Suppose a tank contains 521 m³ of neon (Ne) at an absolute pressure of 1.01×105 Pa. The temperature is changed from 293.2 to 294.4 K. What is the increase in the internal energy of the neon?
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Q: Suppose a tank contains 714 m3 of neon (Ne) at an absolute pressure of 1.01x105 Pa. The temperature…
A: Given: V = 714 m3 P = 1.01 x 105 Pa T1 = 293.2 K T2 = 294.7 K Cv = 3R/2
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Q: Suppose a tank contains 636 m³ of neon (Ne) at an absolute pressure of 1.01x105 Pa. The temperature…
A: Given value--- volume = 636 m3. pressure = 1.01 × 105 Pa. The temperature is changed from 293.2 to…
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A: P1 = 1.80 atmT1 = 315 kV1 = 15 LP2 = 2.10 atmT2= 465 kV2 = 22 L
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A: ∆U=32nRT2-T1
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- Consider the process shown in (Figure 1). Figure p (kPa) 400- EV 200- 100 200 300 0₁ 0 V (cm³) 1 of 1 How much work is done on the gas in this process? Express your answer with the appropriate units. W = Submit μA Value Provide Feedback Request Answer Units ?An automobile tire contains 0.038 m² of air at a gauge pressure of 2.41 × 10³ N/m2. The composition of air is about 78% nitrogen (N2) and 21% oxygen (O2), both diatomic molecules. How much more internal energy, in joules, does the air in the tire have than the same volume of air has at zero gauge pressure outside the tire? Emt,2 - Ent,1 JAn ideal gas of 20 moles expands isothermally at temperature T= 90°C. The final volume is 5 times its initial volume. What is the heat flow into the gas in units of kJ? The universal gas constant R is 8.32 J/(mol·K).
- Problem #1: An ideal gas of initial volume V=1m^3, initial temperature T=1000C and initial pressure P=10,000 Pa is heated up to a final temperature T=3000C and allowed to expand into a final volume V=3m^3. What is the final pressure?A 2100 cm^3 container holds 0.15 mol of helium gas at 330C. 1. How much work must be done to compress the gas to 1400cm^3 at constant pressure? 2. How much work must be done to compress the gas to 1400cm^3 at constant temperature?A student decides to conduct an experiment by using two different flasks and two different gas samples. In flask 1, there exists Neon (Ne) gas, whereas the second flask is filled with nitrogen (N2) gas. If both flasks are kept at 270 K, answer the following questions. (Note: Molar mass of N2 = 28.014 g mol1,molar mass of Neon = 20.1797 g mol, R= 8.31 J. mol1.K1, k=1.38 x 1023 J.K-1, Avogadro's number = 6.02 x 1023 mol1.) a) Find the average kinetic energy of one Neon molecule. b) Calculate the average kinetic energy (translational+rotational) of one nitrogen molecule by including rotational motion in your calculations. c) Find the root-mean-square speed of one neon molecule. V ms1 Check
- An SUV tire contains 0.037 m3 of air at a gauge pressure of 2.61 × 105 N/m2. The composition of air is about 78% nitrogen (N2) and 21% oxygen (O2), both diatomic molecules. How much more internal energy, in joules, does the air in the tire have than the same volume of air has at zero gauge pressure outside the tire? Einternal,2−Einternal,1 = ? Hints: -Assume not only equal volumes but also equal temperatures.-Since the temperature is constant, what must be changing in this process?-The heat capacity, and thus the internal energy, depends upon whether gas is monatomic or diatomic.2.00 mol of helium and 1.00 mol of argon are separated by a very thin barrier. Initially the helium has 7500 J of thermal energy. The helium gains 2500 J of energy as the gases interact and come to thermal equilibrium by exchanging energy via collisions at the boundary. What was the initial temperature of the argon? First, what is the equilibrium temperature of the two gases? Express your answer in kelvins. ► View Available Hint(s) Tf = Submit Part B VE ΑΣΦ help What is the thermal energy of the argon at the equilibrium temperature? Express your answer with the appropriate units.