Answered: An ideal gas originally at 0.87 atm and…

An ideal gas originally at 0.87 atm and 68°C was allowed to expand until its final volume, presSure, and temperature were 95 mL, 0.64 atm, and 48°C, respectively. What was its initial volume? V1 mL

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter5: Gases

Section: Chapter Questions

Problem 61E: An ideal gas is contained in a cylinder with a volume of 5.0 102 mL at a temperature of 30.C and a...

See similar textbooks

Related questions

Q: What is the volume of a 33.8 g sample of CO2 (44.02 g/mole) if it is in a container at 1.20 atm and…

A: Given: Mass of CO2 = 33.8 g Molar mass of CO2 = 44 g/mol Pressure P = 1.20 atm Temperature T =…

Q: An unknown amount of gas occupies 30.0 L at 2.1 atm and 298 K. How many moles does the sample…

A: Given data contains, Volume of gas is 30.0L. Pressure of gas is 2.1 atm. Temperature is 298K.

Q: How many moles of O2 were produced in a decomposition reaction of H2O2 if the pressure was 0.978…

Q: 3. At a pressure of 780.0 mm Hg and 24.2 °C, a certain gas has a volume of 350.0 mL. What will be…

Q: An anesthetic gas contains 64.81% carbon, 13.60% hydrogen, and 21.59% oxygen, by mass. If 2.00 Lof…

A: According to the question, Anesthetic gas contains 64.81% carbon, 13.60% hydrogen and 21.59%…

Q: An ideal gas originally at 0.85 atm and 62°C was allowed to expand until its final volume, pressure,…

A: Given,Initial pressure, P1 = 0.85 atmInitial pressure, T1 = 62 oC = (62 + 273.15) K = 335.15…

Q: Determine the density of a gas with ℳ = 146.07 g/mol at 1.00 atm and 100.0ºC.

A: Density of the gas is related to molar mass, pressure and the temperature by the equation below:…

Q: If a sample of gas has an initial volume of 563.2mL and an initial pressure of 547,563 Pa, what is…

A: Given: Initial volume of gas, V1= 563.2mL Final volume of gas, V2 = ??? initial pressure gas P1=…

Q: What is the volume of a 37.4 g sample of CO2 (44.02 g/mole) if it is in a container at 1.20 atm and…

A: Given, 37.4 g sample of CO2 at 1.20 atm and 298.15 K

Q: A gast at 85.5°C and 1.78atm is compressed until the volume decreases from 505.8ml to 126.1ml and…

A: Solution The new temperature is 301.4 K

Q: At 1.391.39 atm and 22.75 ∘C22.75 ∘C, a 2.772.77 g sample of gas occupies a volume of 15501550 mL.…

A: An ideal gas is an hypothetical gas where the particles are randomly moving with no inter-particle…

Q: An ideal gas originally at 0.85 atm and 65°C was allowed to expand. until its final volume,…

A: Ideal gas law , Ideal gas law state the relation between the pressure, temperature, volume and…

Q: 2.90 x 10^-3g of unknown gas are produced at 298k and 1.00 atm. The volume of gas generated was 3.52…

Q: A pure gas has a density of 1.80 g/L at 20.0 °C and 1.88 atm. Calculate the molecular mass of the…

A: It is given that the density of a gas is 1.80 g/L and has a pressure of 1.88 atm, and the molar mass…

Q: The ideal gas equation is PV = nRT where P is pressure, V is volume, n is the number of moles, R is…

Q: if 19.28 L of CO2 are collected at 52 celceus, at what temperature would the volume of this gas be…

Q: What is the molar volume of an ideal gas at 546 R and 1.00 atm? 16.9 L 89.6 L 22.4 L 11.2 L 44.8 L

A: To calculate the molar volume of an ideal gas at 546 K and 1.00 atm.

