#$&* course phy122 2/1 4Professor Smith,
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Given Solution: ** PV = n R T so n R / P = V / T Since T and V remain constant, V / T remains constant. • Therefore n R / P remain constant. • Since R is constant it follows that n / P remains constant. ** STUDENT QUESTION: I don’t understand why P is in the denominator when nR was moved to the left side of the equation INSTRUCTOR RESPONSE: The given equation was obtained by dividing both sides by P and by T, then reversing the sides. We could equally well have divided both sides by v and by n R to obtain P / (n R) = T / V, and would have concluded that P / n is constant. To say that P / n is constant is equivalent to saying the n / P is constant. Your Self-Critique: Your Self-Critique Rating: ********************************************* Question: why, in terms of the ideal gas law, is T / V constant when only temperature and volume change? YYYYYYYYYYYYYYYYYYYYYYYYYYYYYYYYYYYYYYYYYYY Your Solution: According to dictionary.reference.com ideal gas law is defined as: the law that the product of the pressure and the volume of one gram molecule of an ideal gas is equal to the product of the absolute temperature of the gas and the universal gas constant. confidence rating #$&*: ^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^ I’m not sure how to define this relationship.
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Given Solution: ** STUDENT ANSWER AND INSTRUCTOR RESPONSE: They are inversely proportional. They must change together to maintain that proportion. INSTRUCTOR RESPONSE: You haven't justified your answer in terms of the ideal gas law: PV = n R T so V / T = n R / P. If only T and V change, n and P don't change so n R / P is constant. Therefore V / T is constant, and so therefore is T / V. You need to be able to justify any of the less general relationships (Boyle's Law, Charles' Law, etc.) in terms of the general gas law, using a similar strategy. ** Your Self-Critique: So if PV=n RT then V/T =R/P If only the temperature and volume change, n and P do not change so R/P is constant. V/T is constant and so is T/V Your Self-Critique Rating:
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Given Solution: The Kelvin temperature is 273 K higher than the Celsius temperature (actually 273.15 below, but the degree of precision in the given temperatures is not sufficient to merit consideration of tenths or hundredths of a degree). • 86 C, -100 C and 5500 C are therefore equivalent to ( 86 + 273 ) K = 359 K, -100 + 273 K = 173 K, (5500 + 273) K = 5773 K. The freezing point of water is 0 C or 32 F, and a Fahrenheit degree is 5/9 the size of a Celsius degree. Therefore • 78 F is (78 F - 32 F) = 46 F above the freezing point of water. • 46 Fahrenheit degrees is the same as (5/9 C / F ) * 46 F = 26 C above freezing. • Since freezing is at 0 C, this means that the temperature is 26 C. • The Kelvin temperature is therefore (26 + 273) K = 299 K. Similar reasoning can be used to convert -459 F to Celsius • -459 F is (459 + 32) F = 491 F below freezing, or (5/9 C / F) * (-491 F) = 273 C below freezing. • This is -273 C or (-273 + 273) K = 0 K. • This is absolute zero, to the nearest degree. Your Self-Critique: Your Self-Critique Rating: ********************************************* Question: prin phy and gen phy Ch 13.30 air at 20 C is compressed to 1/9 of its original volume. Estimate the temperature of the compressed air assuming the pressure reaches 40 atm. YYYYYYYYYYYYYYYYYYYYYYYYYYYYYYYYYYYYYYYYYYY Your Solution: I’m going to read below how to solve this and then I will put it into my own words below. confidence rating #$&*: ^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^ I’m not sure how to figure this out, but I will know in a minute. Answer to follow.
