Two students were discussing about the Linde's process, when one of them suggested that Liquefaction of a gas dependsstrongly on two factors. The other student then asked the following questions related to the Liquefaction of gases:(a) What are those two factors? As the temperature is decreased from 700K, which gas will liquefy first-ammonia, methane, orcarbon dioxide? Give reasons?(b) Calculate the rms speed of a sample of 2-butene (C4H8) at 20 oC?(c) A technician connected two balloons together joined by stopcock as shown below. The 3.0 L balloon contains "He" at apressure of 4.0 atm and the other one contains 1.0 L NH3 at a pressure 1.0 atm. Calculate the total pressure of the system afterthe stopcock is opened. Assume the temperature remains constant.

The two factors on which liquification of gases depends are: Temperature Pressure Temperature: At…

Answered: Two students were discussing about the…

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...

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A 0.265 g sample of a metal, M, reacts completely with sulfuric acid according to M(s) + H,SO,(aq) → MSO,(aq) + H,(g) A volume of 277 mL of hydrogen is collected over water; the water level in the collecting vessel is the same as the outside level. Atmospheric pressure is 756.0 Torr, and the temperature is 25 °C. The vapor pressure of water at 25 °C is 23.8 Torr. Calculate the molar mass of the metal. molar mass: g/mol
[ A 1.00 L bottle of carbonated cola contains 5.20 g of carbon dioxide dissolved in it. If the evaporating carbon dioxide is trapped in a cylinder at 1.00 atm and 21.0°C, what volume (in L) does the gas occupy? ] V = nRT/P is the correct equation, I believe. [T = 21.0 C + 273.15 = 294.15 K ; P = 1.00 atm ; R = 0.08206 L*atm/mol*K] How do I properly convert 5.2 g of carbon dioxide to n?
A 7.40 g sample of solid Ni(CN), ·4H,0 was heated such that the water turned to steam and was driven off. Assuming ideal behavior, what volume would that steam occupy at 1.00 bar and 100 °C? It may be useful to consult the periodic table. volume: L
A 355 cm^3 sample of air saturated with water vapor at 27 degrees celsius generates a total pressure of 775 mmHg. How many grams of O2 are present in the sample, given that water has a vapor pressure of 26.7 mmHg and air can be assumed to be 20% O2 and 80% N2?
Predict whether the effects of molecular volume and of intermolecular attractions become more or less significant when the following changes are imposed: (a) A gas is expanded to a larger volume at constant temperature. Intermolecular attractions are significant, and molecular sizes are v significant. (b) More gas is introduced into a container of constant volume at constant temperature. Intermolecular attractions are significant, and molecular sizes are significant. more (c) The temperature of a gas increases at constant pressure. less Intermolecular attractions are significant, and molecular sizes are significant.
A 35.1 g sample of solid CO2 (dry ice) is added to a container at a temperature of 100 K with a volume of 4.0 L. If the container is evacuated (all of the gas removed), sealed and then allowed to warm to room temperature (T=298 K) so that all of the solid CO2 is converted to a gas, what is the pressure inside the container
An empty flask weighs 130.084 g. After vaporization of a sample of volatile liquid at a temperature of 100.0 °C, the flask was sealed, cooled to room temperature, and found to have a mass of 130.316 g. The atmospheric pressure was 759.7 mm Hg. The flask was rinsed and completely filled with water at 18.0 °C. The mass of the water-filled flask was determined to be 379.551 g. What is the pressure of the gas that fills the flask in atmospheres? (Enter your answer as a number without units.)
A 0.483 g sample of a metal, M, reacts completely with sulfuric acid according to M(s) + H,SO,(aq) MSO, (aq) + H, (g) A volume of 209 mL of hydrogen is collected over water; the water level in the collecting vessel is the same as the outside level. Atmospheric pressure is 756.0 Torr, and the temperature is 25 °C. The vapor pressure of water at 25 °C is 23.8 Torr. Calculate the molar mass of the metal. molar mass: g/mol
Consider the following chemical reaction: 2Al(s) + 3H₂SO4 (aq) → Al₂(SO4)3 (aq) + 3H₂ (g) A student collected 316 mL of hydrogen gas over water at a temperature of 29.0 °C and an atmospheric (total) pressure of 771 torr. The vapor pressure of water at 29.0 °C is 30.0 torr. Calculate the mass (g) of aluminum metal required to produce the hydrogen gas.
In addition to filling in the blanks below, show all of your work for this problem on paper for later upload. Lithium hydroxide, LİOH, is used in spacecraft to re-condition the air by absorbing carbon dioxide exhaled by astronauts as shown in the reaction: 2 LIOH(s) + CO2(g) → Liz CO3(s)[+ H2O(1) What volume of carbon dioxide gas at 21.0 °C and 781 mm Hg could be absorbed by 327 g LIOH? Enter your value in the first box and an appropriate unit of measure in the second box.
For many purposes we can treat ...monia (NH3) as an ideal ga temperatures above its boiling point of -33. °C. Suppose the pressure on a 650. mL sample of ammonia gas at 9.00°C is reduced to one-third its initial value. Is it possible to change the temperature of the ammonia at the same time such that the volume of the gas doesn't change? If you answered yes, calculate the new temperature of the gas. Round your answer to the nearest °C. O yes O no °C Ô
Sulfuric acid is essential to dozens of important industries from steelmaking to plastics and pharmaceuticals. More sulfuric acid is made than any other industrial chemical, and world production exceeds 2.0 × 10¹¹ kg per year. The first step in the synthesis of sulfuric acid is usually burning solid sulfur to make sulfur dioxide gas. Suppose an engineer studying this reaction introduces 3.1 kg of solid sulfur and 10.0 atm of oxygen gas at 800. °C into an evacuated 70.0 L tank. The engineer believes K = 0.98 for the reaction at this temperature. Calculate the mass of solid sulfur he expects to be consumed when the reaction reaches equilibrium. Round your answer to 2 significant digits. Note for advanced students: the engineer may be mistaken in his belief about the value of K, and the consumption of sulfur you calculate may not be what he actually observes. p' kg ☐ x10 ×

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