Q: A flask contains 1000 ml of a pure diatomic gas 646 mm Hg and 20 degrees mass of gas is 1.13 g. What…

Q: Given 100ml of a dry gas, measuring 37°C and 760mmHg pressure, what would its volume be at 60°C and…

A: Given that: volume, V1 = 100 mL = 0.1 L temperature, T1 = 37 oC = 37 + 273 = 310 K pressure, P1 =…

Q: iv) At STP, one mole of an ideal gas occupies.... a) 10.22 L b) 20.24 L c) 30.22 L d) none of these

A: STP stands for standard temperature and pressure. Standard temperature is 298 K and standard…

Q: If the initial temperature of an ideal gas at 2.250 atm is 62.00 °C, what final temperature would…

Q: Use the equation below relating the molecular weight of a gas with its mass, volume, and temperature…

A: By using given equation and by putting values with proper units , we can calculate the molecular…

Q: At 571 mm Hg and 323 K, a gas sample has a volume of 2.45 mL. What is the final pressure (in mm Hg)…

Q: A gas mixture is made by combining 7.1 g each of Ar, Ne, and an unknown diatomic gas. At STP, the…

A: The mass of each Ar, Ne and unknown diatomic gas present in mixture is 7.1 g. The volume occupied by…

Q: How many moles of gas are contained in 890.0 mL at 21 °C and 100. kPa pressure? * O 0.073 moles O…

A: In this question, we want to determine the moles of gas. How we can determine the moles of gas, you…

Q: 2.50 g He as non ideal gas is in a container with the volume of 1550 mL. Calculate the pressure of…

A: By knowing the pressure and volume correction factor, we can easily calculate any of the…

Q: Give the Ideal Gas equation and specify what each variable is. Show one mole of gas at S.T.P.…

A: At STP condition : Temperature (T) is 273 K (0 °C) and Pressure (P) is 1 atm The ideal gas…

Q: Using Ideal Gas Law 25.0g of methane (CH4) has a pressure of 450.0kPa at 250℃. Find the volume…

A: Ideal gas law states that the product of pressure and volume of one gram molecule is equal to the…

Q: PA 6.33 L vessel contains 40.5 g of a gas at 1.00 atm and 37.0°C. What is the molar mass of the gas

A: In this question, we have to find out the correct answer of given problem by the help of the…

Q: Some N, gas is mixed with some 0, gas, and the sketch below shows a representative sample of the…

A: Mole fraction = mole of gas /total mole Partial pressure = mole fraction × total pressure Given that…

Q: A 1.25g gas sample occupies 663ml at 25.0C and 1.00 atm. What is the molar mass of the gas

Q: At 25°C and 760 mm of Hg pressure a gas occupies 600ml volume. What will be its pressure at a height…

Q: For an ideal gas, predict the shape of the plot for each of these graphs, where P is pressure, V is…

A: To identify the correct plot between the pressure, volume and moles plots.

Q: What is the volume (in L) of carbon dioxide at 1.00 atm and 298.15 K are released from a car's…

A: Amount of product formed calculation using stoichiometric coefficients

Q: A gaseous product has a mass of 2.34g and occupies a volume of 0.854 L.The temperature in the…

Q: Calculate the partial pressure of each component in a mixture of gases contains 3.50 g N2, 2.50 g…

A: The pressure of the gas depends on the number of gas molecules and does not depends on the nature of…

Q: 9. a) You have determined experimentally that at standard temperature and pressure (0 °C and 1 atm)…

A: For ideal gas the equation of state is : PV = nRT = (W/M)RT Or, M = WRT/PV ...(1) Here, W =…

Q: What is the molar mass of an unknown gas with a density of 1.90 g/L at 1.00 atm and 25.0 °C?…

Q: What is the volume of a 39.2 g sample of CO2 (44.02 g/mole) if it is in a container at 1.20 atm and…

A: Given: mass of CO2 = 39.2 g Pressure in the container = 1.20 atm Temperature = 298.15 K molar mass…

Q: 4. If a gas is cooled from 323.0 K to 273.15 K and the volume is kept constant what final pressure…

A: Gas laws are the laws that relate to the pressure, temperature, and volume of a substance. The…

Q: At 2.00oC and 1.00 atm, a sample of gas occupies 30.0 mL. If the temperature increases to 30.0oC and…

