Give correct detailed Solution Calculate the pressure exerted by 2.57 moles of CO₂ confined in a volume of 4.13 L at 449 K. Use both the van der Waals equation and the ideal gas equationto calculate two pressure values.atm Lmol²Be sure your answer has the correct number of significant digits.The van der Waals constants for CO₂ are a=3.59Part 1 of 2van der Waals equation: atmPart 2 of 2Ideal gas equation: atmx10Xx10X2Sand b=0.0427ŚLmol

Moles of CO2 = 2.57 molVolume = 4.13 LTemperature = 449 Ka = 3.592 b = 0.0427 L/mol

Calculate the pressure exerted by 2.57 moles of CO₂ confined in a volume of 4.13 L at 449 K. Use both the van der Waals equation and the ideal gas equation. to calculate two pressure values. The van der Waals constants for CO₂ are a = 3.59 atm-L² mol² and b=0.0427 L mol

Calculate the pressure exerted by 2.57 moles of CO₂ confined in a volume of 4.13 L at 449 K. Use both the van der Waals equation and the ideal gas equation. to calculate two pressure values. The van der Waals constants for CO₂ are a = 3.59 atm-L² mol² and b=0.0427 L mol

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter8: Properties Of Gases

Section: Chapter Questions

Problem 71QRT

See similar textbooks

Related questions

Q: Find the % of sodium carbonate in a sample if 5.002 g of the sample required 29.10 cm³ of 0.7344 mol…

Q: AICI 12051 3.1 Strong i=4

A: Ionic compounds ionizes in aqueous solution and produce cation and anion. As for example,AB3 is a…

Q: I'm sorry, the solution is incorrect

Q: Determine if the entropy increases or decrease during the following processes and determine fhe…

Q: A chemistry student weighs out 0.0977 g of phosphoric acid (H,PO,), a triprotic acid, into a 250. mL…

A: First find the molarity of phosphoric acid and then by using the formula of concentration, find…

Q: Give detailed Solution with explanation needed..give the name of given compound

A: IUPAC stands for International Union of Pure and Applied Chemistry. It is an international…

Q: Use the References to access important values if needed for this question. The concentration of…

A: This titration is an example of a redox titration because oxidation states of species are changing.…

Q: Write the balanced reaction equation for aqueous ammonia and acetic acid forming aqueous ammonium…

Q: EXPLAIN ACID/BASE EXTRACTION IN DETAIL USING TERMS LIKE SOLUBILITY, POLARITY, SOLUTE, SOLVENT, AND…

A: Acid/base extraction is a common technique used in chemistry to separate and purify compounds based…

Q: Identification Complete each statement. Write your answer at the end of each question. 98. It is the…

A: In analytical analysis various methods are used in different purpose. Here we have to find out…

Q: A stock solution of approximately 7.7x10^-5 molar will be provided in lab. Determine the volumes of…

A: Given: Initial concentration of stock solution = 7.7 X 10-5 M And volume of final solution to be…

Q: Which 0.500 M solution will be the least conductive? Choose all that apply. A.Glucose B.Sodium…

A: The conductivity of a solution is directly proportional to the number of ions present in the…

Q: statement that correctly describes the hydronium-hydroxide balance?

A: Given : We have to explain statement that correctly describes the hydronium-hydroxide balance.

Q: Mass of Sample Volume of KMnO, solution used in titration Equivalents of permanganate used…

A: Titration is a convenient way of determining the concentration of an unknown solution by treating it…

Q: What volume of a 0.186 M calcium hydroxide solution is required to neutralize 11.8 mL of a 0.255 M…

A: Given: concentration of calcium hydroxide = 0.186 M concentration of hydroiodic acid = 0.225 M…

Q: I was told that answer is incorrect. Is there another possible solution?

Q: Compare the three main purification methods (recrystallization, distillation, and extraction) by…

A: The three main purification methods are recrystallization, distillation, and extraction.. With the…

Q: Solid potassium sulfide is slowly added to 150 mL of a 0.277 M nickel(II) iodide solution until the…

A: Number of mols = molar concentration× Volume in L= molar concentration× Volume in ml1000 Ksp of NiS…

Q: in text form with proper workings and explanation for each and every part and steps with concept and…

A: 6. some of the elements which dissolve in water to cause hardness are calcium carbonate (CaCO₃)…

Q: [References] A I:1 mixture by moles of nitrous oxide and oxygen is often used as a sedative in…

A: Given: Total pressure = 3.75 atm mole ratio of N2O and O2 = 1 : 1

Q: To determine the concentration of a solution of hydrochloric acid, a 125.0-mL sample is placed in a…

A: Using Molarity equation M1V1 = M2V2 [Ba(OH)2]…

Q: H3C. CI CH3 CH3

A: It is elimination reaction.Elimination reactions are commonly known by the kind of atoms or groups…

Q: 1.H₂O*, heat 2. Neutralizing work-up NH

A: The given reactant is a secondary amide.Now, when a secondary amide is hydrolyzed, a carboxylic acid…

Q: Could I get a paper version of the solution with better steps?

