Concept explainers
Interpretation:
The mixture of helium (red) and argon (blue) when the temperature is lowered to
Concept Introduction:
Ideal gas equation is an equation that is describing the state of an imaginary ideal gas.
Where,
P is the pressure of the gas
V is the volume
n is the number of moles of gas
R is the universal gas constant
T is the temperature
Charles law,
Volume of the container is directly proportional to Temperature of the container
Where,
V=Volume
T=Temperature
Answer to Problem 9.26CP
The volume of the container will decreases when the temperature decreases.
Explanation of Solution
Given,
According to Charles law,
Volume of the container is directly proportional to Temperature of the container
Where,
V=Volume
T=Temperature
So the volume of the container will reduce to half.
When T=
Figure 1
When T=
Figure 2
The mixture of helium (red) and argon (blue) when the temperature is lowered to
Want to see more full solutions like this?
Chapter 9 Solutions
General Chemistry: Atoms First
- 1. Ammonia gas is produced by the reaction: N2(g) + 3H2(g) → 2NH3 (g). (a) How many liters of ammonia can be produced from 10.8 L of hydrogen? Assume that all gases were measured at a constant temperature and pressure. (b) If the reaction was made to occur at 2 atm pressure at 254 K, how many moles of ammonia were produced?arrow_forwardIn the Dumas-bulb technique for determining the molar mass of an unknown liquid, you vaporize the sample of a liquid that boils below 100 °C in a boiling-water bath and determine the mass of vapor required to fill the bulb (see drawing (Figure 1)). Part A unknown vapor, 1.013 g ; volume of bulb, 355 cm3 ; From the following data, calculate the molar mass of the unknown liquid: mass pressure, 742 torr ; temperature, 99 °C ΑΣφ. ? MM = g/mol Submit Request Answerarrow_forwardBefore small batteries were available, carbide lamps were used for bicycle lights. Acetylene gas, C2H2, and solid calcium hydroxide were formed by the reaction of calcium carbide, CaC2, with water. The ignition of the acetylene gas provided the light. Currently, the same lamps are used by some cavers, and calcium carbide is used to produce acetylene for carbide cannons. What volume (in L) of C2H2 at 1.014 atm and 11.9°C is formed by the reaction of 15.56 g of CaC2 with water?arrow_forward
- a) The densities of air at −85 °C, 0 °C, and 100 °C are 1.877 g dm−3, 1.294 g dm−3, and 0.946 g dm−3, respectively. From these data, and assuming that air obeys Charles’ law, determine a value for the absolute zero of temperature in degrees Celsius. b) A certain sample of a gas has a volume of 20.00 dm3 at 0 °C and 1.000 atm. A plot of the experimental data of its volume against the Celsius temperature, θ, at constant p, gives a straight line of slope 0.0741 dm3 °C−1. From these data alone (without making use of the perfect gas law), determine the absolute zero of temperature in degrees Celsius.arrow_forward1.44. The van der Waals constant b can be used to estimate molecular sizes, assuming the molecules are shaped like spheres: 1. Convert b to units of m³/mol, using the fact that 1 m³ = 1000 L. 2. Divide by Avogadro's number to get the individual molecular contribution to b. 3. Use V = 4/3 πr³ to estimate the radius of the molecule. Using these steps, estimate the sizes of (a) He (b) H₂O (c) C₂H6-arrow_forwardA balloon is filled with helium, and its volume is 2.2 L at 298 K. The balloon is then dunked into a thermos bottle containing liquid nitrogen. When the helium in the balloon has cooled to the temperature of the liquid nitrogen (77 K), so the final volume will be 0.57 L. The balloon in the example above will burst if its volume exceeds 2.3 L. At what temperature would you expect the balloon to burst? I hope this will be solved soon Thank you!arrow_forward
- How much potassium chlorate is needed to produce 20.0 mLmL of oxygen gas at 700. mmHgmmHg and 20. ∘C∘C? How do I do this?arrow_forward2. A 7.94 g piece of solid CO 2 (dry ice) is allowed to sublime in a balloon. The final volume of the balloon is 1.00 301 K. what is the pressure of the gas?arrow_forwardExplain how the volume of the bubbles exhausted by a scuba diver as shown change as they rise to the surface, assuming that they remain intact.arrow_forward
- Lithium metal reacts with molecular oxygen gas to form lithium oxide . A closed container of volume 4 .00 x 103 mL contains oxygen gas at 98 °C and 8.12 x 105 Pa. Then 12.5 g of solid lithium is introduced, and the reaction goes to completion. What is the final pressure (in bar) if the temperature rises to 125.5 °C?arrow_forwardFor many purposes we can treat ammonia (NH3) as an ideal gas at temperatures above its boiling point of −33. °C. Suppose the temperature of a sample of ammonia gas is lowered from 24.0 °C to - 19.0 °C, and at the same time the pressure is changed. If the initial pressure was 0.38 kPa and the volume increased by 35.0%, what is the final pressure? Round your answer to 2 significant digits. kPa x10 Xarrow_forwardA sample of an ideal gas at 1.00 atm1.00 atm and a volume of 1.24 L1.24 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 30.0 atm,30.0 atm, what was the volume of the sample? Assume that the temperature was held constant. V= Larrow_forward
- Chemistry: Matter and ChangeChemistryISBN:9780078746376Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl WistromPublisher:Glencoe/McGraw-Hill School Pub CoChemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage LearningChemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage Learning