part d 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 = nRT.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..SubmitPart DCorrectCorrect answer is shown. Your answer 0.04 m³ was either rounded differently or used a different number of significant figuresthan required for this part.Notice how n is not needed to answer this problem and neither is T, although you do make use of the fact that I is a constant.T₂ =Previous AnswersSome hydrogen gas is enclosed within a chamber being held at 200° C whose volume is 0.0250 m³. Initially, the pressure in the gas is1.50 × 106 Pa (14.8 atm). The chamber is removed from the heat source and allowed to cool until the pressure in the gas falls to0.950 × 106 Pa. At what temperature T2 does this occur?Enter your answer in degrees Celsius.► View Available Hint(s)SubmitΑΣΦ?Q

Answered: Image /qna-images/answer/a367d414-f051-4db5-aa18-df61ced58997.jpg

Part D Some hydrogen gas is enclosed within a chamber being held at 200° C whose volume is 0.0250 m³. Initially, the pressure in the gas is 1.50 x 106 Pa (14.8 atm). The chamber is removed from the heat source and allowed to cool until the pressure in the gas falls to 0.950 x 106 Pa. At what temperature T₂ does this occur? Enter your answer in degrees Celsius. ▸ View Available Hint(s) T₂ = Submit 1971 ΑΣΦ www. ? °C

Part D Some hydrogen gas is enclosed within a chamber being held at 200° C whose volume is 0.0250 m³. Initially, the pressure in the gas is 1.50 x 106 Pa (14.8 atm). The chamber is removed from the heat source and allowed to cool until the pressure in the gas falls to 0.950 x 106 Pa. At what temperature T₂ does this occur? Enter your answer in degrees Celsius. ▸ View Available Hint(s) T₂ = Submit 1971 ΑΣΦ www. ? °C

Principles of Physics: A Calculus-Based Text

5th Edition

ISBN:9781133104261

Author:Raymond A. Serway, John W. Jewett

Publisher:Raymond A. Serway, John W. Jewett

Chapter16: Temperature And The Kinetic Theory Of Gases

Section: Chapter Questions

Problem 66P

See similar textbooks

Similar questions

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?
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.
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?
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.
4. At 20°C a confined ammonia gas has a pressure of 2.50 atm. At what temperature would its pressure be equal to 1 atm? Follow the format in answering: •Given: •Find: •Convert Temperature: •Solving:
(II) Compare the value for the density of water vapor atexactly 100°C and 1 atm with the value predictedfrom the ideal gas law. Why would you expect a difference?
Calculating the Number of Molecules in a Cubic Meter of GasHow many molecules are in a typical object, such as gas in a tire or water in a glass? This calculation can give us an idea of how large N typically is. Let’s calculate the number of molecules in the air that a typical healthyyoung adult inhales in one breath, with a volume of 500 mL, at standard temperature and pressure (STP), which is defined as 0 ºC and atmospheric pressure. (Our young adult is apparently outside in winter.)StrategyBecause pressure, volume, and temperature are all specified, we can use the ideal gas law, pV = NkB T, to find N
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.
One mole of an ideal monatomic gas is initially at a temperature of 274 K. Suppose the amount of gas is doubled to two moles. Does thefinal temperature found in part (a) increase, decrease, or stay thesame? Explain.