The last question РАThe figure shows a PV diagram similar to the cycle of a Dieselengine. It consists of two adiabatic steps (a→b) and (c→d), aconstant pressure step (b→c) and a constant volume step (d→a).We are interested in the efficiency, assuming the engine uses adiatomic (f = 5) ideal gas.a) For each of the four steps, state what type of process it is andthe sign (+,-,or 0) of the work W, the heat Q, and the internalenergy change AU.Туреsign of WStepa→bsign of AUsign of Qb→cc→dd→ab) Express the engine efficiency in terms of the heat input |Qin and the exhausted heat |Qout.c) What is the isobaric heat capacity of n mole of a diatomic ideal gas?d) Use your table to identify the steps where heat enters the engine and where heat is exhausted andcalculate the efficiency. Your result for the efficiency should only contain temperature differencesand numbers.adiabatadiabatda

The heat capacity ratio can be described as: γ=CpCv =7R/25R/2 =1.4

The figure shows a PV diagram similar to the cycle of a Diesel engine. It consists of two adiabatic steps (a→b) and (c→d), a constant pressure step (b→c) and a constant volume step (d-a). We are interested in the efficiency, assuming the engine uses a diatomic (f = 5) ideal gas. a) For each of the four steps, state what type of process it is and the sign (+,-,or 0) of the work W, the heat Q, and the internal energy change AU. Type Step a-b sign of W sign of AU sign of Q b→c c→d d➜a b) Express the engine efficiency in terms of the heat input |Qin and the exhausted heat Qout. c) What is the isobaric heat capacity of n mole of a diatomic ideal gas? d) Use your table to identify the steps where heat enters the engine and where heat is exhausted and calculate the efficiency. Your result for the efficiency should only contain temperature differences and numbers. b adiabat C adiabat d a V

The figure shows a PV diagram similar to the cycle of a Diesel engine. It consists of two adiabatic steps (a→b) and (c→d), a constant pressure step (b→c) and a constant volume step (d-a). We are interested in the efficiency, assuming the engine uses a diatomic (f = 5) ideal gas. a) For each of the four steps, state what type of process it is and the sign (+,-,or 0) of the work W, the heat Q, and the internal energy change AU. Type Step a-b sign of W sign of AU sign of Q b→c c→d d➜a b) Express the engine efficiency in terms of the heat input |Qin and the exhausted heat Qout. c) What is the isobaric heat capacity of n mole of a diatomic ideal gas? d) Use your table to identify the steps where heat enters the engine and where heat is exhausted and calculate the efficiency. Your result for the efficiency should only contain temperature differences and numbers. b adiabat C adiabat d a V

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter6: Thermochemistry

Section: Chapter Questions

Problem 134IP: Nitromethane, CH3NO2, can be used as a fuel. When the liquid is burned, the (unbalanced) reaction is...

