E1C.3(a) A gas at 250 K and 15 atm has a molar volume 12 per cent smaller than that calculated from the perfect gas law. Calculate (i) the compression factor under these conditions and (ii) the molar volume of the gas. Which are dominating in the sample, the attractive or the repulsive forces? E1C.3(b) A gas at 350 K and 12 atm has a molar volume 12 per cent larger than that calculated from the perfect gas law. Calculate (i) the compression factor under these conditions and (ii) the molar volume of the gas. Which are dominating in the sample, the attractive or the repulsive forces?

E1C.3(a) A gas at 250 K and 15 atm has a molar volume 12 per cent smaller than that calculated from the perfect gas law. Calculate (i) the compression factor under these conditions and (ii) the molar volume of the gas. Which are dominating in the sample, the attractive or the repulsive forces? E1C.3(b) A gas at 350 K and 12 atm has a molar volume 12 per cent larger than that calculated from the perfect gas law. Calculate (i) the compression factor under these conditions and (ii) the molar volume of the gas. Which are dominating in the sample, the attractive or the repulsive forces?

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Related questions

Q: Three gases (8.00 gg of methane, CH4CH4, 18.0 gg of ethane, C2H6C2H6, and an unknown amount of…

A: We know that the gaas law is PV=nRT -----(i) where P is pressure of the system,V is…

Q: A mixture containing 0.250 mol N2 (g), 0.150 mol CH4 (g), and 0.100 mol O2 (g) is confined in a 1.00…

A: Moles of N2 = 0.250 mole CH4 = 0.150 mole O2 =0.100 mole

Q: A 1.00 L rigid cylinder contains one mole of neon gas at 25 °C. Calculate the pressure using (a) the…

A: a) ideal gas law : P = nRT/V Given: n = 1 T= 25o C = 25 + 273.15 = 298.15K V = 1 L R = 0.082057338…

Q: 1. A sample of air was compressed to a volume of 24.4 L. The temperature was 298 K and the pressure…

Q: The van der Waals equation of state was designed (by Dutch physicist Johannes van der Waals) to…

A: Please find your solution below : In van der waals equation, the parameters a and b are the…

Q: What is the density (in g/Lg/L) of hydrogen gas at 24 ∘C∘C and a pressure of 1670 psipsi?…

A: Density (d) =massvolume = mV

Q: The ideal gas law is PV = NkT, with k denoting the Boltzmann constant. It is important that the…

A: Ideal gas law is obtained by combining all the Gas laws to derive a common relation among all the…

Q: Your lungs are 5.23 L and 310.0 K at 1.01 atm. If 80.0% of the air is N2 and 20.0% is O2 what is the…

A: Since you have asked multiple questions, we will solve the first question for you. If you want any…

Q: When limestone (solid CaCO3) is heated, it decomposes into lime (solid CaO) and carbon dioxide gas.…

Q: The van der Waals equation of state was designed (by Dutch physicist Johannes van der Waals) to…

A: The van der-Waal's equation is given by (P+an2V2)(V-nb)=nRT R = gas constant n = number of moles of…

Q: The van der Waals equation of state was designed (by Dutch physicist Johannes van der Waals) to…

A: Since you have posted questions with multiple subparts, we are entitled to answer the first 3 only.…

Q: Be sure to answer all parts. (a) What is the total volume of gaseous products, measured at 350°C and…

A: 2 C8H18 (g)+ 25 O2 (g) → 16 CO(g) + 18 H2O (g)Volume of gaseous products = volume of CO2 , V1+…

Q: . What pressure would 131 g of Xe gas exert in a vessel of volume 1.0 dm³ at 25°C, if it ehaved like…

A: Answer:-This question is answered by using the simple concept of calculation of pressure using the…

Q: 313 K according to the reaction below. During the reaction, the pressure and temperature change. In…

A: The effect of pressure and temperature is measured by Boyle’s law and Charles's law respectively.…

Q: What are the units of a? What are the units of b? For argon the numerical value of a is 1.337 and…

A: Value of a = 1.337 b = 0.0320

Q: The Goodyear blimps, which frequently fly over sporting events, hold approximately 1.55×105 ft^3 of…

A: PV = nRT where P is pressure, V is volume, n is number of moles = mass/ molar mass R is gas constant…

Q: Calculate the pressure exerted in atm by 3.0 moles of ammonia when it is behaving as (a) a perfect…

A: Using Ideal gas equation are :---PV =nRTP is the pressure.V is the volume.n is the number of moles.R…

Q: 3. Rust is formed when iron gets oxidized by oxygen: 4 Fe (s) + 3 O₂(g) → 2 Fe₂O3(s) Calculate the…

Q: 2. A 0.500 g impure sample of LINO; is heated, causing it to decompose according to the following…

A: Given temperature = 300 K. 1 atm = 760 mm Hg. The pressure of the dry gas = 760 – 26.7 =733.3 mm Hg.

