An ideal gas in a sealed container has an initial volume of 2.45 L. At constant pressure, it is cooled to 15.00 °C, where itsfinal volume is 1.75 L. What was the initial temperature?T =°C* TOOLSx10 A flexible container at an initial volume of 4.11 L contains 9.51 mol of gas. More gas is then added to the container until itreaches a final volume of 14.3 L. Assuming the pressure and temperature of the gas remain constant, calculate the numberof moles of gas added to the container.number of moles of gas:mol* TOOLSx10

Answered: Image /qna-images/answer/0e309c4b-73d6-44d8-af1d-b54234fc48cb.jpg

An ideal gas in a sealed container has an initial volume of 2.45 L. At constant pressure, it is cooled to 15.00 °C, where its final volume is 1.75 L. What was the initial temperature? T = °C С ТOOLS x10

An ideal gas in a sealed container has an initial volume of 2.45 L. At constant pressure, it is cooled to 15.00 °C, where its final volume is 1.75 L. What was the initial temperature? T = °C С ТOOLS x10

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: A tank was filled with 12 g of oxygen (O2), 73 g of nitrogen (N2) and 4 g of carbon dioxide(CO2). At…

Q: Fe(s) + H2SO(aq) → FeS0.(aq) + H2(g) The volume of the balloon was 4.8 x10° L. What mass of Fe was…

A: Equation can be written as: Fe(s)+H2SO4→FeSO4(aq)+H2(g) Molar mass of Fe = 56 g/mol H2 = Molar mass…

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: Scuba divers who suffer from decompression sickness are treated in hyperbaric chambers using a gas…

A: Answer -

Q: Gases evolved from the fermentation of glucose in your home brew. At 20.1 oC and 0.86 atm you…

Q: 35.5 g O, in a 15.7 L container at 1.25 atm ☐ K x10

A: Given that,Mass of Molar mass of Volume of the gas= Pressure of the gas in the container=…

Q: For many purposes we can treat nitrogen (N2) as an ideal gas at temperatures above its boiling point…

Q: To identify a diatomic gas (X2X2), a researcher carried out the following experiment: She weighed an…

Q: For many purposes we can treat methane (CH4) as an ideal gas at temperatures above its boiling point…

A: The objective of the question is to calculate the final pressure.

Q: A cylinder is filled with 10.0 L of gas and a piston is put into it. The initial pressure of the gas…

Q: A cylinder of volume 27.0 L is filled with 25.1 g of jobstium gas (MM = 72.21 g - mol-1) from the…

A: Given data, Mass = 25.1 g Molar mass = 72.21 g/mol. To calculate the number of moles.

Q: A 5.00 L tank at 29.6 °C is filled with 17.3 g of boron trifluoride gas and 12.8 g of chlorine…

Q: Volume of acetic anhydride: 2.98 mL Mass of salicylic acid: 1.00 g Mass of aspirin recovered: 0.67…

A: Two sub-part question based on mole concept. For the synthesis of aspirin from acetic anhydride and…

Q: A canister containing 8g of helium gas (atomic mass 4.0 u) was used to fill up party balloons. When…

A: Answer: This question is based on ideal gas equation and we have to use it to find out the mass of…

Q: A 6.00 L tank at 27.5 °C is filled with 14.6 g of sulfur hexafluoride gas and 3.50 g of dinitrogen…

A: Step 1: Step 2: Step 3: Step 4:

Q: For many purposes we can treat butane (C₂H₁0) as an ideal gas at temperatures above its boiling…

A: At constant volume if the pressure of the gas is increased, the temperature will increase. This…

Q: For many purposes we can treat nitrogen 2) as an ideal gas at temperatures above its boiling point…

Q: Consider the reaction of 1.41 g Ca(s) with 107 mL of 0.325 M HBr(aq) according to the following…

A: The reaction taking place is given as, => Ca (s) + HBr (aq) -----> CaBr2 (aq) + H2 (g) Given :…

Q: Calculate to three significant digits the density of carbon dioxide gas at exactly 25 °C and exactly…

Q: A tank contains a mixture of 14.6 g of argon gas and 9.69 g of neon gas at 27 °C. The total pressure…

A: We are having 9.69g Neon & 14.6g Argonnoof moles of Neon present = weight of Neon(g)Molar mass…

Q: For many purposes we can treat butane (C4H10) a as an ideal gas at temperatures above its boiling…

A: Gay- Lusaac'a law : This law states that the pressure (P) of a fixed mass of gas held at a constant…

Q: Water decomposes according to the following reaction: 2 H2O (g) -> O2 (g) + 2 H2 (g). If 0.050 mol…

A: Given : Volume = 1L Moles of water = 0.050 moles Temperature = 298K

Q: Nitrogen dioxide (NO₂) cannot be contained in a pure form in the gas phase because it exists as a…

Q: Four gases, A, B, C and D, are mixed into a sealed container. The total pressure is 3.31. What is…

A: Total pressure of a mixture is the sum of partial pressure of its constituents.

