A 1.00 L rigid cylinder contains one mole of neon gas at 25 °C. Calculate the pressure using (a) the ideal gas law, and (b) the van der Waals equation (c) A much more accurate equation is the virial equation, В (Т) + Vm С (Т) pVm 1+ RT where B(T) and C(T) and C(T) are 11.42 cm3 mol1 and 221 cm6 mol2, respectively. Assuming the pressure calculated using the virial equation is the "true" value, determine the percent error by using ideal gas law and van der Waals equation are functions of temperature. For neon at 25°C, the values of B(T)

A 1.00 L rigid cylinder contains one mole of neon gas at 25 °C. Calculate the pressure using (a) the ideal gas law, and (b) the van der Waals equation (c) A much more accurate equation is the virial equation, В (Т) + Vm С (Т) pVm 1+ RT where B(T) and C(T) and C(T) are 11.42 cm3 mol1 and 221 cm6 mol2, respectively. Assuming the pressure calculated using the virial equation is the "true" value, determine the percent error by using ideal gas law and van der Waals equation are functions of temperature. For neon at 25°C, the values of B(T)

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

Similar questions

A scuba diver’s tank contains 0.30 kg oxygen (O2) compressed into a volume of 2.32 L.(a) Use the ideal gas law to estimate the gas pressure inside the tank at 5°C, and express it in atmospheres and in pounds per square inch.(b) What volume would this oxygen occupy at 30°C and a pressure of 0.98 atm?
The average kinetic energy of the molecules in a gas sample depends only on the temperature, T. However, given the same kinetic energies, a lighter molecule will move faster than a heavier molecule, as shown in the equation for rms speed 3 RT rms speed where R = 8.314 J/ (mol·K) and M is molar mass in kilograms per mole. Note that a joule is the same as a kilogram-meter squared per second squared (kg-mIs²). What is the rms speed of O, molecules at 307 K? rms speed: m/s What is the rms speed of He atoms at 307 K? rms speed: m/s
0.17 moles of hydrogen gas and 0.33 moles of nitrogen gas are created from thereaction 2NH3 (g) → 3H2 (g) + N2 (g). The final total pressure in the reaction vessel is0.75 atm. Calculate the partial pressure of the hydrogen gas at the end of the reaction.Assume the number of moles of NH3 (g), left after the reaction occurs, is negligible.
An “empty" spray can contains residual propellant gas that has a pressure of 772 torr at 23°C. The can is then heated to 475 °C. (a) What is the gas pressure in the hot can if the volume remains constant? (b) What is the gas pressure in the hot can if the can slightly expands during heating and its volume increases by 6.50%?
Consider an ideal gas mixture of 0.50 g H2 and 4.00 g N2 in a 1.00 L flask at 25 oC. (a) Calculate the partial pressure of each gas, (b) the mole fraction for each gas, and (c) the average molecular weight of the gas.
A sample of 3.42 mol of xenon is confined at low pressure in a volume at a temperature of 86 °C. Describe quantitatively the effects of each of the following changes on the pressure, the average kinetic energy per molecule in the gas, and the root-mean-square speed. (a) The temperature is increased to 199 °C (b) The volume is tripled. (c) The amount of xenon is decreased to 1.87 mol Give each answer as a decimal factor of the form: new value factor old value. A factor of 1 means no change. ChangeP KEavgms
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
A sample of an ideal gas at 1.00 bar and a volume of 1.91 L1.91 L was placed in a weighted balloon and dropped into the ocean. As the sample descended, the water pressure compressed the balloon and reduced its volume. When the pressure had increased to 60.0 bar,60.0 bar, what was the volume of the sample? Assume that the temperature was held constant.
4.) (a) 0.375 g of CO2 gas is held in a 520.-mL container at 24. oC. What is its pressurre? atm (b) 0.375 g of N2 are held in an identical container at the same temperature. What is its pressure? atm (c) Are the pressures the same or different? Why? (d) If both these samples were contained in the same 520.-mL container, what would the partial pressure of each gas be? What would the total pressure be? (FYI, these gases do not react.) PCO2= atm PN2= atm…
11. (a) In a 20.0 L steel container, we have only 77.7 g of CO2(g), 66.6 g of N2(g), and O2(g). The temperature is 25.0 ◦C and the total pressure is 8.88 atm. What mass of O2(g) do we have, and what is its partial pressure? The molar masses of C, N, and O are 12.01, 14.01, and 16.00 g/mol. (b) The density of a sample of pure CH4(g) at a constant pressure of 1.00 atm is 0.666 g/L. What is the average speed, or root mean square speed, of the CH4(g) molecules in this sample? The molar masses of C and H are 12.01 and 1.01 g/mol.
Liquid water can be decomposed into hydrogen and oxygen under suitable conditions (e.g., electrolysis) via the balanced reaction: 2H2O(l) -> 2H2(g) +O2(g) If an experiment generates 2500 cm3 of H2 gas, what volume of O2 is generated under the same conditions of temperature and pressure?