See similar textbooks

Similar questions

A suburban house has two window-unit air conditioners, with each consuming 500 kWh of electricity each month. How much electricit is consumed during the three summer months? 2.4 MWh3.0 MWh 4.5 MWh 3.6 MWh
consider the following balancing process at 700c 2H2 (g) + 2s2 (g) 《》 2H2 (g) An analysis shows that there are 2.5 moles of H2, 135 × 10 ^ -5 moles of S2 and 8.70 moles of H2S contained in a 12-liter flask calculating Kc and Kp
Develop a general equation for the standard heat of reaction as a function of temperature for one of the reactions given in parts a, b, c a. N2(g)+3H2(g) → 2NH3(g) b. 4NH3(g) +5O2(g) → 4NO(g)+6H2O(g) c. 2Na(s)+2H2O(g) →2NaOH(s)+H2(g)
Which of the following processes has ΔS<0? Select one: C3H8(g) + 5O2(g) → 3CO2(g) + 4H2O(g) 1.0 L of He(g) is compressed to 500 mL. Milk is added to a cup of coffee. H2O(s) → H2O(l) CaCl2(s) → Ca2+(aq) + 2Cl–(aq)
Nitromethane, CH3NO2, can be used as a fuel. When the liquid is burned, the (unbalanced) reaction is mainly CH3NO2(l) + O2(g) CO2(g) + N2(g) + H2O(g) a. The standard enthalpy change of reaction (Hvan ) for the balanced reaction (with lowest whole-number coefficients) is 1288.5 kJ. Calculate Hf0 for nitromethane. b. A 15.0-L flask containing a sample of nitromethane is filled with O2 and the flask is heated to 100.C. At this temperature, and after the reaction is complete, the total pressure of all the gases inside the flask is 950. torr. If the mole fraction of nitrogen (nitrogen) is 0.134 after the reaction is complete, what mass of nitrogen was produced?
Subject: Physical Chemistry you are a food specialist in a company that specializes in refrigerated delicacies, and one of your brands requires being maintained at a temperature of 5°C. You determine average water activity (aw) at this temperature to be 0.2. One day, you are informed that the cooling systems on one of the delivery trucks carrying your company’s products malfunctioned while en route to its destination and it would not be fixed until the next delivery. The driver has informed you that the temperature in the delivery bay of the truck is averaging 55°C. You estimate a heat of sorption (Q) of 19 kJ/mol. Calculate the water activity of the brand at this elevated temperature and comment on it’s integrity. Should the delivery still push through? Or should the products be recalled and disposed
Develop a general equation for the standard heat of reaction as a function of temperature for one of the reactions given in parts (a), (b) a. CO2 (g) + 3H2 (g) → CH3OH(g) + H2O(g) b. C2H2 (g) + H2O(g) → ⟨(CH2)2⟩O(g)
Given the following information, Calculate delta G(degree). Give your answer in kJ. 3Ag+ (aq) + Cr (s) → 3 Ag (s) + Cr3+ (aq) __________________________________________ Ag+(aq) + 1 e- → Ag (s) 0.80 V Cr3+(aq) + 3 e - → Cr (s) -0.74 V
Which one of the following processes does NOT involve the transfer of energy via work when the reaction is carried out at constant pressure in a vessel open to the atmosphere? - Reaction of nitrogen monoxide gas and oxygen gas to form gaseous nitrogen dioxide. - Decomposition of solid calcium carbonate to solid calcium oxide and carbon dioxide gas. - Conversion of gaseous nitrogen dioxide to gaseous dinitrogen tetroxide. - Reaction of solid copper(II) sulfate and water vapor to form solid copper(II) sulfate pentahydrate. - Combustion of solid sucrose (C12H22O11) in oxygen gas to form carbon dioxide gas and liquid water.
Develop a general equation for the standard heat of reaction as a function of temperature for one of the reactions given in parts (a), (b), (c) a. H2S(g) + 2H2O(g) → 3H2(g) + SO2(g) b. N2(g) + O2(g) → 2NO(g) c. CaCO3(s) → CaO(s) + CO2 (g)
Consider the combustion of liquid methanol, CH3OH(l):CH3OH(l) + 3/2O2(g)----> CO2(g) + 2 H2O(l) ΔH = -726.5 kJ(a) What is the enthalpy change for the reverse reaction?(b) Balance the forward reaction with whole-number coefficients.What is ΔH for the reaction represented by thisequation? (c) Which is more likely to be thermodynamicallyfavored, the forward reaction or the reverse reaction?(d) If the reaction were written to produce H2O(g) insteadof H2O(l), would you expect the magnitude of ΔH to increase,decrease, or stay the same? Explain.
The excessive production of ozone (O3) gas in the lower atmosphere causes rubber to deteriorate, green plants to turn brown, and persons with respiratory disease to have difficulty breathing. The reaction describing the formation of ozone from oxygen is shown below. 3 O2(g) <==> 2 O3(g) Calculate Grxn at 300 K for this reaction in a flask where [O2] = 1.179 x 10-2 M and [O3] = 7.973 x 10-3 M.Assume G° = 326 kJ. Use molarity to construct the reaction quotient, and express your answer in kJ.