Q: Combination of all four gas laws leads to the ideal gas law, PV = nRT Ris the ideal gas constant (R…

A: The question is based on ideal gas equation as mentioned in the question it self.…

Q: An unknown gas has a density of 1.48 g/L and a molar mass of 68.2 g/mol. You have measured the…

A: For the ideal gas, the temperature pressure and the volume are related by the ideal gas equation.…

Q: States of Matter = Using the combined gas law For many purposes we can treat butane (C4H10) as an…

A: The objective of the question is to determine if it is possible to change the temperature of butane…

Q: A gas with an initial volume of 2.00 L at 275.0 K is heated. The final volume is 3.000 L. Calculate…

Q: A 9.00 L tank at 11.1 °C is filled with 14.5 g of dinitrogen difluoride gas and 13.4 g of chlorine…

Q: To identify a diatomic gas (X2), a researcher carried out the following experiment: She weighed an…

A: According to the ideal gas law: PV = nRT where P, V, n, R and T represent pressure, volume, number…

Q: For many purposes we can treat ammonia NH3 as an ideal gas at temperatures above its boiling point…

A: Yes it is possible to change the temperature of ammonia at the same time keeping the volume of the…

Q: A 44.0 L metal cylinder stores a sample of gas at 6 °C under 1.02 atm. The temperature of the…

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

Q: To identify a diatomic gas (X2X2), a researcher carried out the following experiment: She weighed an…

A: Using the ideal gas equation, we can calculate the molar mass of the diatomic gas.

Q: For many purposes we can treat nitrogen (N2) as an ideal gas at temperatures above its boiling point…

A: The relationship between the temperature, pressure, and volume of the initial and final state of an…

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

A: Given,mass of methane gas ( CH4 ) = 8.00 gmass of ethane gas ( C2H6 ) = 18.0 gpressure = 3.50…

Q: Calculating partial pressure in a gas mixture A 8.00 L tank at 9.28 °C is filled with 6.17 g of…

A: The objective of this question is to calculate the mole fraction, partial pressure of each gas, and…

Q: The ideal gas law relates the amount of gas present to its pressure, volume, and temperature. The…

Q: For many purposes we can treat propane (C3Hg) as an ideal gas at temperatures above its boiling…

A: Answer:Here:

Q: Dry ice is solid carbon dioxide. A 1.47−g sample of dry ice is placed in an evacuated 4.37−L vessel…

A: in this question given data, dry ice means CO2, 44g/mole Volume = 4.37 1.47g of dry ice 27∘C…

Q: A 7.00 L tank at 6.54 °C is filled with 17.3 g of sulfur tetrafluoride gas and 17.7 g of chlorine…

A: Given : Mass of sulfur tetrafluoride i.e SF4 = 17.3 g Mass of chlorine pentafluoride i.e ClF5 = 17.7…

Q: app.101edu.co Question 34.c of 34 A sample of gas contains 5.25 moles at 37.8 °C in a volume of 3.61…

Q: For many purposes we can treat ammonia (NH,) as an ideal gas at temperatures above its boiling point…

A: The relationship between a fixed amount of gas's pressure, volume, and absolute temperature is…

Q: A piece of sodium metal reacts completely with water as follows: 2Na(s) + 2H,0(D→ 2NAOH(aq) + H2(g)…

A: Recall the given equation as follows 2Nas + 2H2Ol →2NaOHaq + H2g Again recall the ideal gas…

Q: A gas cylinder contains (6.9600x10^1) L of the gas argon when it is full. If the cylinder was at an…

A: Given: The pressure of the argon gas = 1.6700×103 kPa The volume of the argon gas = 6.9600×101 L The…

Concept explainers

Mole Concept

Mole concept is a method to determine the amount of any substance that consists of some elemental particles using a grouping unit called ‘mole’. The mole concept enables one to handle the large amount of small elementary particles. The mole concept can be used in many calculations related to mole calculation, molar amount, mole ratio, and so on, which are significant in chemistry.