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Given Solution: Evidently if the air is compressed to 1/9 its original volume, there would be no temperature change, it would end up with 9 times its original pressure. However it was noted that the pressure changes from 1 atm to 40 atm, so if the pressure is 40 times the original pressure, there has to be a heating process. The absolute temperature would need to rise by a factor of 40/9. If the original temperature was 20 C the Kelvin temperature would be (20+273)= 273 K. so the final temperature would be 293K*40/9=130K First we reason this out intuitively: If the air was compressed to 1/9 its original volume and the temperature didn’t change, it would end up with 9 times its original pressure. However the pressure changes from 1 atm to 40 atm, which is a 40-fold increase. The only way the pressure could end up at 40 times the original pressure, as opposed to 9 times the original, would be to heat up. Its absolute temperature would therefore have to rise by a factor of 40 / 9. Its original temperature was 20 C = 293 K, so the final temperature would be 293 K * 40/9, or over 1300 K. Now we reason in terms of the ideal gas law. P V = n R T. In this situation the number of moles n of the gas remains constant. Thus P V / T = n R, which is constant, and thus P1 V1 / T1 = P2 V2 /T2. The final temperature T2 is therefore • T2 = (P2 / P1) * (V2 / V1) * T1. From the given information P2 / P1 = 40 and V2 / V1 = 1/9 so • T2 = 40 * 1/9 * T1. The original temperature is 20 C = 293 K so that T1 = 293 K, and we get • T2 = 40 * 1/9 * 293 K, the same result as before. Your Self-Critique: Well, the formula definitely makes it easier, but if I can’t remember the formula I know that I can still solve for the answer. Your Self-Critique Rating:
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Given Solution: (Note that the given 220 kPa initial gauge pressure implies an absolute pressure of 311 k Pa; assuming atmospheric pressure of about 101 k Pa, we add this to the gauge pressure to get absolute pressure). Remember that the gas laws are stated in terms of absolute temperature and pressure. The gas goes through three states. The temperature and pressure change between the first and second states, leaving the volume and the number n of moles constant. Between the second and third states pressure returns to its original value while volume remains constant and the number n of moles decreases. From the first state to the second: T1 = 288 K, T2 = 311 K so T2 / T1 = 311 / 288 = 1.08, approx. This is approx. an 8% increase in temperature. The pressure must therefore rise to P2 = 3ll / 288 * 321 kPa = 346 kPa, approx (note that we have to use actual rather than gauge pressure so init pressure is 220 kPa + 101 kPa = 321 kPa, approx. ) From the second state to the third, pressure is then released by releasing some gas, changing the number n of moles of gas in order to get pressure back to 331 kPa. Thus n3 / n2 = P3 / P2 = 321 kPa / 346 kPa or approximately .93, which would be about a 7% decrease. So we have to release about 7% of the air. Note that these calculations have been done mentally, and they might not be particularly accurate. Work out the process to botain the accurate numerical results. Note also that temperature changes from the second to third state were not mentioned in the problem. We would in fact expect a temperature change to accompany the release of the air, but this applies only to the air that escapes. The air left in the tire would probably change temperature for one reason or another, but it wouldn't do so as a direct result of releasing the air. STUDENT QUESTION It seems that the air goes from 288 to 311 K, so the ratio should be n2 / n1 = 288 / 311 and the proportional loss should be about (1 - 288 / 311) INSTRUCTOR RESPONSE The Kelvin temperature goes from 288 K to 311 K. If the air is released at constant pressure, then volume and pressure remain constant while temperature and number of moles vary according to n T = P V / R so that n1 T1 = n2 T2, and n2 = n1 * (T1 / T2) = n1 * (288 / 311) and the change in amount of gas is n1 - n2 = n1 - 288/311 n1 = n1( 1 - 288 / 311), or about 7.4% of n1. If the temperature is first raised to 311 K, then the gas is released, it is the pressure and amount of gas that change. In that case the change in the amount of the gas is n1 - n3 = n1 - (321 kPa / 346 kPa) * n1 = n1 ( 1 - 321 / 346), or about 7.2% of n1. The fractions 288/311 and 321 / 346 don't differ by much, not do the percents, but they do differ. Your Self-Critique: I am now solving for these problems before typing them in, that helps tremendously! Your Self-Critique Rating:
