A race car on Bonneville flats is operated by a jet engine. The jet fuel isconsumed at a rate of k = 8.76 moving at a constant speed of 298.54relative to the car. The car experiences a resistance of 2kv, where v isthe speed of the car. The initial weight of the car is half car and halffuel. What is the speed of the car at the instant it runs out of fuel?

Step 1:To solve this problem, we'll use Newton's second law of motion, which states that the net…

Answered: A race car on Bonneville flats is…

Physical Chemistry

2nd Edition

ISBN:9781133958437

Author:Ball, David W. (david Warren), BAER, Tomas

Publisher:Ball, David W. (david Warren), BAER, Tomas

Chapter2: The First Law Of Thermodynamics

Section: Chapter Questions

Problem 2.43E

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Similar questions

In the 1880s, Frederick Trouton noted that the enthalpy of vaporization of 1 mol pure liquid is approximately 88 times the boiling point, Tb, of the liquid on the Kelvin scale. This relationship is called Troutons rule and is represented by the thermochemical equation liquid gas H = 88 Tb, joules Combined with an empirical formula from chemical analysis, Troutons rule can be used to find the molecular formula of a compound, as illustrated here. A compound that contains only carbon and hydrogen is 85.6% C and 14.4% H. Its enthalpy of vaporization is 389 J/g, and it boils at a temperature of 322 K. (a) What is the empirical formula of this compound? (b) Use Troutons rule to calculate the approximate enthalpy or vaporization or one mole of the compound. Combine the enthalpy of vaporization per mole with that same quantity per gram to obtain an approximate molar mass of the compound. (c) Use the results of parts (a) and (b) to find the molecular formula of this compound. Remember that the molecular mass must be exactly a whole-number multiple of the empirical formula mass, so considerable rounding may be needed.
The distance between downtown San Francisco and downtown Oakland is 9 miles. However, a car driving between the two points travels 12.3miles. Of these distances, which one is analogous to a state function? Why?
Use the data in Table 2.2 to determine Hp T for Ar at 0C and 1atm. Make any reasonable assumptions necessary.
Why is equation2.37 written interms of CV and Cp and not c-v and c-p ?
Which of the following quantities can be taken to be independent of temperature? independent of pressure? (a) H for a reaction (b) S for a reaction (c) G for a reaction (d) S for a substance
The Dieterici equation of state for one mole of gas is p=RTe-aVRTV-b Where a and b are constants determined experimentally. For NH3g, a = 10.91 atm. L2 and b = 0.0401 L. Plot the pressure of the gas as the volume of 1.00 mol of NH3g expands from 22.4 L to 50.0 L at 273 K, and numerically determine the work done by the gas by measuring the area under the curve.
In the equation w = P V, why is there a negative sign?
Use the data in Table 2.2 to determine PH T for N2 at 50C and 20atm. Make any reasonable assumptions necessary.
Consider 2.00 moles of an ideal gas that are taken from state A (PA = 2.00 atm, vA = 10.0 L) to state B (PB = 1.00 attn, VB = 30.0 L) by two different pathways: These pathways are summarized on the following graph of P versus V: Calculate the work (in units of J) associated with the two pathways. Is work a state function? Explain.
It is the relationship between pressure and volume in the adiabatic processes of an ideal gas, where r is the adiabatic treatment or the relationship between volume and temperature in is given by the relationship e T-なごの TiV =Te V O
A high pressure gas canister bursts. When the debris is cleared, frost is found to have formed on the metal. A scientist decides to use the ideal gas law to find out how much the temperature of the gas changed when the cylinder burst. Why is this approach incorrect? A They don't know the number of moles of the gas. (B) The gas was being stored as a compressed liquid. C The expansion was adiabatic. (D) The expansion was isothermal.
A quantity of gas in a piston cylinder has a volume of 0.475 m3 and a pressure of 200 Pa. The piston compresses the gas to 0.272 m3 in an isothermal (constant-temperature) process. What is the final pressure of the gas?

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