Question

100%

An ideal gas in a sealed container has an initial volume of 2.45 L. At constant pressure, it is cooled to 15.00 °C, where its
final volume is 1.75 L. What was the initial temperature?
T =
°C
* TOOLS
x10

A flexible container at an initial volume of 4.11 L contains 9.51 mol of gas. More gas is then added to the container until it
reaches a final volume of 14.3 L. Assuming the pressure and temperature of the gas remain constant, calculate the number
of moles of gas added to the container.
number of moles of gas:
mol
* TOOLS
x10

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

VIEW

Step 2

VIEW

Step by step

Solved in 2 steps with 2 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

The combined gas law states that for a fixed amount of gas, the quantity PVIT is constant. This is often expressed by the equation P¡V PV2 T2 where P is the pressure, V is the volume, and T is the temperature, and the subscripts 1 and 2 denote two different conditions. Rearrange the combined gas law to solve for Pj. P = A gas with an initial temperature of 271 K and initial volume of 15.0 L is heated to 317 K and compressed to 10.2 L. The final pressure of the gas is 4.28 atm. What was the initial pressure (P¡) of the gas? P1 = atm
Refrigerators are usually kept at about 5ﾟC, when Room temperature is about 20ﾟC. If you were to take an empty 2 liter soda bottle at Room temperature and place it in the fridge, would you expect it to contract to 1/4 its original volume?
A tank was filled with 18 g of oxygen (O2), 75 g of nitrogen (N2) and 4 g of carbon dioxide(CO2). At 25°C the pressure of the tank was 8.5 atm. If the partial pressure of CO2 in the tank is x atm, what is the value of x?
1. Which diagrams showing relationships between pressure, volume, and temperature below is/are incorrect for ideal gases? A B C KKKK V P T/P D PV
Show complete solutions and enclose all final answers in a box. Round off final answers to 4 decimal places and floating values for intermediate answers. Use 2 decimal places for molecular weights.
A 10.0 L tank at 2.5 °C is filled with 17.5 g of chlorine pentafluoride gas and 3.17 g of boron trifluoride gas. You can assume both gases behave as ideal gases under these conditions. Calculate the mole fraction and partial pressure of each gas, and the total pressure in the tank. Be sure your answers have the correct number of significant digits. mole fraction: x10 chlorine pentafluoride partial pressure: ? atm mole fraction: boron trifluoride partial pressure: atm Total pressure in tank: atm O
For 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 23.0°C⁢ to −19.0°C, and at the same time the pressure is changed. If the initial pressure was 6.3atm and the volume increased by 55.0%, what is the final pressure? Round your answer to the correct number of significant digits.
For many purposes we can treat butane (C,H10) : as an ideal gas at temperatures above its boiling point of – 1. °C. Suppose the pressure on a 43.0 g sample of butane gas at 14.0°C is reduced to one-third its initial value. Oyes Is it possible to change the temperature of the butane at the same time such that the volume of the gas doesn't change? к10 no If you answered yes, calculate the new temperature of the gas. Round your answer to the nearest °C.
For many purposes we can treat ammonia (NH,) as an ideal gas at temperatures above its boiling point of –33. °C. Suppose the temperature of a sample of ammonia gas is raised from – 25.0 °C to 17.0 °C, and at the same time the pressure is changed. If the initial pressure was 0.15 kPa and the volume decreased by 50.0%, what is the final pressure? Round your answer to 2 significant digits. kPa 1 Don't Know Submit etv DII esc %23 24 6 7 09 2 4 OP E T Y.
Using the ideal gas equation: PV = nRT, calculate the volume (in liters) a 3.1 mol sample of a gas occupies at 21.8 °C and 2.5 atm.
A reaction between liquid reactants takes place at −5.0 °C in a sealed, evacuated vessel with a measured volume of 50.0 L. Measurements show that the reaction produced 8.0 g of boron trifluoride gas. Calculate the pressure of boron trifluoride gas in the reaction vessel after the reaction. You may ignore the volume of the liquid reactants. Round your answer to 2 significant digits. pressure: atm x10 X Ś
Charles' Law explores the effects of temperature on the volume of an ideal gas. Charles’ Law is described as V₁/T₁ = V₂/T₂. A gas with an initial volume of 2.00 L at 275.0 K is heated. The final volume is 3.0 L. Calculate the final temperature of the gas, in K.