part c Learning Goal:To understand the ideal gas law and be able to apply it toa wide variety of situations.The absolute temperature T, volume V, and pressure pof a gas sample are related by the ideal gas law, whichstates thatpV = nᎡᎢ .Here n is the number of moles in the gas sample and Ris a gas constant that applies to all gases. This empiricallaw describes gases well only if they are sufficiently diluteand at a sufficiently high temperature that they are not onthe verge of condensing.In applying the ideal gas law, p must be the absolutepressure, measured with respect to vacuum and not withrespect to atmospheric pressure, and I must be theabsolute temperature, measured in kelvins (that is, withrespect to absolute zero, defined throughout this tutorialas -273°C). If p is in pascals and V is in cubic meters,use R = 8.3145 J/(mol · K). If p is in atmospheresand V is in liters, use R = 0.08206 L.atm/(mol. K).instead.CorrectOne mole of gas occupies 22.4 L at STP (standard temperature and pressure: 0 °C and 1 atm). This fact may be worthmemorizing. In this problem, the temperature is slightly higher than STP, so the gas expands and 22.4 L can be filled by slightlyless than 1 mol of gas.Part CSome hydrogen gas is enclosed within a chamber being held at 200° C with a volume of 0.0250 m³. The chamber is fitted with a movablepiston. Initially, the pressure in the gas is 1.50 × 106 Pa (14.8 atm). The piston is slowly extracted until the pressure in the gas falls to0.950 × 106 Pa. What is the final volume V₂ of the container? Assume that no gas escapes and that the temperature remains at 200°C.Enter your answer numerically in cubic meters.► View Available Hint(s)V₂ =SubmitΑΣΦPart D Complete previous part(s)?3m

Initial volume, v = 0.0250 m³ Initial pressure, p = 1.50×106 Pa Final volume, P = 0.950×106 Pa Final…

Part C Some hydrogen gas is enclosed within a chamber being held at 200° C with a volume of 0.0250 m³. The chamber is fitted with a movable piston. Initially, the pressure in the gas is 1.50 x 106 Pa (14.8 atm). The piston is slowly extracted until the pressure in the gas falls to 0.950 x 106 Pa. What is the final volume V₂ of the container? Assume that no gas escapes and that the temperature remains at 200°C. Enter your answer numerically in cubic meters. ▸ View Available Hint(s)

Part C Some hydrogen gas is enclosed within a chamber being held at 200° C with a volume of 0.0250 m³. The chamber is fitted with a movable piston. Initially, the pressure in the gas is 1.50 x 106 Pa (14.8 atm). The piston is slowly extracted until the pressure in the gas falls to 0.950 x 106 Pa. What is the final volume V₂ of the container? Assume that no gas escapes and that the temperature remains at 200°C. Enter your answer numerically in cubic meters. ▸ View Available Hint(s)

College Physics

1st Edition

ISBN:9781938168000

Author:Paul Peter Urone, Roger Hinrichs

Publisher:Paul Peter Urone, Roger Hinrichs

Chapter13: Temperature, Kinetic Theory, And The Gas Laws

Section: Chapter Questions

Problem 24PE: Suppose a gasfilled incandescent light bulb is manufactured so that the gas inside the bulb is at...

See similar textbooks

Similar questions

One process for decaffeinating coffee uses carbon dioxide ( M=44.0 g/mol) at a molar density of about 14,0 mol/m3 and a temperature of about 60 . (a) Is CO2 a solid, liquid, gas, or supercritical fluid under those conditions? (b) The van der Waals constants for carbon dioxide are a=0.3658 Pa m6/mol2 and b=4.286105 m3/mol. Using the van der Waals equation, estimate pressure of CO2 at that temperature and density. `
In the text, it was shown that N/V=2.681025m3 for gas at STP. (a) Show that this quantity is equivalent to N/V=2.681019cm3, as stated. (b) About how many atoms are mere in one m3 (a cubic micrometer) at STP? (c) What does your answer to part (b) imply about the separation of Mama and molecules?
Unreasonable results. (a) Find the temperature of 0.360 kg of water, modeled as an ideal gas, at a pressure of 1.01105 Pa if it has a volume of 0.615 m3. (b) What is unreasonable about this answer? How could you get a better answer?
(a) What is the gauge pressure in a 25.0 cc car tire containing 3.60 mol of gas in a 30.0-L volume? (b) What will its gauge pressure be if you add 1.00 L of gas originally at atmospheric pressure and 25.0 ? Assume the temperature remains at 25.0 cc and the volume remains constant.
Suppose a gasfilled incandescent light bulb is manufactured so that the gas inside the bulb is at atmospheric pressure when the bulb has a temperature of 20.0C. (a) Find the gauge pressure inside such a bulb when it is hot, assuming its average temperature is 60.0C (an approximation) and neglecting any change in volume due to thermal expansion or gas leaks. (b) The actual final pressure for the light bulb will be less than calculated in part (a) because the glass bulb will expand. What will the actual final pressure be, taking this into account? Is this a negligible difference?
A mole of gas has isobaric expansion coefficient dV/dT=R/p and isochoric pressure-temperature coefficient dp/dT=p/T . Find the equation of state of the gas.
As shown below, which is the phase diagram for carbon dioxide, what is the vapor pressure of solid carbon dioxide (dry ice) at -78.5 (Note that the axes in the figure ale nonlinear and the graph is not to scale.)
The product of the pressure and volume of a sample of hydrogen gas at 0.00 is 80.0 J. (a) How many moles of hydrogen are present? (b) What is the average translational kinetic energy of the hydrogen molecules? (c) What is the value of the product of pressure and volume at 200 ?
Let’s assume dry air behaves like an ideal gas and has a molar mass of 28.8 g/mol.a) What is the approximate density of dry air at sea level when the air temperature is 32°C? Hint: How is the unit of standard atmosphere (symbol atm) defined?b) Briefly show and/or explain why this assumption for the molar mass of dry air is reasonable.c) Briefly show and/or explain how the density of air would change with increasing humidity.
Hi, could I get some help with this macro-connection physics problem involving the Ideal Gas Law? The set up is: What is the average volume in nm3 (cubic nanometers) taken up by molecules of an ideal gas at room temperature (taken as 300 K), and 1 atm of pressure or 101325 N/m2 to 4 digits of precision if kB = 1.38e-23 J/K and 1 nm = 10-9 m? Thank you.
1. A three-liter tank contains two gram-moles of nitrogen at − 150.8o C. Estimate the tank pressure using the ideal gas equation of state and then using the Virialequation of state truncated after the second term. Taking the second estimate to be correct, calculate the percentage error that results from the use of the ideal gas equation at the system conditions. Data for nitrogen: Tc = 126.2 K, pc = 33.5 atm, and ω = 0.04012. 2. One mole of propane gas is to be expanded from 0.001 m3 to 0.040 m3 while incontact with a heating bath at 100o C. The expansion is not reversible. The heatextract from the bath is 600 J. Determine the work for the expansion using theVan der Waals equation of state.
Boyles Law states that when a sample of gas is compressed at a constant temperature, the product of the pressure and the volume remains constant: PV=C. A. Find the rate of change of volume with respect to pressure. B. A sample of gas in a container at low pressure and is steadily compressed at constant temperature for 10 minutes. Is the volume decreasing more rapidly at the beginning or the end of the 10minutes? Please Explain.. C. Prove that the isothermal compressibility is given by B=1/P.