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Given Solution: Simple reasoning: the volume increases by a factor of 20, which by itself would imply that the pressure decreases by a factor of 20. But absolute temperature also decreases by a factor of 223 / 283, which would also imply a pressure decrease. Bottom line: The pressure changes by factor (1/20) * (223/283) = .039, ending up at .039 of its original value. More reliable analysis: If V_0 and V_f are the initial and final volumes, then V_f / V_0 = 20 The initial and final temperatures are 10 C = 283 K and -50 C = 223 K, so the ratio of temperatures is T_f / T_0 = 223 / 283. Since no helium escapes, n is constant to the PV = n R T implies that P V / T is constant. Thus P_0 V_0 / T_0 = P_f V_f / T_f. Solving this for the pressure P_f we obtain P_f = P_0 * V_0 / V_f * T_f / T_0 = P_0 * (1/20) * (223/283) = P_0 * .039. That is, the pressure at the new altitude is about .039 that at the surface. Assuming the surface pressure to have been 1 atmosphere, the gauge pressure at altitude would be (.039 atm - 1 atm) = -.961 atm. &&&&&&&&&&&&&&&&&&&&&&&&&&&&&&&&&&&&&&&&&&&&& Self-critique (if necessary): ------------------------------------------------ Self-critique Rating: #$&* ********************************************* Question: (a) What is the average kinetic energy in joules of hydrogen atoms on the 5500ºC surface of the Sun? (b) What is the average kinetic energy of helium atoms in a region of the solar corona where the temperature is 6.00×10^5 K ? The average kinetic energy of particles at temperature T is KE_ave = 3/2 k T, where k = R / N_A is the Boltzmann constant (R is the gas constant and N_A is avagodro's number). The average kinetic energy of a particle does not depend on what kind of particle it is. However the less massive the particle, the greater will be its speed at the average kinetic energy. At 5500 C the absolute temperature is 5773 K so the average KE of a particle is KE_ave = 3/2 k T = 3/2 * 1.38 * 10^-23 Joules / (particle Kelvin) * 5773 K = 1.19 * 10^-19 Joules. YYYYYYYYYYYYYYYYYYYYYYYYYYYYYYYYYYYYYYYYYYY Your solution: a. I hope that I am right on this: Ke_ave=3/2T=3/2*1.38*10^-23J /(particle K)*5733K= b. 3/2*1.38*10^-23J/(particle K)*6.00*10^5K= confidence rating #$&*: ^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^ Uncetain…
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Given Solution: &&&&&&&&&&&&&&&&&&&&&&&&&&&&&&&&&&&&&&&&&&&&& Self-critique (if necessary): How do I solve for this? I am drawing a blank once again. I realize that I plug the numbers into the equation, but in your example above how did you reduce from 10^-23 to 10^-19? I’m sure this is something simple, but right now I’m not seeing it. Sorry Professor. What is particle K?
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Given Solution: Outline of solution strategy: If we multiply the number of watts per unit of area by the surface area of the Sun we get the number of watts radiated from the Sun. The energy flows outward in a spherically symmetric manner; at any distance the entire power is distributed over the radius of a sphere concentric with the Sun and of radius equal to the distance. So if we divide that number of watts by the area of a sphere whose radius is equal to that of the Earth’s orbit, we get the number of watts per unit of area at that distance. This strategy is followed in the student solution given below: Good student solution: Surface area of sphere of radius r is 4 pi r^2; if flux intensity is I then flux = 4 pi r^2 I. When r = 1.5 * 10^11 m, I = 1500 W / m^2, so the flux is 4 pi r^2 I = 4 pi * (1.5 * 10^11 m)^2 * 1500 W / m^2 = 4.28 * 10^26 watts. 4.28055 x 10 ^ 26 W / (4*`pi * (6.96 x 10 ^ 8 m)^2) = 4.28055 x 10 ^ 26 W / 6.08735 x 10 ^ 18 m^2 = 70318775.82 J/s/m^2 = 7.03 x 10 ^ 7 J/s/m^2 If the sun is radiating as an ideal blackbody, e = 1, then T would be found as follows: H = `dQ/`dt = 4.28055 x 10 ^ 26 W = (4*`pi * (6.96 x 10 ^ 8 m)^2) * (1) * (5.67051 x 10^-8 W/m^2*K) * T^4 So T^ 4 = 4.28055 x 10 ^ 26 W / 6.087351 x 10 ^ 18 m^2) * 1 * (5.67051 x 10^-8 W/m^2*K) T^4 = 1.240 * 10 ^ 15 K ^4 T = 5934.10766 K on surface of sun. ** Your Self-Critique: Oh my. This is a bit overwhelming. How did she/he get the 10^26 watts listed above? Where did the 6.96x10^8m^2 come from? What does the e signify? Your Self-Critique Rating: ********************************************* Question: univ phy (omitted from 12th edition, but should be worked now) was 17.115 Solar radiation of intensity 600 watts / m^2 is incident on an ice sheet. The temperature above and below the ice sheet is 0 Celsius. Assuming that 70% of the radiation is absorbed at the surface of the ice, how long take to melt a layer of ice 1.2 cm thick? YYYYYYYYYYYYYYYYYYYYYYYYYYYYYYYYYYYYYYYYYYY Your Solution: Shew. This is also over my head. I will again read below and see what I can come up with.
