One mole of an ideal gas is contained in a cylinder with a movable piston. The temperature is constant at 77°C. Weights are removed suddenly from the piston to give the following sequence of threepressures.a. P, = 4.60 atm (initial state)b. P₂ = 2.73 atmc. P3 1.00 atm (final state)What is the total work (in joules) in going from the initial to the final state by way of the preceding two steps?JWhat would be the total work if the process were carried out reversibly?

One mole of an ideal gas is contained in a cylinder with a movable piston. The temperature is constant at 77°C. Weights are removed suddenly from the piston to give the following sequence of three pressures. a. P₁ = 4.60 atm (initial state) b. P₂ = 2.73 atm c. P3 1.00 atm (final state) What is the total work (in joules) in going from the initial to the final state by way of the preceding two steps? ] What would be the total work if the process were carried out reversibly?

One mole of an ideal gas is contained in a cylinder with a movable piston. The temperature is constant at 77°C. Weights are removed suddenly from the piston to give the following sequence of three pressures. a. P₁ = 4.60 atm (initial state) b. P₂ = 2.73 atm c. P3 1.00 atm (final state) What is the total work (in joules) in going from the initial to the final state by way of the preceding two steps? ] What would be the total work if the process were carried out reversibly?

Chemistry

10th Edition

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Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter6: Thermochemistry

Section: Chapter Questions

Problem 130CP: Consider 2.00 moles of an ideal gas that are taken from state A (PA = 2.00 atm, vA = 10.0 L) to...

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9.11 Analyze the units of the quantity (pressurevolume) and show that they are energy units, consistent with the idea of PV-work.
A bottle of soda has a head space containing 25.0 mL of CO2 gas at 4.2 atm pressure when the soda is at 4.4C. The bottle is opened slowly, letting the excess pressure escape. Howmuch work does the escaping CO2 do if the ambient pressure is 1.0 atm? Assume that the temperature remains constant.
Dry ice is solid carbon dioxide; it vaporizes at room temperature and normal pressures to the gas. Suppose you put 21.5 g of dry ice in a vessel fitted with a piston (similar to the one in Figure 6.9 but with the weight replaced by the atmosphere), and it vaporizes completely to the gas, pushing the piston upward until its pressure and temperature equal those of the surrounding atmosphere at 24.0C and 751 mmHg. Calculate the work done by the gas in expanding against the atmosphere. Neglect the volume of the solid carbon dioxide, which is very small in comparison to the volume of the gas phase.
Coal is used as a fuel in some electric-generating plants. Coal is a complex material, but for simplicity we may consider it to be a form of carbon. The energy that can be derived from a fuel is sometimes compared with the enthalpy of the combustion reaction: C(s)+O2(g)CO2(g) Calculate the standard enthalpy change for this reaction at 25C. Actually, only a fraction of the heat from this reaction is available to produce electric energy. In electric generating plants, this reaction is used to generate heat for a steam engine, which turns the generator. Basically the steam engine is a type of heat engine in which steam enters the engine at high temperature (Th), work is done, and the steam then exits at a lower temperature (Tl). The maximum fraction, f, of heat available to produce useful energy depends on the difference between these temperatures (expressed in kelvins), f = (Th Tl)/Th. What is the maximum heat energy available for useful work from the combustion of 1.00 mol of C(s) to CO2(g)? (Assume the value of H calculated at 25C for the heat obtained in the generator.) It is possible to consider more efficient ways to obtain useful energy from a fuel. For example, methane can be burned in a fuel cell to generate electricity directly. The maximum useful energy obtained in these cases is the maximum work, which equals the free-energy change. Calculate the standard free-energy change for the combustion of 1.00 mol of C(s) to CO2(g). Compare this value with the maximum obtained with the heat engine described here.
The statement Energycan beneithercreatednor destroyedis sometimes used as an equivalent statement of the first law of thermodynamics. There areinaccuracies to the statement, however. Restate it tomake it less inaccurate.
In the reaction of two moles of gaseous hydrogen and one mole of gaseous oxygen to form two moles of gaseous water vapor, two moles of products are formed from three moles of reactants. If this reaction is done at 1.01 104 Pa (and at 0 C), the volume is reduced by 22.4 L. (a) In this reaction, how much work is done on the system (H2, O2, H2O) by the surroundings? (b) The enthalpy change for this reaction is 483.6 kJ. Use this value, along with the answer to (a), to calculate rU, the change in internal energy in the system.
It takes 2260 J to vaporize a gram of liquid water to steam at its normal boiling point of 100C. What is H for this process?What is the work, given that the water vaporexpands against a pressure of 0.988atm? What is U for thisprocess?
Calculate w for the following reactions that occur at 298 K and 1 atm pressure. Consider only PV work from the change in volume of gas, and assume that the gases are ideal and the chemical equation represents amounts in moles. (a) Fe2O3(s) + 2Al(s) 2Fe(s) + Al2O3(s) (b) 2H2(g) + O2(g) 2H2O()
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