?: The partial pressures are the sa b) Which gas particles have the greatest kinetic energy? b) Which gas molecules have the greatest average veloci He [Select] [Select] He Ne Ar The kinetic energies are all the same

Determine the pressure exerted by 2.10 mol of gas in a 2.92-L container at 32°C. a. 16.1 atm b. 5.51 atm c. 18.0 atm d. 52.6 atm e. 1.89 atm

A non-flexible container has a pressure of 740mmHg with 30 particles trapped inside. It is in a room where the temperature is 205 K. The continer is moved to a room at 195K and the number of particles is increased to 50 particles. What will be the new pressure inside the container? **Round your answer to two decimal places! Remember to use a VnTP table!

What is the formula for copper(II) phosphate? Capitalization and punctuation count. formula: How many atoms of phosphorus are in 5.90 mol of copper(II) phosphate? number of P atoms =

You are a nurse and you have several patients that need treatment. Thank goodness you were taught how to manipulate gas laws in order to help the patients. Help each patient solve the issue they are encountering. Patient B needs nitrous oxide (N₂O) before surgery, and you have to figure out if there is enough nitrous oxide in the cylinder. How many moles of nitrous oxide is in a cylinder of 9.0kg (6kg when empty) at standard temperature and pressure?

A sample of gas in a closed non-flexible container has a pressure of 16.6 atm and a temperature of 200 K. What is the new pressure (in atm) when the temperature rises to 300 K? Include units on your answer. Remember to use a VnTP table!

MISSED THIS? Watch KCV 11.4. IWE 11.5: Read Section 11.7. You can click on the Review link to access the section in your e Text. A 0.14 mol sample of nitrogen gas occupies a volume of 2.15 L. Part A What is the volume of 0.30 mol of nitrogen gas under the same conditions? Express your answer volume to two significant figures.

If the volume of the gas is increased to 5.39 L, what is the pressure? (Assume constant temperature.) Express your answer in millimeters of mercury to three significant figures.

A balloon with an initial volume of 3.4 L at a temperature of 292 K is warmed to 396 K. Y Part A What is its volume at 396 K?

A snorkeler with a lung capacity of 4.6 L inhales a lungful of air at the surface, where the pressure is 1.0 atm. The snorkeler then descends to a depth of 21 m. where the pressure increases to 3.1 atm. Y Part A What is the capacity of the snorkeler's lungs at this depth? (Assume constant temperature.)

The solubility of a solute is best described as which of the following? the ability of the solute to dissociate into ions when dissolved in water the moles of solute that can dissolve in 1 L of solution the maximum amount of solute that can be dissolved in a specified amount of solvent the ability of the solute to dissolve in water the mass of solute necessary to dissolve in 1 L of water

Which of the following is a statement of Dalton's law of partial pressure? The partial pressure of a gas is equal to the total pressure of the mixture. Gases can exist as mixtures at STP only. In a mixture of two gases, the pressure of each gas is ½ the total pressure. The total pressure of a mixture of gases is the product of the partial pressures of each gas in the mixture. The total pressure of a mixture of gases is the sum of the partial pressure of each gas that makes up the mixture.

A flask with a sample of gas at room temperature and pressure weighs 97.4842 g. The same flask with air (density = 1.17 g/L) weighs 96.8848 g. The same flask filled with water (d = 0.998 g/mL) weighs 345.86 g. The pressure in the room is 0.989 atm and the temperature is 22.2 °C. Calculate the volume of the flask. Calculate the mass of the air that the flask can hold. Calculate the mass of the empty (no air) flask. Calculate the mass of the gas in the flask. Use the ideal gas law to calculate the moles of gas in the flask. Calculate the molar mass of the gas in the flask.

NH,CI(s) → NH₂Cl(aq), ΔH = 14.8 kJ/mol If 44.1 g of NH CI is dissolved in 215 g of water at 31.0°C, determine the final temperature of the solution. The specific heat capacity of the solution is 4.18 J/g°C.

Determine the molar mass of each of the following gases: Part C 0.786 g of a gas that occupies 875 mL at 1.30 atm and 19 °C. Express your answer with the appropriate units. M = Part D 2.28 g of a gas that occupies 1.38 L at 685 mmHg and 17 °C. Express your answer with the appropriate units. M =

At constant pressure the temperature of a 4.00 L sample of gas is increased from 25 °C to 50. °C. What is the new volume of the gas sample?

A 0.220 g sample of carbon dioxide, CO2, has a volume of 574 mL and a pressure of 453 mmHg. Part A What is the temperature of the gas in kelvins? Express your answer to three significant figures. T = K Part B What is the temperature of the gas in degrees Celsius? Express your answer to three significant figures. T = °C

You may want to reference (Page) Section 11.9 while completing this problem. When Zn reacts with HCl solution, the products are H₂ gas and ZnCl₂: Zn(s) + HCl(aq)→H₂(g) + ZnCl2 (aq) A volume of 447 mL of H₂ gas is collected over water at a total pressure of 729 mmHg and 16 °C. The vapor pressure of water at 16 °C is 14 mmHg. What was the partial pressure of the H₂ gas? Express your answer to three significant figures and include the appropriate units. P= 715 mmHg

An air bubble has a volume of 0.520 L ar 19 C. You may want to reference (Page) Section 11.3 while completing this problem. What is the volume, in liters, at 420 K, if n and P do not change? Express the volume to two significant figures and include the appropriate units.