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Given Solution: ** Thermal energy is not radiating in significant quantities from the ice, so only the incoming radiation needs to be considered, and as stated only 70% of that energy is absorbed by the ice.. • 70% of the incoming 600 watts/m^2 is 420 watts / m^2, or 420 Joules/second for every square meter if ice. • Melting takes place at 0 C so there is no thermal exchange with the environment. Thus each square meter absorbs 420 Joules of energy per second. We need to consider the volume of ice corresponding to a square meter. Having found that we can determine the energy required to melt the given thickness: • A 1.2 cm thickness of ice will have a volume of .012 m^3 for every square meter of surface area; the mass will be close to 1000 kg/m^3, so there are about 12 kg of ice for every m^2 of surface (you can obtain a more accurate result by using the a more accurate density; the density of ice (which floats in water) is actually somewhat less than that of water). • It takes about 330,000 Joules to melt a kg of ice at 0 C, so to melt 12 kg requires around 4,000,000 J. At 420 Joules/sec this will require roughly 10,000 seconds, or around 3 hours. All these calculations were done mentally and are therefore approximate. You should check them yourself, using appropriately precise values of the constants, etc. ** Self-critique: Professor, how did you get the volume for the ice when we have no dimensions for the ice? How did you calculate for the mass from the information we are given above? Would you mind showing your work, step by step? ------------------------------------------------ Self-Critique Rating: ********************************************* Question: `q004. A body with a 1/2 m^2 surface area, at temperature 25 Celsius, has an emissivity of approximately 1. It exchanges energy by radiation with a large surface at temperature -20 Celsius. At what net rate does it lose energy? By what percent would the rate of energy loss change if the large surface was at temperature -270 Celsius? YYYYYYYYYYYYYYYYYYYYYYYYYYYYYYYYYYYYYYYYYYY Your Solution: I need to know the specific heat of the human body so I looked it up and it is 3500 J. I also know that I need to find the differences in temperatures which is 5 degrees C. I also need to find the conductivity. I will use the following formula to solve this question: R=k(dT/dx) *A So. I first need to find k. I will use this formula k=(dQ/dt)/(A(dt/dx) K=(3500J/5)/(1.2m^2(5/dx) Professor, I’m really drawing a blank here. I am really not even sure if I have chosen the right formula. I think that I have. I am sure that I need to solve for k first but I don’t know how to find dx. Do I have anything right on this problem? I’m really thinking that I need a tutor about right now. I feel like such an inconvenience to you. I’m constantly asking questions and I know that you are very busy trying to teach class both in person and online. Please help. confidence rating #$&*: ^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^ Terrible! ------------------------------------------------ Self-Critique Rating: " Self-critique (if necessary): ------------------------------------------------ Self-critique rating: " Self-critique (if necessary): ------------------------------------------------ Self-critique rating: #*&!