Q: Assuming that a 1.5 g gas occupying a volume of 500 ml at a pressure of 1.75 atm and a temperature…

A: Given: Mass of gas = 1.5 g. Volume of gas = 500 mL = 0.500 L…

Q: 13.A gas was found to have a density of 1.76 mg/mL at 24.0°C and a pressure of 98.8 kPa. What is its…

A: The molecular mass of a gas to be given, Given : Density=1.78 mg/mL Temperature=(240 C) 297 K…

Q: #1.The volume of a gas at 99.0 kPa is 300.0 mL. If the pressure is increased to 188 kPa, what will…

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

Q: For an ideal gas, predict the shape of the plot for each of these graphs, where Pis pressure, V is…

A: Dear student this question is related to Boyle' s law.

Q: An unknown gas has a density of .355g/L at 17 celsius and 189mm Hg. Calculate the molar mass of the…

A: Since density = mass / volume Hence mass of gas = density X volume = 0.355 V hence moles of gas =…

Q: A 4.00 L flask filled with He at 6.00 atm is connected to another 2.00 L flask containing N2 at 3.00…

A: Considered that the temperature of the system is 298.15 K. The number of moles of He and N2 is…

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

An ideal gas originally at 0.87 atm and 68°C was allowed to expand until its final volume, presSure, and
temperature were 95 mL, 0.64 atm, and 48°C, respectively. What was its initial volume?
V1
mL

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

VIEW

Step 2

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 2 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

An ideal gas is contained in a cylinder with a volume of 5.0 102 mL at a temperature of 30.C and a pressure of 710. torr. The gas is then compressed to a volume of 25 mL, and the temperature is raised to 820.C. What is the new pressure of the gas?
Pressures of gases in mixtures are referred to as partial pressures and are additive. 1.00 L of He gas at 0.75 atm is mixed with 2.00 L of Ne gas at 1.5 atm at a temperature of 25.0 C to make a total volume of 3.00 L of a mixture. Assuming no temperature change and that He and Ne can be approximated as ideal gases, what are a the total resulting pressure, b the partial pressures of each component, and c the mole fractions of each gas in the mix?
When hydrogen peroxide decomposes, oxygen is produced: 2H2O2(aq)2H2O+O2(g)What volume of oxygen gas at 25C and 1.00 atm is produced from the decomposition of 25.00 mL of a 30.0% (by mass) solution of hydrogen peroxide (d=1.05g/mL)?
A 0.105-g sample of a gaseous compound has a pressure of 561 mm Hg in a volume of 125 mL at 23.0 C. What is its molar mass?
The atmosphere in a sealed diving bell contained oxygen and helium. If the gas mixture has 0.200 atm of oxygen and a total pressure of 3.00 atm, calculate the mass of helium in 10.0 L of the gas mixture at 40C.
Consider these four gas samples, all at the same temperature. The larger boxes have twice the volume of the smaller boxes. Rank the gas samples with respect to: (a) pressure, (b) density, (c) average kinetic energy, and (d) average molecular speed. (Green spheres are He; violet spheres are Ne.)
What is the value of the ideal gas constant R if the volume is specified in milliliters rather than liters?
Phosgene is a highly toxic gas made up of carbon, oxygen, and chlorine atoms. Its density at 1.05 atm and 25C is 4.24 g/L. (a) What is the molar mass of phosgene? (b) Phosgene is made up of 12.1% C, 16.2% O, and 71.7% Cl. What is the molecular formula of phosgene?
You have a gas, one of the three known phosphorus-fluorine compounds (PF3, PF3, and P2F4). To find out which, you have decided to measure its molar mass. (a) First, yon determine that the density of the gas is 5.60 g/L at a pressure of 0.971 atm and a temperature of 18.2 C. Calculate the molar mass and identify the compound. (b) To check the results from part (a), you decide to measure the molar mass based on the relative rales of effusion of the unknown gas and CO2. You find that CO2 effuses at a rate of 0.050 mol/min, whereas the unknown phosphorus fluoride effuses at a rate of 0.028 mol/min. Calculate the molar mass of the unknown gas based on these results.