Q: If 1.00 molmol of argon is placed in a 0.500-LL container at 24.0 ∘C∘C , what is the difference…

Q: The van der Waals equation, nRT = [P + (n/V)2a)](v-nb) incorporates corrections to the ideal gas law…

A: Ideal gas law is PV = nRT Van der Waals equation is First-term accounts for the intermolecular…

Q: The product gas, C,H2, is collected over water at a temperature of 20 °C and a pressure of 745 mm…

Q: The van der Waals equation of state was designed (by Dutch physicist Johannes van der Waals) to…

Q: 4. Consider a sample of gas at 393 K and 22 atm. (a) Calculate the molar volume V (L/mol) of the…

Q: According to the ideal gas law, a 1.042 mol sample of methane gas in a 1.670 L container at 267.2 K…

Q: A 3.85 g sample of a KCl−KClO3 mixture is decomposed by heating and produces 117 mL O2(g), measured…

A: Given, V = 117 mL = 0.117 L as 1 mL = 0.001 L T = 23.5 + 273 = 296.5 K P = 110 kPa The value of R is…

Q: The van der Waals constants a and b are 5.489 L2 atm mole-1 and 0.0638 L mole-1 for C2H6. (a)…

A: Given, Vander Waals constant , a=5.489L2 atmmol2b=0.0638Lmol

Q: Constants R = 0.0821atmolmolK . 1atm = 760mmHs , 1 gas = 22.41 (STP) Hydrogen was prepared in 1776…

A: Since from the given reaction we can say that 3 moles of Fe is reacting to form 4 moles of H2 Hence…

Q: p/ bar Vm/L mol1 p/ gL1 Pressure 0.759938 0.506625 0.253313 Molar volume 29.8649 44.8090 89.6384…

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

A CamScanner 09-05-2021 08.01.p x
O File | C:/Users/taylo/OneDrive/Desktop/CamScanner%2009-05-2021%2008.01.pdf
(D Page view
A Read aloud
V Draw
E Highlight
O Erase
5
of 9
Scanned with CamScanner
E1C.3(a) A gas at 250 K and 15 atm has a molar volume 12 per cent smaller
than that calculated from the perfect gas law. Calculate (i) the compression
factor under these conditions and (ii) the molar volume of the gas. Which are
dominating in the sample, the astractive or the repulsive forces?
E1C.3(b) A gas at 350 K and 12 atm has a molar volume 12 per cent larger
than that calculated from the perfect gas law. Calculate (i) the compression
factor under these conditions and (ii) the molar volume of the gas. Which are
dominating in the sample, the attractive or the repulsive forces?
Scanned with CamScanner
O Ai
56°F Sunny ^
O G 1) 8:15 AM

Expert Solution

This question has been solved!

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

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

Step 2

Step 3

Step 4

Step 5

Step 6

Trending now

This is a popular solution!

Step by step

Solved in 6 steps

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

Question: provide the name of this molecule
The ideal gas law describes the relationship among the pressure P, volume V, number of moles n, and absolute temperature T of an ideal gas. Here is the relationship expressed mathematically: PV = nRT where R is a proportionality constant. The units of R are determined by the units of pressure and volume used in the equation. When bar used for pressure and L for volume, the appropriate R value is 0.08314 L bar mol-¹ K-¹. Part A How many air molecules are in a 4.05 x 3.66 x 3.05 m³ room? Assume atmospheric pressure of 1.00 bar, a room temperature of 20.0 °C, and ideal behavior. Express your answer using three significant figures. ► View Available Hint(s) VE ΑΣΦ + Review | Constants | molecules
Calculate the pressure exerted in atm by 3.0 moles of ammonia when it is behaving as (a) a perfect gas in atm at 25°C in 22.414L and (b) van der Waals (VDW) gas at 100°C in 1000.0 cm3. Given van der Waals constants: a(NH3) (L2.atm/mol2) = 4.17 and b(NH3)(L/mol) = 0.037. The pperfect gas = .............atm and pVDW = ................ atm 3 sig. figures normal format.
A sealed container holding 0.0255 L0.0255 L of an ideal gas at 99.526 kPa99.526 kPa and 73 °C73 °C is placed into a refrigerator and cooled to 37 °C37 °C with no change in volume. Calculate the final pressure of the gas.
Please help me to give you thumbs up
2.00L of carbon dioxide gas (the main component of the Martian atmosphere) is contained at a pressure of 101.3 kPa at room temperature (21oC) on Earth. The daytime temperature at the equator during summer on Mars is also 21oC. If the atmospheric pressure on Mars is 6.01 mmHg, what volume would the gas occupy on Mars?
Using (a) the ideal gas law and (b) the van der Waals equation, calculate the pressure exerted by 50.0 g carbon dioxide in a 1.00-L vessel at 25°C. Do attractive or repulsiveforces dominate?
Answer part a and b
I only need help with part b
5.69 You want to store 165 g of CO2 gas in a 12.5-L tank at room temperature (25°C). Calculate the pressure the gas would have using (a) the ideal gas law and (b) the van der Waals equation. (For CO2, a = 3.59 atm L^2/mol^2 and b = 0.0427 L/mol.)
The van der Waals equation of state was designed (by Dutch physicist Johannes van der Waals) to predict the relationship between pressure p, volume V and temperature T for gases better than the Ideal Gas Law does: 2 p+a (V-nb)=nRT The van der Waals equation of state. R stands for the gas constant and n for moles of gas. v? The parameters a and b must be determined for each gas from experimental data. Use the van der Waals equation to answer the questions in the table below. What are the units of a? What are the units of b? For ammonia the numerical value of a is 4.169 and the numerical value of b is 0.0371. atm Use the van der Waals equation to calculate the pressure of a sample of ammonia at 195.0 °C with a molar volume of 4.12 L/mol. Round your answer to 3 significant digits. Use the Ideal Gas Law to calculate the pressure of the same sample under the same conditions. Round this answer to 3 significant digits also. || atm O
Everything needed is included. An empty 1.0-liter cylinder is filled with 48.0 grams of methane (CH4 ) at 273 K. 2a. Predict (calculate) the pressure, assuming methane behaves as an ideal gas. 2b. Suppose the pressure is measured and is found to actually be 56 atm. Determine the compression factor Z, and indicate whether attractive or replusive intermolecular forces are dominant in methane under these conditions.