If two chemical samples both produce an orange flame upon testing, which of the following is true? The two samples contain identical compounds. The samples both contain chlorine atoms. The samples both contain calcium atoms. The samples both contain potassium atoms.

Almost every episode of the TV shows such as "Breaking Bad" ends with one of the characters in a predicament such as about to be caught by thugs, or about to be exposed by the authority. Which of the following techniques has been used in such narratives? Flash forward Cut-up technique Cliffhanger

All pressure-volume-temperature relationships for gases can be combined into a single relationship known as the combined gas law. This expression can be used when looking at the effect of changes in two of these variables on the third as long as the amount of gas (number of moles) remains constant. To use the combined gas law properly, you must always express the temperatures in kelvins. The combined gas law can be represented as follows: P₁V₁ Ti = P2V₂ T2 V₂ = 38.1 L Consider 4.40 L of a gas at 365 mmHg and 20. °C. If the container is compressed to 2.10 L and the temperature is increased to 31 °C, what is the new pressure, P2, inside the container? Assume no change in the amount of gas inside the cylinder. Express your answer with the appropriate units.

Bacteria and viruses are inactivated by temperatures above 145 °C in an autoclave. An autoclave contains steam at 1.00 atm and 100 °C. At what pressure, in atmospheres, will the temperature of the steam in the autoclave reach 145 °C, if n and V do not change?

Suppose water is raised by capillary action to a height of 4.55 cm in a glass tube. Refer to the angle values given in the table to answer the questions. Enter a positive number for height if the water is raised above the surrounding water level and a negative number if it is pushed below.

A 50.00 mL sample of Ca(OH)2 (aq) required 46.78 mL of 0.04498 M HCI (aq) for complete neutralization. Find the molarity of the original Ca(OH)2 (aq) solution. O a. 0.001052 M Ob. 0.02104 M c. 0.02104 M Od. 0.04208 M Oe. 0.08416 M

When an inflated balloon is untied in a room, the air inside rushes out of the balloon filling the room. The entropy of the air as the gas expands giving it greater freedom of of kinetic energy states. Treat the motion and allowing it to occupy -- balloon and its air as the system.

Ammonia gas has a molar mass of approximately 17 grams per mole. At 290K and 1.2 atm, a sample of ammonia has a volume of 3.7 L. In three to five sentences, explain how you can find the mass of the ammonia. Then, given R = the mass. 0.0821L-atm mol-K calculate

A gas has a volume of 182 mL, a temperature of 18°C, and a pressure of 283 mm Hg. If the temperature is held constant and the volume increases to 213 mL, what is the final pressure?

A gas, behaving ideally, has a pressure P₁ and at a volume V₁. The pressure of the gas is changed to P₂. Using Avogadro's, Charles', or Boyle's law, develop an expression that would be used to solve for the new volume V₂. ► View Available Hint(s) O P₁V₁= P₂V2 O V₁/P₁= V₂/P2 O P₁V₂ = P₂V₁ O P₁/V₁ = P2/V2

Which of the following equations is the combined gas law? P₁V₁/T₁= P₂V2/T2 V₁/T₁=V₂/T₂ P₁V₁= P₂V2 P₁/T₁= P2/T₂

5. The solubility of aspirin in water is 0.33 g per 100 mL at room temperature. Check the amount of water you used at your procedure to see how much water was used in washing, a) Calculate the maximum amount of aspirin that dissolved?

Classify each phase change based on whether it describes a transition between a gas and a liquid, a gas and a solid, or a liquid and a solid. condensation Gas and liquid deposition melting Gas and solid Answer Bank sublimation freezing evaporation Liquid and solid

What would happen to each of the properties if the intermolecular forces between molecules increased for a given fluid? Assume temperature remains constant. surface tension Increase vapor pressure boiling point Decrease Answer Bank viscosity Stay the same

8. A bag of potato chips contains 585 mL of air at 25°C and a pressure of 765 mm Hg. Assuming the bag does not break, what will be its volume at the top of a mountain where the pressure is 0.75 atm and a temperature of 5.0 °C?

Calculate the root mean square speed and average speed for a sample of gas having 5, 10 and 15 molecules each one in a set is moving with a speed of 15 x 102, 5 x 102 and 10 × 10² m s-1 respectively. A B C D 9.79 × 102 18.34 × 102 X 36 × 103 87 × 102 X

Calculate the pH for each case in the titration of 50.0 mL of 0.190 M HCIO(aq) with 0.190 M KOH(aq). Use the ionization constant for HCIO. What is the pH after addition of 40.0 mL KOH? pH= What is the pH after addition of 60.0 mL KOH? pH=

a. The average human takes in about 400 mL of air while breathing normally. If the weather outside is -10°C, how would this volume of air change as it warms in the lungs to body temperature of 37°C? 2 points