Concept explainers

Kinetic-Theory of Gases

Kinetic theory of gases is the model or method which was developed in the 19th century by Maxwell and Boltzmann. This is possible as the interatomic force which is of short-range forces that are important for solids and liquids can be neglected for gases. This theory or gas law gives a molecular interpretation of the pressure and temperature of a gas and is consistent with gas laws and Avogadro’s hypothesis. This theory is very helpful to correctly explain the specific heat capacities of many gases, kinetic energy and it also explains the transport qualities such as viscosity, thermal conductivity, and diffusion with molecular parameters. As stated in the kinetic-molecular theory, the temperature of a substance or gas particle is related to the average kinetic energy of the particles of that substance. When a substance is heated, some of the absorbed energy is stored within the particles, while some of the energy increases the motion of the particles, called average kinetic energy.

Question

Give correct detailed Solution

Calculate the pressure exerted by 2.57 moles of CO₂ confined in a volume of 4.13 L at 449 K. Use both the van der Waals equation and the ideal gas equation
to calculate two pressure values.
atm L
mol²
Be sure your answer has the correct number of significant digits.
The van der Waals constants for CO₂ are a=3.59
Part 1 of 2
van der Waals equation: atm
Part 2 of 2
Ideal gas equation: atm
x10
X
x10
X
2
S
and b=0.0427
Ś
L
mol

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

SEE SOLUTION Check out a sample Q&A here

Step 1: Determine the given variables.

VIEW

Step 2: Write the Gas equation.

VIEW

Step 3: Calculation of pressure of real gas.

VIEW

Step 4: Calculation of pressure of ideal gas.

VIEW

Solution

VIEW

Step by step

Solved in 5 steps with 5 images

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

Describe the factors responsible for the deviation of the behavior of real gases from that of an ideal gas.
A mixture at 33 °C contains H2at 325 torr. N;at 475 tore and O2at 650. torr. What is the total pressure of the gases in the system? Which gas contains the greatest number of moles?
Pressures of gases in mixtures are referred to as partial pressures and are additive. 1.00 L of He gas at 0.75 atm is mixed with 2.00 L of Ne gas at 1.5 atm at a temperature of 25.0 C to make a total volume of 3.00 L of a mixture. Assuming no temperature change and that He and Ne can be approximated as ideal gases, what are a the total resulting pressure, b the partial pressures of each component, and c the mole fractions of each gas in the mix?
A 1.000-g sample of an unknown gas at 0C gives the following data: P(atm) V (L) 0.2500 3.1908 0.5000 1.5928 0.7500 1.0601 1.0000 0.7930 Use these data to calculate the value of the molar mass at each of the given pressures from the ideal gas law (we will call this the apparent molar mass at this pressure). Plot the apparent molar masses against pressure and extrapolate to find the molar mass at zero pressure. Because the ideal gas law is most accurate at low pressures, this extrapolation will give an accurate value for the molar mass. What is the accurate molar mass?
99 Pure gaseous nitrogen dioxide (NO2) cannot be obtained, because NO2dimerizes, or combines with itself, to produce a mixture of NO2 and N2O4. A particular mixture of NO2, and N2O4 has a density of 2.39 g/L at 50°C and 745 torr. What is the partial pressure of NO2 in this mixture?
Under what conditions does the behavior of a real gas begin to differ significantly from the ideal gas law?
Hydrogen gas is used in weather balloon because it is less expensive than Helium. Assume that 5.57 g of H2 is used to fill a weather balloon to an initial volume of 67 L at 1.04 atm. If the ballloon rises to an altitude where the pressure is 0.047 atm, what is its new volume? Assume that the temperature remains constant.
Consider a 5.00-L tank containing 375 g of Ar at a temperature of 25 C. (a) Calculate the pressure in the tank using both the ideal gas law and the van der Waals equation. (b) Which correction term, a(n/V)2 or bn, has the greatest influence on the pressure of this system?
Calculate the molar volume of ethane at 1.00 atm and 0C and at 10.0 atm and 0C, using the van der Waals equation. The van der Waals constants are given in Table 5.7. To simplify, note that the term n2a/V2 is small compared with P. Hence, it may be approximated with negligible error by substituting nRT/P from the ideal gas law for V in this term. Then the van der Waals equation can be solved for the volume. Compare the results with the values predicted by the ideal gas law.
A 1.26-g sample of a gas occupies a volume of 544 mL at 27 C and 744 torr? What is the molecular formula and name of the gas if its empirical formula is C2H5.
A 0.245-L flask contains 0.467 mol CO2 at 159 C. Calculate the pressure: (a) using the ideal gas law (b) using the van der Waals equation (c) Explain the reason for the difference. (d) Identify which correction (that for P or V) is dominant and why.
Shown below are three containers of an ideal gas (A, B, and C), each equipped with a movable piston (assume that atmospheric pressure is 1.0 atm). a How do the pressures in these containers compare? b Are all the gases at the same temperature? If not, compare the temperatures. c If you cooled each of the containers in an ice-water bath to 0.0C, describe how the volumes and pressures of the gases in these containers would compare.